Which of the following pieces of glassware would be best to choose for the following tasks?

For each task, select either the volumetric flask, Erlenmeyer flask, beaker, volumetric pipet, or graduate cylinder and explain why it would be the best choice.

a. Accurately deliver 15.00 mL of solution

b. Heat a reaction mixture on a hot plate

c. Accurately make a diluted solution to four significant figures

d. Approximately deliver 15 mL of solution

Answer:

Goiter.

Explanation:

The thyroid gland is responsible for the secretion of the triidotyronine and thyroxine hormone in the body. The thyroid hormone regulates the metabolism and amount of particular ions in the body.

The iodine acts as the precursor for the maintenance of the thyroxine. The deficiency of the thyroid hormone can cause goiter.  The thyroid gland gets swollen and cause problem in the breathing. The production of mucus and cough is common in goiter.

Thus, the answer is goiter.

Answer:

1.3 × 10³ mL

Explanation:

Let's consider the following reaction.

Zn + 2 HCl → ZnCl₂ + H₂

The percent yield is 78.0%. The real yield (R) of zinc chloride is 35.5 g. The theoretical yield (T) of zinc chloride is:

35.5 g (R) × (100 g T/ 78.0 g R) = 45.5 g T

The molar mass of zinc chloride is 136.29 g/mol. The moles corresponding to 45.5 g of zinc chloride is:

45.5 g × (1 mol/ 136.29 g) = 0.334 mol

The molar ratio of HCl to ZnCl₂ is 2:1. The moles of HCl that react with 0.334 moles of ZnCl₂ are 2 × 0.334 mol = 0.668 mol.

We need 0.668 moles of a 0.50 M HCl solution. The volume required is:

0.668 mol × (1000 mL/0.50 mol) = 1.3 × 10³ mL

Answer:

[H⁺] = 16.6 (±1.9) x10⁻⁴ M

Explanation:

The pH is defined as:

So we can calculate [H⁺]:

[H⁺] = 1.66x10⁻³ M

The relative uncertainty in [H⁺] is

Thus the uncertainty in the concentration is:

1.66x10⁻³ M * 0.115 = 1.91x10⁻⁴ M

Answer:

The balanced chemical reaction is given as:

[tex]C_4H_9OH(l)+6O_2(g)\rightarrow 4CO_2(g)+5H_2O(g)[/tex]

Explanation:

Combustion is defined as chemical reaction which an organic compounds reacts with oxygen gas to to give water and carbon dioxide as a products along with releases of heat energy.

The combustion of liquid butanol gives water vapor and carbon dioxide as a product and this reaction is given as:

[tex]C_4H_9OH(l)+6O_2(g)\rightarrow 4CO_2(g)+5H_2O(g)[/tex]

According to reaction, 1 mole of butanol reacts with 6 moles of oxygen gas to gives 4 moles of carbon dioxide gas and 5 moles of water vapors.

The combustion of liquid butanol, in the presence of oxygen, forms carbon dioxide and water vapor. The balanced chemical equation is: C4H9OH(l) + 6O2(g) → 4CO2(g) + 5H2O(g).

The combustion of liquid butanol (C4H9OH) in the presence of oxygen (O2) produces carbon dioxide (CO2) and water (H2O). The balanced chemical equation for the combustion of liquid butanol can be written as:  

C4H9OH(l) + 6O2(g) → 4CO2(g) + 5H2O(g)

Here, C4H9OH(l) represents liquid butanol, O2(g) represents oxygen gas, CO2(g) represents carbon dioxide gas and H2O(g) represents water vapor. This equation states that one mole of butanol reacts with six moles of oxygen to form four moles of carbon dioxide and five moles of water vapor.

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Answer:

11,547.67 meters of copper can be drawn.

Explanation:

Mass of mineral = 6.95 lb = 6.95 × 453.592 = 3,152.46 g

1 lbs = 453.592 g

An ore of copper is 66.0% copper by mass, So mas of copper in  3,152.46 grams of ore= m

[tex]m = \frac{66.0}{100}\times 3,152.46 g=2080.63 g[/tex]

Volume of copper = V

Density of copper = d = [tex]8.95 /cm^3[/tex]

[tex]V=\frac{m}{d}=\frac{2080.63 g}{8.95 /cm^3}=232.47 cm^3[/tex]

Diameter of the wire drawn from the [tex]232.47 cm^3[/tex] of copper= d

d = [tex]6.304\times 10^{-3} inch=6.304\times 10^{-3}\times 2.54 cm=0.01601 cm[/tex]

(1 inch= 2.54 cm)

Radius of the wire= r = 0.5 ×  d =0.5 × 0.01601 =0.008005 cm

Length of the wire = h

Volume of the cylindrical wire = [tex]\pi r^2 h[/tex]

[tex]V=\pi r^2 h[/tex]

[tex]232.47 cm^3=3.14\times (0.008005 cm)^2\times h[/tex]

Solving for h :

h =1,154,767.015 cm

1 cm = 0.01 m

h = 1,154,767.015 cm = 1,154,767.015× 0.01 m = 11,547.67 m

11,547.67 meters of copper can be drawn.

