In a combustion reaction, 46.0g of ethanol reacts with 96.0 g of oxygen to produce water and carbon dioxide. If 54.0 g of water is produced, what mass of carbon dioxide is produced?

Final answer:

The formation of a new planetary system involves the condensation of solid particles, accretion and collision of planetesimals, and the formation of protoplanets.

Explanation:

The formation of a new planetary system according to the nebular theory involves several steps. One important step is the condensation of solid particles from the solar nebula, which leads to the formation of planetesimals. The planetesimals then continue to accrete and collide with each other, gradually growing in size. This process eventually results in the formation of protoplanets, which are still in the process of forming into fully developed planets. Therefore, the correct answer is C) repulsion of gaseous masses.

Answer:

Quantity of heat released = -63.1 kJ

Explanation:

Given:

Enthalpy of vaporization of water, ΔHvap = 40.7 kJ/mol

Mass of water, m = 27.9 g

To determine:

The amount of heat (Q) released

Explanation:

The reaction is: H2O(g) ↔ H2O(l)

The amount of heat evolved during condensation which involves a phase transition from vapor to liquid is given as:

[tex]Q = n*\-Delta Hvap[/tex]

n = moles of water

Since this is a condensation process: ΔHcond = -ΔHvap

[tex]Q = \frac{27.9 g}{18 g/mol} * -40.7 kJ/mol = -63.1 kJ[/tex]

Answer:

6.6 moles of CO2 is produced

Explanation:

97 g of C3H8 is equal to 2.2 moles, so we'll use ratio method according to which for 97 g of C3H8 6.6 moles of CO2 is produced

Final answer:

To find the height of a stack of 1000 pennies, multiply the thickness of one penny (1.52mm) by 1000, resulting in a stack 1520mm tall, which is 152 centimeters.

Explanation:

The question concerns how tall a stack of 1000 pennies would be in centimeters. To answer this, we must know the thickness of one penny. If we assume the thickness of a single penny is approximately 1.52mm (0.0598 inches), we can calculate the height of 1000 pennies by multiplying the thickness of one penny by the number of pennies in the stack. Since there are 10 millimeters in 1 centimeter, we'll need to convert millimeters to centimeters.

Here is the calculation:

To find the grams of acetone in the given solution, we can use the formula for molality and calculate the mass of acetone based on the molality, molar mass of acetone, and mass of the solvent.

The mass of the solution is given as 450.0 g and the molality is given as 0.7500 molal. To find the grams of acetone in the solution, we can use the formula for molality:

Molality (m) = moles of solute / mass of solvent (in kg)

Since 0.7500 molal corresponds to 0.7500 mol of acetone per 1 kg of water, we can calculate the mass of acetone by multiplying the molality by the molar mass of acetone and the mass of the solvent:

Mass of acetone = 0.7500 molal * (58.08 g/mol) * (0.4500 kg)

Therefore, there are 22.52 grams of acetone in this amount of solution.

Answer: Option (B) is the correct answer.

Explanation:

Physical properties and changes are defined as the property or changes that does not cause any change in the chemical composition of a substance.

For example, cutting a piece of sodium with knife is a physical change.

Whereas boiling point, density, melting point etc are all physical changes.

On the other hand, changes that bring change in chemical composition of a substance are known as chemical changes.

For example, reactivity, toxicity etc are all chemical changes.

Hence, we can conclude that the statement physical changes can change compounds into elements, is not true regarding physical properties and changes.

Answer: The term is Mass number.

Explanation:

Atomic number is defined as the number of protons or number of electrons present in an atom. It is represented as Z.

Z = Number of protons = Number of electrons

Mass number is defined as the sum of number of protons and neutrons in an atom. It is represented as A.

A = Number of proton + Number of neutrons

Hence, the correct answer is Mass number.

Answer:[tex]4.98\times 10^{23}[/tex] molecules

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 number of moles, we use the equation:

[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}=\frac{76.3g}{92.02g/mol}=0.83 moles[/tex]

1 mole of [tex]N_2O_4[/tex] contains =[tex]6.023\times 10^{23}[/tex] molecules

0.83 moles of [tex]N_2O_4[/tex] contains =[tex]\frac{6.023\times 10^{23}}{1}\times 0.83=4.98\times 10^{23}[/tex] molecules

Thus total number of molecules in 76.3 g of [tex]N_2O_4[/tex] is [tex]4.98\times 10^{23}[/tex] molecules

Taking into account the definition of molar mass and Avogadro's number, 4.99×10²³ molecules are contained in 76.3 g of N₂O₄.

