What is the electron configuration of an element with atomic number 20?

We see that in 1 rock, there are 31 atoms of Argon and 1 atom of Potassium so the relative concentration of Potassium is:

1 / 32

or can be written as:

1 / 2^5

So this means that 5 half-lives have passed.

So the years are:

years passed = 5 * 1.25 billion years = 6.25 billion years

Answer:

1.3 billion years

Explanation:

Answer;

6CO2 + 18ATP + 12 NADPH → C6H12O6 + 18ATP + 18Pi + 12NADP+

Explanation;

-The process of Calvin Cycle Synthesizes Hexoses from Carbon Dioxide and Water.

-The ATP and NADPH molecules produced by the light-dependent reactions of photosynthesis power sugar synthesis in the Calvin cycle. In the Calvin cycle, three molecules of CO2 are added to three molecules of ribulose bisphosphate (RuBP), a 5-carbon sugar already present in the stroma.

-This results to a total of eighteen carbons in the cycle.  As the three RuBP molecules accept a molecule of carbon dioxide, they immediately break down into six 3-carbon molecules of phosphoglyceric acid which is a hexose.

Answer:

Ca and Br

Explanation:

i took an online test and this was the answer

A salt is formed when a metal combines with a nonmetal hence the pair that will form a salt is Ca and Br.

A salt is an ionic substance. An ionic substance is formed when a metal donates an electron to a nonmetal in an ionic bond. Hence, we must look out for the pair that consists of a metal and a nonmetal.

Closely examining the options, we can see that only the pair involving Ca and Br is comprised of a metal and a nonmetal hence they can form a salt.

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Answer:

Gravitational force will increase with greater mass

The volume of balloon at 1.0 atmis [tex]\boxed{9.68{\text{ L}}}[/tex].

Further Explanation:

A hypothetical gas comprising of a large number of randomly moving particles is called ideal gas. The collisions between such particles are considered to be perfectly elastic. Practically, no gas can be ideal so it is just a theoretical concept.

Given information:

Volume of balloon at 2.2 atm: 4.4 L

To determine:

Volume of balloon at 1.0 atm

Boyle’s law:

This law describes relationship between volume and pressure of gas. According to this law,volume of the gas is inversely proportional to its pressure, provided the temperature and the number of moles of gas remain constant. Mathematical form of Boyle’s law is,

[tex]{\text{P}} \propto \dfrac{1}{{\text{V}}}[/tex]  

Or,

[tex]{\text{PV}} = {\text{k}}[/tex]  

Where,

V is volume occupied by the gas.

P is the pressure of the gas.

k is a constant.

At two volumes [tex]{{\text{V}}_{\text{1}}}[/tex] and [tex]{{\text{V}}_{\text{2}}}[/tex] andpressures [tex]{{\text{P}}_{\text{1}}}[/tex] and [tex]{{\text{P}}_{\text{2}}}[/tex], equation of Boyle’s law modifies as follows:

[tex]{{\text{P}}_1}{{\text{V}}_1} = {{\text{P}}_2}{{\text{V}}_2}[/tex]                                                        …… (1)

Rearrange equation (1) to calculate [tex]{{\text{V}}_{\text{2}}}[/tex].

[tex]{{\text{V}}_2} = \dfrac{{{{\text{P}}_1}{{\text{V}}_1}}}{{{{\text{P}}_2}}}[/tex]                                                            …… (2)

Substitute 4.4 L for [tex]{{\text{V}}_{\text{1}}}[/tex] , 2.2 atm for [tex]{{\text{P}}_{\text{1}}}[/tex] and 1.0 atm for [tex]{{\text{P}}_{\text{2}}}[/tex] in equation (2).