The temperature represented by a root-mean-square velocity of 1150 m/s for water molecules in a flame is approximately [tex]5.74 \cdot 10^2^4 Kelvin.[/tex]

The temperature represented by a root-mean-square velocity of water molecules can be calculated using the formula:

[tex]\[ v_{rms} = \sqrt{\frac{3kT}{m}} \][/tex]

Where:

- [tex]\( v_{rms} \)[/tex] = root-mean-square velocity of the molecules (1150 m/s in this case)

[tex]\( k \) = Boltzmann constant (1.38 x 10^-23 J/K)\\\( T \) = temperature in Kelvin (what we're trying to find)\\\( m \) = molecular mass of the water (18.0 g/mol or 0.018 kg/mol)[/tex]

Now, we can rearrange the formula to solve for \( T \):

[tex]\[ T = \frac{m v_{rms}^2}{3k} \][/tex]

Substitute the given values:

[tex]\[ T = \frac{0.018 kg/mol \times (1150 m/s)^2}{3 \times 1.38 \times 10^{-23} J/K} \][/tex]

Calculating:

[tex]\[ T = \frac{0.018 \times 1322500}{4.14 \times 10^{-23}} \]\[ T \approx \frac{23745}{4.14 \times 10^{-23}} \]\[ T \approx 5.74 \times 10^{24} K \][/tex]

The temperature represented by a root-mean-square velocity of 1150 m/s for water molecules in a flame is approximately [tex]5.74 \cdot 10^2^4 Kelvin.[/tex]

To calculate the temperature, we used the formula for root-mean-square velocity and rearranged it to solve for temperature. Plugging in the given values, we obtained the temperature in Kelvin. This extremely high temperature result suggests that either the calculation or the assumptions about the system may not be accurate or applicable in a real-world scenario.

Complete Question:

Suppose that the root-mean-square velocity vrms of water molecules (molecular mass is equal to 18.0 g/mol) in a flame is found to be 1150 m/s. What temperature does this represent?

Explanation:

The reaction equation will be as follows.

        [tex]C_{6}H)_{12}O_{6}(s) + 6O_{2}(g) \rightarrow 6CO_{2}(g) + 6H_{2}O(l)[/tex]

It is given that the total energy liberated is -2810 kJ/mol. As the sign is negative this means that energy is being released. Also, it is given that the energy required to synthesis is -64.1 kJ/mol.

Therefore, calculate the number of moles of compound as follows.

         No. of moles = [tex]\frac{\text{total energy}}{\text{energy necessary to synthesise 1 mole of compound X}}[/tex]

                               = [tex]\frac{-2810 kJ}{-64.1 kJ/mol}[/tex]

                               = 43.83 mol

                               = 44 mol (approx)

Thus, we can conclude that the number of moles of compound is 44 mol.

The number of moles of the compound that could theoretically be generated resulting in approximately 44 moles when rounded to two significant figures.

To calculate the number of moles of hypothetical compound X that can be generated from the combustion of one mole of fructose, we use the provided Gibbs free energy change (ΔG°') of fructose and compound X. The energy liberated from the combustion of fructose is given as -2810 kJ/mol, and the energy required to synthesize one mole of compound X is -64.1 kJ/mol.

By dividing the total energy released by combustion by the energy required to synthesize one mole of compound X, we can find out the number of moles of compound X that can be theoretically produced.

Here’s the calculation:

Rounded to two significant figures, the number of moles of compound X that can be theoretically generated is 44 moles.

Answer:

Hi

The Fermi Level is a term used to describe the set of electron energy levels at a temperature of absolute zero. Fermi's energy concept is important for the understanding of the electrical and thermal properties of solids. Both electrical and thermal processes involve energy values of a small fraction of an electron-volt. In thermal equilibrium, the net current of both electrons and holes is zero.

Explanation:

Under equilibrium conditions, the probability of an electron state being occupied if it is located at the Fermi level is 50 percent probability.

Fermi Level is the term that is used to define the highest or most optimal energy level that an electron can occupy when the temperature is at absolute zero.