Avogadro's Number or Avogadro's Constant is called the number of particles that make up a substance (usually atoms or molecules) and that can be found in the amount of one mole of said substance. Its value is 6.023×10²³ particles per mole. Avogadro's number applies to any substance.

The molar mass of substance is a property defined as its mass per unit quantity of substance, in other words, molar mass is the amount of mass that a substance contains in one mole.

Being the molar mass of N₂O₄ is 92.02 g/mol, you can apply the following rule of three: If by definition of molar mass 92.02 grams of the compound are contained in 1 mole, 76.3 grams are contained in how many moles?

[tex]amount of moles=\frac{76.3 gramsx1 mole}{92.02 grams}[/tex]

amount of moles= 0.829 moles

Then you can apply the following rule of three: If by definition of Avogadro's number, 1 mole of the compound contains 6.023×10²³ molecules, 0.829 moles contains how many molecules?

amount of molecules= (6.023×10²³ molecules× 0.829 moles)÷ 1 mole

amount of molecules= 4.99×10²³ molecules

Finally, 4.99×10²³ molecules are contained in 76.3 g of N₂O₄.

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Avogadro's Number:

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molar mass:

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A neutralization reaction is a chemical reaction between an acid and a base that results in water and a salt. Option B, HNO3(aq) + LiOH(aq) → H2O(l) + LiNO3(aq), is an example of this as it involves the reaction between an acid (Hydrogen Nitrate) and a base (Lithium Hydroxide) to form water and a salt (Lithium Nitrate).

In chemistry, a neutralization reaction is a type of chemical reaction where an acid and a base react to form a salt and water. Looking at the provided options, the reaction B. HNO3(aq) + LiOH(aq) → H2O(l) + LiNO3(aq) is a neutralization reaction. This is because Hydrogen Nitrate (HNO3) is an acid and Lithium Hydroxide (LiOH) is a base. The result of their interaction is water (H2O) and a salt (LiNO3).

A neutralization reaction is characterized by an acid reacting with a base and forming water and a salt, which is what happens in this reaction. Hence, option B depicts a neutralization reaction.

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From his experiments, Rutherford deduced two main conclusions: first, the majority of an atom's space is empty, and second, the alpha particles' drastic deflections were due to a highly concentrated, positive charge, i.e., the atomic nucleus. The nucleus, according to Rutherford, is 100,000 times smaller than the atom.

Ernest Rutherford, after conducting multiple experimental runs, arrived at two conclusions with respect to the internal structure of atoms:

Rutherford's theory suggested that the nucleus was about 10-15 m in size, which made it 100,000 times smaller than the atom itself. The experiment had a profound impact on the field of Physics, leading Rutherford to propose that nearly all the mass of atoms is concentrated in their nucleus. This revolutionary understanding significantly altered the then-existing atomic model and paved the way for a deeper understanding of atomic structure.

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Answer:

43.7%

Explanation:

Air contains water in a gaseous form called water vapor

In the given neutralization reaction, X would be CH₃COOH.

Let's consider the incomplete reaction below.

NaOH + X ⇒ NaCH₃COO + H₂O

This seems to be a neutralization reaction.

It is a reaction between an acid and a base to form salt and water.

We can identify:

What is X in this reaction?

In the given neutralization reaction, X would be CH₃COOH.

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Answer:

Single-displacement

Explanation:

Answer: The concentration of [tex]K^+[/tex] ions in the solution is 0.09 M

Explanation:

We are given:

Concentration of [tex]K_2CO_3[/tex] = 0.045 M

The chemical equation for complete dissociation of potassium carbonate follows:

[tex]K_2CO_3(aq.)\rightarrow 2K^+(aq.)+CO_3^{2-}(aq.)[/tex]

By stoichiometry of the reaction:

1 mole of potassium carbonate produces 2 moles of potassium ions and 1 mole of carbonate ions.