[tex]\begin{aligned}{{\text{V}}_2} &= \frac{{\left( {2.2{\text{ atm}}} \right)\left( {4.4{\text{ L}}} \right)}}{{\left( {{\text{1}}{\text{.0 atm}}} \right)}} \\&= 9.68{\text{ L}} \\\end{aligned}[/tex]  

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Answer details:

Grade: Senior School

Subject: Chemistry

Chapter: Ideal gas equation

Keywords: Boyle’s law, P, V, k, pressure of gas, volume occupied by gas, constant, temperature, ideal gas, 2.2 atm, 1.0 atm, 4.4 L, 9.68 L.

the maximum electrical work that the cell can accomplish when 51.0 g of copper is plated out is approximately [tex]\( -167549 \, \text{J} \).[/tex]

To find the maximum electrical work that the cell can accomplish when 51.0 g of copper is plated out, we can use the relationship between electrical work ( w ) and the amount of substance involved in the redox reaction.

The electrical work ( w ) done by a cell operating under standard conditions is given by:

[tex]\[ w = -nFE \][/tex]

Where:

- ( n ) is the number of moles of electrons transferred in the balanced redox reaction.

- ( F ) is the Faraday constant [tex](\( 96485 \, \text{C/mol} \)).[/tex]

- ( E ) is the standard cell potential of the redox reaction (in volts).

First, we need to determine the number of moles of electrons transferred in the reaction. From the balanced redox reaction:

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

We see that 2 moles of electrons are transferred for every 1 mole of copper plated out.

Given that the molar mass of copper ([tex]\( \text{Cu} \))[/tex] is approximately [tex]\( 63.55 \, \text{g/mol} \)[/tex], we can calculate the number of moles of copper plated out:

[tex]\[ \text{Moles of Cu} = \frac{\text{Mass}}{\text{Molar mass}} = \frac{51.0 \, \text{g}}{63.55 \, \text{g/mol}} \][/tex]

[tex]\[ \text{Moles of Cu} \approx 0.802 \, \text{mol} \][/tex]

Since 2 moles of electrons are transferred for every 1 mole of copper plated out, the number of moles of electrons transferred (\( n \)) is twice the number of moles of copper plated out:

[tex]\[ n = 2 \times 0.802 \, \text{mol} \][/tex]

[tex]\[ n = 1.604 \, \text{mol} \][/tex]

Now, we can use the standard reduction potentials to find the standard cell potential (E ) for the reaction. From the standard reduction potentials table, we have:

[tex]\[ E^\circ_{\text{cell}} = E^\circ_{\text{cathode}} - E^\circ_{\text{anode}} \][/tex]

[tex]\[ E^\circ_{\text{cell}} = E^\circ_{\text{Cu}^{2+}/\text{Cu}} - E^\circ_{\text{Zn}^{2+}/\text{Zn}} \][/tex]

Given that [tex]\( E^\circ_{\text{Cu}^{2+}/\text{Cu}} = 0.34 \, \text{V} \) and \( E^\circ_{\text{Zn}^{2+}/\text{Zn}} = -0.76 \, \text{V} \)[/tex], we have:

[tex]\[ E^\circ_{\text{cell}} = (0.34 \, \text{V}) - (-0.76 \, \text{V}) \][/tex]

[tex]\[ E^\circ_{\text{cell}} = 1.10 \, \text{V} \][/tex]

Now, we can calculate the maximum electrical work [tex](\( w \)):[/tex]

[tex]\[ w = -nFE \][/tex]

[tex]\[ w = -(1.604 \, \text{mol} \times 96485 \, \text{C/mol} \times 1.10 \, \text{V}) \][/tex]

[tex]\[ w \approx -1.604 \times 96485 \times 1.10 \, \text{J} \][/tex]

[tex]\[ w \approx -167548.6 \, \text{J} \][/tex]

[tex]\[ w \approx -167549 \, \text{J} \][/tex]

So, the maximum electrical work that the cell can accomplish when 51.0 g of copper is plated out is approximately [tex]\( -167549 \, \text{J} \).[/tex]

The electron is the subatomic particle that is specifically responsible for combining atoms together to form a new substance. It does this through chemical bonding, where the outer shell electrons of atoms interact with each other. This process forms the basis of all matter in the universe.

In the formation of substances, the subatomic particle that is specifically responsible for combining atoms together is the electron. In chemical bonds, it's the exterior electrons of the atoms that interact and form these bonds. For instance, in the formation of a molecule of water (H₂O), two hydrogen atoms and one oxygen atom bond together, facilitated by the interactions of their electrons.