The Fermi level is equidistant between the valence band and conduction band. This is because when the temperature is at absolute zero, the electrons are all in the lowest state of energy.

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Answer: 1.88times as that of Cl2

Explanation:

According to Graham law of effusion , the rate of effusion is inversely proportional to the square root of the molar mass

Rate= 1/√M

R1/R2 =√M2/M1

Let the rate of diffusion of Ne= R1

And rate of diffusion of Cl2 = R2

M1 ,molar mass of Ne= 20g/mol

M2,molar mass of Cl2 =71g/mol

R1/R2 = √ (71/20)

R1/R2 = 1.88

R1= 1.88R2

Therefore the Ne effuses at rate that is 1.88times than that of Cl2 at the same condition.

Using Graham's law of effusion, Ne gas is found to effuse approximately 1.88 times faster than Cl₂ gas under the same conditions.

This is because the rate of effusion is inversely proportional to the square root of molar mass.

To determine the rate at which Neon (Ne) effuses compared to Chlorine (Cl₂) under the same conditions, we can use Graham's law of effusion. According to Graham's law, the rate of effusion of a gas is inversely proportional to the square root of its molar mass.

The molar mass of Ne is approximately 20 g/mol, and the molar mass of Cl₂ is approximately 71 g/mol. Applying Graham's law:

(Rate of Ne) / (Rate of Cl₂) = [tex]\sqrt{sqrt(Molar mass of Cl_{2} / Molar mass of Ne)}[/tex]

This means Ne gas effuses approximately 1.88 times faster than Cl₂ gas under the same conditions.

The question is incomplete, here is the complete question:

A chemist prepares a solution of mercury(II) iodide [tex](HgI_2)[/tex] by measuring out 0.0122 µmol of mercury(II) iodide into a 400 mL volumetric flask and filling the flask to the mark with water.

Calculate the concentration in mol/L of the chemist's mercury(II) iodide solution. Be sure your answer has the correct number of significant digits.

Answer: The molarity of chemist's mercury (II) iodide solution is [tex]3.05\times 10^{-8}mol/L[/tex]

Explanation:

To calculate the molarity of solution, we use the equation:

[tex]\text{Molarity of the solution}=\frac{\text{Moles of solute}\times 1000}{\text{Volume of solution (in mL)}}[/tex]

We are given:

Moles of mercury (II) iodide = [tex]0.0122\mu mol=0.0122\times 10^{-6}mol[/tex]    (Conversion factor:  [tex]1mol=10^6\mu mol[/tex] )

Volume of solution = 400. mL

Putting values in above equation, we get:

[tex]\text{Molarity of }HgI_2=\frac{0.0122\times 10^{-6}\times 1000}{400.}\\\\\text{Molarity of }HgI_2=3.05\times 10^{-8}mol/L[/tex]

Hence, the molarity of chemist's mercury (II) iodide solution is [tex]3.05\times 10^{-8}mol/L[/tex]

Answer:

1.84 × 10³ N

Explanation:

To determine the weight of the system, we will determine its mass which is equal to the sum of the masses of the plastic tank (8 kg) and the water.

We have 0.18 m³ of water with a density of 1000 kg/m³. Its mass is:

0.18 m³ × 1000 kg/m³ = 180 kg

The mass of the system is 180 kg + 8 kg = 188 kg.

We can find the weight (w) of the system using Newton's second law of motion.

w = m × g = 188 kg × 9.81 m/s² = 1.84 × 10³ N

where

g is the gravity

The weight of the combined system, including the plastic tank and the water, is 180 kg.

The weight of an object depends on its mass and the gravitational force acting on it. To find the weight of the combined system, we need to determine the mass of the plastic tank and the water it contains. The 8-kg plastic tank does not contribute to the weight of the system, but the weight of the water can be calculated using its density.

The volume of the water is given as 0.18 m³, and the density of water is 1000 kg/m³. Multiplying these values together will give us the mass of the water:

Weight of the water = density × volume = 1000 kg/m³ × 0.18 m³ = 180 kg

Therefore, the weight of the combined system, including the plastic tank and the water, is 180 kg.

Answer:

Ratio of rates of effusion of He to Ne is 2.245

Explanation:

According to Graham's law rate of effusion is inversely proportional to square root of molar mass of a gas

So, [tex]\frac{r_{He}}{r_{Ne}}=\sqrt{\frac{M_{Ne}}{M_{He}}}[/tex]

where, [tex]r_{He}[/tex] and [tex]r_{Ne}[/tex] are rate of effusion of He and Ne respectively. [tex]M_{He}[/tex] and [tex]M_{Ne}[/tex] are molar mass of He and Ne respectively.