So, the concentration of potassium ions in the given solution = [tex](2\times 0.045M)=0.09M[/tex]

Hence, the concentration of [tex]K^+[/tex] ions in the solution is 0.09 M

Answer: The number of neutrons in copper-65 are 36.

Explanation:

Atomic number is defined as the number of protons that are present in an atom. It is represented as 'Z'

Z = Atomic number = Number of protons

Atomic mass of an element is defined as the sum of number of neutrons and number of protons that are present in an atom. It is represented as 'A'.

A = Atomic mass = Number of neutrons + Number of protons

For Copper, the atomic number is 29.

We are given:

Atomic mass of copper-65 = 65

Number of neutrons = 65 - 29 = 36

Hence, the number of neutrons in the given isotope of copper are 36.

The molar mass of the gas is approximately [tex]47.56 \text{ g/mol}[/tex]

To calculate the molar mass of the gas, we can use the Ideal Gas Law, which is given by:

[tex]\[ PV = nRT \][/tex]

where:

- [tex]\( P \)[/tex] is the pressure of the gas,

- [tex]\( V \)[/tex] is the volume of the gas,

- [tex]\( n \)[/tex] is the number of moles of the gas,

- [tex]\( R \)[/tex] is the ideal gas constant, and

- [tex]\( T \)[/tex]  is the temperature of the gas in Kelvin.

First, need to convert the temperature from Celsius to Kelvin:

[tex]\[ T(K) = T(\°C) + 273.15 \] \[ T(K) = 24 + 273.15 = 297.15 K \][/tex]

The density [tex]\( \rho \)[/tex] of the gas is given as 1.49 g/L. The density is the mass [tex]\( m \)[/tex] divided by the volume [tex]\( V \)[/tex]:

[tex]\[ \rho = \frac{m}{V} \][/tex]

express the mass in terms of the molar mass [tex]\( M \)[/tex] and the number of moles [tex]\( n \)[/tex]:

[tex]\[ m = M \cdot n \][/tex]

Substituting this into the density equation gives:

[tex]\[ \rho = \frac{M \cdot n}{V} \][/tex]

Now, can rearrange the Ideal Gas Law to solve for [tex]\( n \)[/tex]:

[tex]\[ n = \frac{PV}{RT} \][/tex]

Substituting this expression for [tex]\( n \)[/tex]  into the density equation gives:

[tex]\[ \rho = \frac{M \cdot PV}{RTV} \][/tex]

[tex]\[ \rho = \frac{M \cdot P}{RT} \][/tex]

Now, can solve for the molar mass [tex]\( M \)[/tex]:

[tex]\[ M = \frac{\rho RT}{P} \][/tex]

know that the ideal gas constant [tex]\( R \)[/tex] is 0.0821 L·atm/(mol·K), so we can plug in the values:

[tex]\[ M = \frac{1.49 \text{ g/L} \cdot 0.0821 \text{ L\·atm/(mol\·K)} \cdot 297.15 \text{ K}}{0.787 \text{ atm}} \] \[ M = \frac{1.49 \cdot 0.0821 \cdot 297.15}{0.787} \] \[ M = \frac{37.41}{0.787} \] \[ M \approx 47.56 \text{ g/mol} \][/tex]

Therefore, the molar mass of the gas is approximately 47.56 g/mol.

Answer : The reduction reaction takes place at cathode.

Explanation :

Voltaic cell : It is defined as a device which is used for the conversion of the chemical energy produces in a redox reaction into the electrical energy.

In the voltaic cell, the oxidation occurs at an anode which is a negative electrode and the reduction occurs at the cathode which is a positive electrode.

For example : The redox reaction occurs between the zinc and copper sulfate.

The balanced two-half reactions will be,

Oxidation half reaction (cathode) : [tex]Zn(s)\rightarrow Zn^{2+}(aq)+2e^-[/tex]

Reduction half reaction (anode) : [tex]Cu^{2+}(aq)+2e^-\rightarrow Cu(s)[/tex]

Thus the overall reaction will be,

[tex]Zn(s)+Cu^{2+}(aq)\rightarrow Zn^{2+}(aq)+Cu(s)[/tex]

Hence, the reduction reaction takes place at cathode.