Atoms are the fundamental building blocks of matter, made up of different subatomic particles, namely electrons, protons, and neutrons. The atom is regarded as the smallest unit of an element that carries the properties of that element. However, it's the electrons in the outer shell of an atom that play an integral role in the formation of different substances via chemical bonding.

These chemical bonds are the basis for all matter in the universe, ranging from the ionic lattice structure of NaCl (common salt) to covalent molecular structures like proteins and sugars found in living organisms. Therefore, comprehending the role of electrons in the atomic construction of matter is key to understanding the vast array of chemical phenomena that occur in our universe.

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The enthalpy of formation of liquid ethanol (C2H5OH) is represented by the chemical equation combining carbon (solid), hydrogen gas, and oxygen gas to form ethanol.

The enthalpy of formation of liquid ethanol (C2H5OH) can be represented by the balanced chemical equation showing its formation from its elements in their standard states.

The equation is as follows:

C(s) + 3H2(g) + 1/2O2(g) → C2H5OH(l)

The enthalpy change for this reaction is -277.6 kJ/mol, indicating that the formation of liquid ethanol from its elements is exothermic.

Answer:

evaporation

Explanation:

Evaporation is the process where a liquid, in this case water, changes from its liquid state to a gaseous state. Liquid water becomes water vapor. Although lower air pressure helps promote evaporation, temperature is the primary factor.

The answer is: oil.

Synfuel (synthetic fuel) is a liquid fuel, rarely gaseous fuel, made from syngas.

Syngas is a mixture of carbon monoxide (CO) and hydrogen (H₂).

Syngas goes to additional conversion process to become liquid fuel.

Some methods for manufacturing synthetic fuels are methanol (CH₃OH) to gasoline conversion and direct coal liquefaction.

Crystal formation form many metals results into combining of many molecular orbitals during formation.

This is because each metallic atomic orbital contributes for the formation of crystal.

When compared with the relative energies of the molecular orbitals it was found that they have lower energy than the atomic orbitals. Thus the new crystals are stable in nature.

Final answer:

Reduction of D-gulose typically produces D-gulitol (sorbose alcohol), a sugar alcohol. This reaction is analogous to the reduction of D-glucose to sorbitol, involving conversion of the aldehyde group to an alcohol.

Explanation:

The student asked about the product formed by the reduction of D-gulose. D-Gulose, an aldose sugar, can undergo reduction to yield a sugar alcohol, similar to how D-glucose can be reduced to sorbitol. In the case of D-gulose, the reduction typically would produce D-gulitol, also known as sorbose alcohol.

The reducing sugar characteristic mentioned in reference to lactose is due to the presence of a free aldehyde group or an equivalent group in cyclic forms that can act as a reducing agent, for instance in Fehling's solution or Tollen's reagent reactions. This is relevant because the reduction of D-gulose would involve the conversion of its aldehyde group to an alcohol.

1. **Convert the mass of A to moles:**

  - [tex]\(29.5 \, \text{g}\)[/tex] of A is approximately [tex]\(1.88 \, \text{mol}\)[/tex].

2. **Convert the number of moles of A to the number of moles of B:**

  - [tex]\(1.88 \, \text{mol}\)[/tex] of A corresponds to approximately [tex]\(2.82 \, \text{mol}\)[/tex] of B.

3. **Convert the number of moles of B to the molecules of B:**

  - [tex]\(2.82 \, \text{mol}\)[/tex] of B is approximately [tex]\(1.70 \times 10^{24}\)[/tex] molecules.