Molar mass of He = 4.003 g/mol

Molar mass of Ne = 20.18 g/mol

So, [tex]\frac{r_{He}}{r_{Ne}}=\sqrt{\frac{20.18}{4.003}}=2.245[/tex]

So, ratio of rates of effusion of He to Ne is 2.245

Answer:

214 milliliters of KOH needs to be added in 1 litre of 0.784 M acetic acid to make a acetate buffer of 5.31

Explanation:

To solve the problem, let us first use the Henderson-Hasselbalch equation to determine the amount of acetate needed to make a buffer of pH 5.31.

Henderson-Hasselbalch equation:

[tex]pH=pKa + log(\frac{[CH_{3}COO^{-}]}{[CH_{3}COOH]})[/tex]

Here, let us consider the moles of both species instead of the molar concentration, as the volume for both is the same. Also, acetate will be formed by the neutralization of acetic acid, hence the final moles of acetic acid will be the difference of initial moles of acetic acid and the moles of acetate formed. Now the equation becomes as follows:

[tex]pH=pKa + log(\frac{n_{ CH_{3}COO^{-}}}{n_{iCH_{3}COOH}-n_{ CH_{3}COO^{-}}}})[/tex]

From given data

pH = 5.31

pKa = 4.76

n(CH₃COO⁻) = ?

ni(CH₃COOH) = 0.784 mol (initial moles of acetic acid)

Placing the data in the equation, we get:

[tex]5.31=4.76 + log(\frac{n_{ CH_{3}COO^{-}}}{0.784-n_{ CH_{3}COO^{-}}}})\\ \\ n_{ CH_{3}COO^{-}}=10^{5.31-4.76}(0.784-(n_{ CH_{3}COO^{-}}))\\ \\ n_{ CH_{3}COO^{-}}= 2.78 mol-3.55(n_{ CH_{3}COO^{-}})\\ \\ n_{ CH_{3}COO^{-}}= 0.61mol[/tex]

The molar ratio of KOH and CH₃COOH is 1:1, i.e 1 mol of KOH will react with CH₃COOH and give 1 mol of acetate (CH₃COO⁻). Hence, 0.61 mol of KOH will give 0.61 mol of KOH. Now to determine the volume of 2.85 M KOH that contains 0.61 moles:

[tex]M_{KOH} =\frac{n_{KOH} }{V_{KOH} (L)}[/tex]

[tex]2.85=\frac{0.61}{V_{KOH} (L)}\\ \\ V_{KOH} (L)=\frac{0.61}{2.85}\\ \\ V_{KOH}=0.214 litre[/tex]

Finally convert liter into milliliter dividing by 1000 (mL/L)

Volume of KOH required = 214 milliliters

Answer:

Oxygen       35.6 percent

Carbon        60 percent

Hydrogen    4.4 percent

Explanation:

Molecular mass of aspirin[tex](C_9H_8O_4)=180 gm/mol.[/tex]

Mass of carbon in 180 gm of aspirine[tex]=12\times 9=108\ gm.[/tex]

Therefore, percentage of carbon in aspirin is [tex]=\dfrac{108}{180}\times 100=60\ percent.[/tex]

Similarly, mass of hydrogen in 8 gm of aspirine[tex]=1\times 8=8\ gm[/tex].

Hydrogen's percentage in aspirin[tex]=\dfrac{8}{180}\times 100=4.4\ percent.[/tex]

Also, mass of oxygen in aspirin is [tex]=16\times 4=64\ gm.[/tex]

Oxygen's percentage in aspirin[tex]=\dfrac{64}{180}\times 100=35.6\ percent.[/tex]

Hence, this is the required solution.

Final answer:

The percent composition of aspirin (C9H8O4) is calculated based on its molecular mass of 180.15 amu. It is 60.03% carbon, 4.48% hydrogen, and 35.49% oxygen.

Explanation:

To determine the percent composition of aspirin, which has the molecular formula C9H8O4, we need to calculate the percentage of each element in the compound based on its molecular mass. The molecular mass of aspirin is 180.15 amu. This is calculated by adding the masses of nine carbon (C) atoms, eight hydrogen (H) atoms, and four oxygen (O) atoms together.

To find the percent composition, we first calculate the total mass of each type of atom in one molecule of aspirin and then divide it by the molecular mass of aspirin. To express it as a percentage, we multiply by 100%. The atomic masses are approximately 12.01 amu for carbon, 1.008 amu for hydrogen, and 16.00 amu for oxygen.

The calculations for percent composition are as follows:

Therefore, the percent composition of aspirin (C9H8O4) is 60.03% carbon, 4.48% hydrogen, and 35.49% oxygen.

