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3 years ago

Convert 7.2 × 10^23 molecules of CO2 to moles (round to the nearest tenth). Unit?

Chemistry

1 answer:

Svetach [21]3 years ago

5 0

7.2 * 10^23 molecules CO2 1 mole CO2

x ___________________

6.02* 10^23 molecules CO2

=1.196

=1.2 moles of CO2

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The concentration of glucose inside a cell is 0.12 mM. Outside the cell the concentration of glucose is 12.9 mM. Calculate the c

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Answer:

The value of he change in Gibbs free energy ΔG = - 18.083 KJ

Explanation:

Given data

The concentration of glucose inside a cell is (P) = 0.12 m M

The concentration of glucose outside a cell is (R) = 12.9 m M

No. of moles = 1.5 moles

The change in Gibbs free energy

ΔG = RT ㏑ $\frac{P}{R}$

ΔG = 8.314 × 310 ㏑ $\frac{0.12}{12.9}$

ΔG = - 12.055 $\frac{J}{mole}$

Since No. of moles = 1.5 moles

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ΔG = - 12.055 × 1.5

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3 years ago

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3 years ago

Nitrogen dioxide and water react to form nitric acid and nitrogen monoxide, like this:

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Answer: The value of the equilibrium constant Kc for this reaction is 3.72

Explanation:

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Equilibrium concentration of $NO$ = $\frac{16.6g}{30g/mol\times 9.5L}=0.058M$

Equilibrium concentration of $NO_2$ = $\frac{22.5g}{46g/mol\times 9.5L}=0.051M$

Equilibrium concentration of $H_2O$ = $\frac{189.0g}{18g/mol\times 9.5L}=1.10M$

Equilibrium constant is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as $K_c$

For the given chemical reaction:

$2HNO_3(aq)+NO(g)\rightarrow 3NO_2(g)+H_2O(l)$

The expression for $K_c$ is written as:

$K_c=\frac{[NO_2]^3\times [H_2O]^1}{[HNO_3]^2\times [NO]^1}$

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Thus the value of the equilibrium constant Kc for this reaction is 3.72

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2 years ago

Convert 7.2 × 10^23 molecules of CO2 to moles (round to the nearest tenth). Unit?​

Convert 7.2 × 10^23 molecules of CO2 to moles (round to the nearest tenth). Unit?