**Convert the mass of A to moles:**

The first step is to convert the mass of substance A to moles using its molar mass. The formula for moles [tex](\(n\))[/tex] is given by the mass [tex](\(m\))[/tex] divided by the molar mass [tex](\(M\)):[/tex]

[tex]\[ n_A = \frac{m_A}{M_A} \][/tex]

Given that the mass of substance A [tex](\(m_A\))[/tex] is 29.5 g and its molar mass [tex](\(M_A\))[/tex] is 15.7 g/mol:

[tex]\[ n_A = \frac{29.5 \, \text{g}}{15.7 \, \text{g/mol}} \approx 1.88 \, \text{mol} \][/tex]

**Convert the number of moles of A to the number of moles of B:**

The reaction ratio states that 2 moles of A produce 3 moles of B. Therefore, if [tex]\(n_A\)[/tex] is 1.88 mol, the corresponding moles of B [tex](\(n_B\))[/tex] can be calculated using the ratio:

[tex]\[ n_B = \frac{3}{2} \times n_A \][/tex]

[tex]\[ n_B = \frac{3}{2} \times 1.88 \, \text{mol} \approx 2.82 \, \text{mol} \][/tex]

**Convert the number of moles of B to the molecules of B:**

To convert moles of B to molecules [tex](\(N_B\))[/tex], you use Avogadro's number [tex](\(6.022 \times 10^{23}\) mol\(^{-1}\)):[/tex]

[tex]\[ N_B = n_B \times N_A \][/tex]

[tex]\[ N_B = 2.82 \, \text{mol} \times (6.022 \times 10^{23} \, \text{mol}^{-1}) \approx 1.70 \times 10^{24} \, \text{molecules} \][/tex]

The question probable may be:

In a chemical reaction, exactly 2 mol of substance A react to produce exactly 3 mol of substance B.

How many molecules of substance B are produced when 29.5 g of substance A reacts? The molar mass of substance A is 15.7 g/mol.

Convert the mass of A to moles

Convert the number of moles of A to the number of moles of B

Convert the number of moles of B to the molecules of B

Evaporation is an endothermic process that requires the absorption of heat to occur, typically resulting in a perceived cooling effect. However, it is not inherently a cooling or warming process, nor is it an exothermic process.

Evaporation is an endothermic process, meaning it requires an input of heat to occur. The heat energy is used to overcome intermolecular attractions, allowing matter to change from one physical state to another. This is why when you leave a swimming pool or when you sweat, you feel cool. The process of evaporation absorbs heat from your body.

However, it's important to note that evaporation is not always a cooling process. While evaporation takes heat from the source, it doesn't inherently reduce the temperature of the source, the perceived cooling is due to the loss of heat. Also, evaporation is not a warming process, or an exothermic process, as it doesn't produce heat. In fact, the reverse process of evaporation - condensation - is exothermic, releasing heat as matter changes state.

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Answer:

350g dextrose

Explanation:

To calculate how many g of dextrose are in 500ml of solution we have to know the following:

When we talk about x% m/v (mass / volume) it means that there are x grams of solute in 100 ml of solution. Then 70% means that there is 70g of dextrose per 100ml of solution.

To solve this we can say that if in 100 ml there are 70g. How many grams are in 500 ml?

We apply the simple three rule and solve:

   100ml -----------> 70g dextrose

   500ml----------> X g dextrose

500ml x 70g / 100ml = X

                         350g = X

There are 350 grams of dextrose in 500 ml of the 70% dextrose solution.

A 70% solution of dextrose means that the solution contains 70 grams of dextrose per 100 milliliters of solution.

To calculate the grams of dextrose in 500 ml of this solution, we can set up a proportion:

(70 g / 100 ml) = (x g / 500 ml)

To solve for x, we can cross-multiply and then divide:

70 g * 500 ml = 100 ml * x g

35,000 g·ml = 100 ml * x g

Dividing both sides by 100 ml: 350 g = x g

Thus, there are 350 grams of dextrose in 500 ml of the 70% dextrose solution.

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To prepare 100 mL of a 0.15 M NaOH solution, you will need approximately 0.60 g of NaOH.

To calculate the mass of NaOH needed to prepare a 0.15 M solution, we need to use the formula:

Mass (g) = Molarity (M) x Volume (L) x Molar Mass (g/mol)

In this case, the molarity is 0.15 M and the volume is 100 mL (or 0.1 L). The molar mass of NaOH is 22.990 + 15.999 + 1.008 = 39.997 g/mol.

Mass (g) = 0.15 M x 0.1 L x 39.997 g/mol = 0.5999 g, which can be rounded to 0.60 g.