Answer:

a. 3MnO2 + 4Al —> 3Mn+ 2Al2O3

3 moles of MnO2 required 4 moles of Al to produce 3 moles of Mn and 2moles of 2Al2O3

b. B203 + 3CaF2 —> 2BF3 + 3CaO

1mole of B203 requires 3 moles of CaF2 to produce 2moles of BF3 and 3 moles of CaO

c. 3NO2 + H2O —> 2HNO3 + NO

3 moles of NO2 requires 1mole of H2O to produce 2moles of HNO3 and 1mole of NO

d. C6H6 + 3H2 —> C6H12

1mole of C6H6 requires 3 moles of H2 to produce 1mole of C6H12

Final answer:

To balance the equations, ensure there are equal numbers of each atom. The balanced equations and their meanings in terms of molecules and moles are...

Explanation:

In order to balance the equations, you need to ensure that there are equal numbers of each type of atom on both sides of the equation. Here are the balanced equations for each reaction:

a. MnO2(s) + 2Al(s) -> Mn(s) + Al2O3(s)

b. B2O3(s) + 3CaF2(s) -> 2BF3(g) + 3CaO(s)

c. 2NO2(g) + H2O(l) -> HNO2(aq) + NO(g)

d. C6H6(g) + 3H2(g) -> C6H12(g)

In terms of the number of individual molecules, the balanced equation shows the ratio in which the reactants combine to form the products. In terms of moles of molecules, the balanced equation allows you to calculate the amount of each substance involved in the reaction using the mole ratio.

Complete Question:

If heat is added to ice and liquid water in a closed container and after the addition of the heat, ice and liquid water remain, (A) the vapor pressure of the water will decrease. (B) the temperature will increase somewhat. (C) the temperature will decrease somewhat. (D) the vapor pressure of the water will remain constant.

Answer:

A

Explanation:

When heat is added to a system, the internal energy of the molecules increases, and they become more agitated, because of that the temperature intends to increase. But when exists a liquid-vapor equilibrium this increase of temperature may be balanced by the vapor pressure.

The vapor pressure is the pressure that the vapor does when it is in equilibrium with the liquid. So, as higher is it, as easy it will be to the liquid to evaporate. When the temperature increases more liquid will evaporate, because the molecules are more agitated, and so the vapor pressure must increase.

But, if the ice and liquid remain, it indicates that no liquid was evaporated, so, the pressure decreased, to avoid the effect of the temperature, which will remain constant.

Answer:

Partial pressure N₂ . (Partial pressure H₂O)² / (Partial pressure H₂)² . (Partial pressure NO)² = Kp

Explanation:

The reaction is:

2NO + 2H₂ → N₂ + 2H₂O

The expression for Kp (pressure equilibrium constant) would be:

Partial pressure N₂ . (Partial pressure H₂O)² / (Partial pressure H₂)² . (Partial pressure NO)²

There is another expression for Kp, where you work with Kc (equilibrium constant)

Kp = Kc (R.T)^Δn

where R is the Ideal Gases constant

T° is absolute temperature

Δn = moles of gases formed - moles of gases, I had initially

The pressure equilibrium constant expression for the reaction 2NO + 2H2 -> N2 + 2H2O is Kp = (p(N2))^1 * (p(H2O))^2 / (p(NO))^2 * (p(H2))^2.

The pressure equilibrium constant expression is defined as the ratio of the product of the partial pressures of the products raised to their stoichiometric coefficients divided by the product of the partial pressures of the reactants raised to their stoichiometric coefficients.

For the reaction 2NO + 2H2 -> N2 + 2H2O, the pressure equilibrium constant expression can be written as:

Kp = (p(N2))^1 * (p(H2O))^2 / (p(NO))^2 * (p(H2))^2

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Answer:

See picture below

Explanation:

To do this, we first need to know how are the bonds in this molecule are. To do so, let's calculate the number of insaturations in the molecule:

n°I = C+1 - (H-N+X)/2

These numbers indicate if the molecule has double bond, triple bond, ring, cyclo, among other options:

n°I = 3 - (3+1)/2

n°I = 1

As it's a very small molecule, we can assume this molecule only have a double bond, and it's an alkene.

So the lewis structure, shows the electrons and the bonding, and also shows the unshared electron pairs, depending on how much electron have each molecule.

In the case of carbon:

[C] = [He] 2s2 2p2 ----> 4 electrons

[H] = 1s1 ----> 1 electron

[Cl] = [Ne] 3s2 3p5 ----> 7 electrons.

Therefore, we also know that Carbon has a double bond, so, the main molecule would have something like this:

C = C

so next to the carbons, we can put two hydrogens and in the other carbon, the chlorine and the remaining hydrogen.

See picture below for structure:

The Lewis structure of C₂H₃Cl is attached in the image below.

Lewis structures are also known as Lewis dot structures or electron dot structures. They are diagrams that represent the arrangement of atoms and valence electrons in a molecule or ion.

In a Lewis structure, the symbol of each atom is used to represent the nucleus and inner-shell electrons, while dots or lines are used to represent the valence electrons. Valence electrons are the outermost electrons involved in bonding and determining the chemical properties of an atom. The image is attached below.

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Answer:

[tex]C_6H_{12}O_6[/tex]

Explanation:

Mass of water obtained = 0.0609 g

Molar mass of water = 18 g/mol

Moles of [tex]H_2O[/tex] = 0.0609 g /18 g/mol = 0.00338 moles

2 moles of hydrogen atoms are present in 1 mole of water. So,

Moles of H = 2 x 0.00338 = 0.00676 moles

Molar mass of H atom = 1.008 g/mol

Mass of H in molecule = 0.00676 x 1.008 = 0.00681 g

Mass of carbon dioxide obtained = 0.1486 g

Molar mass of carbon dioxide = 44.01 g/mol

Moles of [tex]CO_2[/tex] = 0.1486 g  /44.01 g/mol = 0.00337 moles

1 mole of carbon atoms are present in 1 mole of carbon dioxide. So,

Moles of C = 0.00337 moles

Molar mass of C atom = 12.0107 g/mol

Mass of C in molecule = 0.00337 x 12.0107 = 0.04047 g

Given that the compound only contains hydrogen, oxygen and carbon. So,

Mass of O in the sample = Total mass - Mass of C  - Mass of H

Mass of the sample = 0.1014 g

Mass of O in sample = 0.1014 - 0.04047 - 0.00681 = 0.05412 g  

Molar mass of O = 15.999 g/mol

Moles of O  = 0.05412  / 15.999  = 0.00338 moles

Taking the simplest ratio for H, O and C as:

0.00676 : 0.00338 : 0.00337

= 2 : 1 : 1

The empirical formula is = [tex]CH_2O[/tex]

Molecular formulas is the actual number of atoms of each element in the compound while empirical formulas is the simplest or reduced ratio of the elements in the compound.

Thus,  

Molecular mass = n × Empirical mass

Where, n is any positive number from 1, 2, 3...

Mass from the Empirical formula = 1×12 + 2×1 + 16= 30 g/mol

Molar mass = 180 g/mol

So,  

Molecular mass = n × Empirical mass

180 = n × 30

⇒ n = 6

The formula of compound = [tex]C_6H_{12}O_6[/tex]

Final answer:

The molecular formula of the compound is (CHO)6.

Explanation:

To determine the molecular formula of the compound, we need to find the empirical formula first. We can do this by finding the moles of carbon and hydrogen in the sample using the masses of CO2 and H2O produced.

Mass of CO2 = 0.1486 g
Mass of H2O = 0.0609 g

Now, we need to convert the masses of CO2 and H2O to moles and divide by the smallest value to find the ratio of moles of carbon to hydrogen.

After finding the ratio, we multiply it by a common factor to get whole numbers. In this case, the ratio is 1:1, so the empirical formula is CHO.

The empirical formula has a molar mass of 30 g/mol.

To find the molecular formula, we divide the given molar mass of 180 g/mol by the empirical formula molar mass. The result is 6, which means the molecular formula is (CHO)6.

Answer:

∴ wt% CCl4 = 50.597 %

∴ wt% C9H10 = 46.541 %

∴ wt% C9H12 = 2.861 %

Explanation:

⇒ mass sln = 71.1 g CCl4 + 65.4 C9H10 + 4.02 g C9H12

⇒ mass sln = 140.52 g

∴ CCl4:

⇒ wt% CCl4 = ((71.1 g CCl4)/(140.82 g sln))×100

⇒ wt% CCl4 = 50.597 %

∴ C9H10:

⇒ wt% C9H10 = ((65.4 g C9H10)/(140.52 g sln))×100

⇒ wt% C9H10 = 46.541 %

∴ C9H12:

⇒ wt% C9H12 = ((4.02 g C9H12)/(140.52 g sln))×100

⇒ wt% C9H12 = 2.861 %

The percent by mass of each component in the solution is calculated by dividing each component's mass by the total mass and multiplying by 100. The results are 50.62% for carbon tetrachloride, 46.53% for isopropenylbenzene, and 2.86% for 2-ethyltoluene.

In order to calculate the percent by mass of each component of the solution, the total mass of the solution needs to be determined first. The total mass would be obtained by summing the individual masses of the carbon tetrachloride, isopropenylbenzene, and 2-ethyltoluene. That is, 71.1 g + 65.4 g + 4.02 g = 140.52 g.

Then, the mass of each component is divided by the total mass and multiplied by 100 to obtain the percentage.

Our three significant figures in each of the percentages are due to the fact that our least precise measurement, 4.02 g of 2-ethyltoluene, has four significant figures.

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Answer: 8.7 grams

Explanation:

According to avogadro's law, 1 mole of every substance occupies 22.4 L at STP and contains avogadro's number [tex]6.023\times 10^{23}[/tex] of particles.  

To calculate the moles, we use the equation:

[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text {Molar mass}}=\frac{4.6g}{27g/mol}=0.17moles[/tex]

[tex]4Al(s)+3O_2(g)\rightarrow 2Al_2O_3(s)[/tex]

As oxygen is in excess, Aluminium is the limiting reagent and limits the formation of products.

According to stoichiometry:

4 moles of aluminium give = 2 moles of [tex]Al_2O_3(s)[/tex]

Thus 0.17 moles of aluminium give=[tex]\frac{2}{4}\times 0.17=0.085mol[/tex]

Mass of [tex]Al_2O_3=moles\times {\text {molar mass}}=0.085\times 102g/mol=8.7g[/tex]

Thus the mass of [tex]Al_2O_3(s)[/tex]  is 8.7 grams

Answer:

The increasing order of masses of molecule ions:

118 g/mol(75.8%) ,  120 g/mol(24.2%)

Explanation:

Chlorine occurs as 35-Cl (75.8%) and 37-Cl (24.2%).

Atomic mass of 35-Cl = 35 g/mol

Atomic mass of 37-Cl = 37 g/mol

Mass of Chlorocyclohexane in which 35-cl is present as a chlorine atom: [tex]C_6H_{11}Cl[/tex]

[tex]=6\times 12 g/mol+11\times 1 g/mol+1\times 35 g/mol=118 g/mol[/tex]

Mass of Chlorocyclohexane in which 37-Cl is present as a chlorine atom: [tex]C_6H_{11}Cl[/tex]

[tex]=6\times 12 g/mol+11\times 1 g/mol+1\times 37 g/mol=120 g/mol[/tex]

The increasing order of masses of molecule ions:

118 g/mol(75.8%) < 120 g/mol(24.2%)

Answer:

Side products coincides with a loss in percentage yield of the product

Explanation:

- The product yield is defined as

product yield= actual yield/theoretical yield

- Byproducts are undesired products that come from the same reaction pathway that our products → even if the reaction procedes ideally , we will always have byproducts → byproducts do not alter the Yield by themselves

- Side products , however , come from undesired products from side reactions  and consume reactants due to these alternative pathways without producing our product → side products do alter the yield of the product

The mass of HCl that is contained in the solution is 147 g HCl

Why?

To find the mass of HCl we have to apply what is called a conversion factor. In a conversion factor we put the units we don't want at the bottom, and the ones we want at the top.

For this question, we want to go from liters of solution to mass of HCl, and the conversion factor is laid out as follows:

[tex]0.356Lsolution*\frac{1000mL}{1L}*\frac{1.19 g solution}{1 mL solution}*\frac{34.70 g HCl}{100 g solution}=147 g HCl[/tex]

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Explanation:

For a compound to show hydrogen bonding it is necessary that the hydrogen atom of the compound should be attached to more electronegative atom like fluorine, oxygen or nitrogen.

For example, [tex]CH_{3}CH_{2}OH[/tex], [tex]CH_{3}NH_{2}[/tex] and [tex]NH_{3}[/tex] all these compounds contain an electronegative atom attached to hydrogen atom.

Therefore, these pure compounds will exhibit hydrogen bonding.

Thus, we can conclude that out of the given options [tex]CH_{3}CH_{2}OH[/tex], [tex]CH_{3}NH_{2}[/tex] and [tex]NH_{3}[/tex] are the pure compounds which will exhibit hydrogen bonding.

Answer:

The melting point would be 250. That is the answer I think

Explanation:

The solid substance will turn into vapor when the temperature is increased from room temperature into meeting point temperature.

The given parameters;

A substance boils when the atmospheric pressure is equal to the vapor pressure.

Since the vapor pressure of the solid substance occurs at the meeting temperature of the substance, once the temperature of the solid substance is increased to the meeting point temperature, the solid substance will turn into vapor (gas).

Thus, we can conclude that the solid substance will turn into vapor when the temperature is increased from room temperature into meeting point temperature.

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The given question is lacking some details, the complete question is following

Question:

An aqueous solution at 25 °C has a OH⁻ concentration of 2.5 x 10⁻⁴ M . Calculate the H₃O⁺ concentration. Be sure your answer has the correct number of significant digits

Answer:

Concentration of H₃O⁺ is:

[tex][H_{3}O^{+}]=4.0X10^{-9} M[/tex]

Explanation:

In aqueous solutions the product of the concentration of hydronium ions H₃O⁺ and hydroxide ions OH⁻ is 1.0 x 10⁻¹⁴. This value is the dissociation or ionization constant of water at 25 °C. Its formula is given as:

[tex]Kw = [H_{3} O^{+}][OH^{-} ][/tex]

[tex]1.0 X 10^{-14}= [H_{3}O^{+}](2.5 X 10^{-4})[/tex]

[tex][H_{3}O^{+}]= \frac{1.0X10^{-14}}{2.5 X 10^{-4}}[/tex]

[tex][H_{3}O^{+}]=4.0X10^{-9} M[/tex]

P.S: As the smallest number of significant figure in the ratio was two, so the answer contains two significant figures.

To calculate the hydronium ion concentration from the hydroxide ion concentration of 0.001 M at 25 °C, use the water ion-product constant, Kw (1.0 × 10^-14), and the inverse relationship between [H3O+] and [OH-] to find [H3O+] = 1.0 × 10^-11 M.

To calculate the hydronium ion concentration in an aqueous solution with a hydroxide ion concentration of 0.001 M at 25 °C, we use the ion-product constant for water (Kw), which is 1.0 × 10-14 at 25 °C. The concentration of hydronium ions [H3O+] and hydroxide ions [OH-] are inversely proportional, which means as the concentration of one goes up, the other goes down. Therefore, the calculation for the hydronium ion concentration can be done using the equation:

Kw = [H3O+] × [OH-]

Substituting in the values we have:

1.0 × 10-14 = [H3O+] × 0.001

Therefore, the concentration of hydronium ions [H3O+] is:

[H3O+] = ⅖{1.0 × 10-14}{0.001}

[H3O+] = 1.0 × 10-11 M

Make sure that your final answer has the correct number of significant figures, which is guided by the number of significant figures in the given hydroxide ion concentration (0.001 M has one significant figure).

Answer:

5.3 × 10⁻³ kg

Explanation:

There is some info missing. I think this is the original question.

A chemist adds 135.0 mL of a 0.21 M zinc nitrate (Zn(NO₃)₂) solution to a reaction flask. Calculate the mass in kilograms of zinc nitrate the chemist has added to the flask. Be sure your answer has the correct number of significant digits.

We have 135.0 mL of a 0.21 M zinc nitrate (Zn(NO₃)₂) solution. The moles of zinc nitrate are:

0.1350 L × 0.21 mol/L = 2.8 × 10⁻² mol

The molar mass of zinc nitrate is 189.36 g/mol. The mass corresponding to 2.8 × 10⁻² moles is:

2.8 × 10⁻² mol × 189.36 g/mol = 5.3 g

1 kilogram is equal to 1000 grams. Then,

5.3 g × (1 kg/1000 g) = 5.3 × 10⁻³ kg

Answer: noble gases are in reactive.

Explanation: noble gases are present in the right most corner of the periodic table in the 8th group. So their outermost shells are complete. Their boiling point, mass increases down the group. the have strong forces of interaction. their ionization energy decreases down the group

Explanation:

Apple cider vinegar or balsamic vinegar might contain various synthetics which might  interact with or nullified the findings, whereas white vinegar comprises of acidic acid only. In fact, apple cider vinegar and balsamic vinegar are deep in appearance this would make it very difficult to determine the color. This is why it is preferable to use white vinegar in the Titration process.

The challenge that would be encountered with the titration if you had used balsamic vinegar as an analyte is the inability to determine the endpoint of the titration with your naked eye.

An analyte, also known as a titrand is a solution whose concentration is needed to be determined. During titration, it will be difficult and impossible to determine the endpoint of titration because it will be difficult to catch the color changes with visible eyes.

To eliminate this difficulty, balsamic vinegar needs to be diluted with enough water to detect the color change, or the use of white vinegar is used.

Similarly, apple cider, as well as balsamic vinegar, comprises additional acid than acetic acid, this will increase the level of acidity during the titration, unlike white vinegar that contains only acetic acid.

Thus, the acid in apple cider vinegar or balsamic vinegar will be more and higher during titration compared to that of white vinegar.

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