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lianna [129]
3 years ago
15

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

hange in Gibbs free energy for the transport of 1.50 moles of glucose into the cell at 37°C.
Chemistry
1 answer:
Alenkasestr [34]3 years ago
7 0

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

Therefore

ΔG = - 12.055 × 1.5

ΔG = - 18.083 KJ

This the value of he change in Gibbs free energy.

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When 9.2 g of frozen N2O4 is added to a 0.50 L reaction vessel and the vessel is heated to 400 K and allowed to come to equilibr
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<u>Answer:</u> The value of K_c for the given reaction is 1.435

<u>Explanation:</u>

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

\text{Molarity of the solution}=\frac{\text{Mass of solute}}{\text{Molar mass of solute}\times \text{Volume of solution (in L)}}

Given mass of N_2O_4 = 9.2 g

Molar mass of N_2O_4 = 92 g/mol

Volume of solution = 0.50 L

Putting values in above equation, we get:

\text{Molarity of solution}=\frac{9.2g}{92g/mol\times 0.50L}\\\\\text{Molarity of solution}=0.20M

For the given chemical equation:

                 N_2O_4(g)\rightleftharpoons 2NO_2(g)

<u>Initial:</u>          0.20

<u>At eqllm:</u>     0.20-x        2x

We are given:

Equilibrium concentration of N_2O_4 = 0.057

Evaluating the value of 'x'

\Rightarrow (0.20-x)=0.057\\\\\Rightarrow x=0.143

The expression of K_c for above equation follows:

K_c=\frac{[NO_2]^2}{[N_2O_4]}

[NO_2]_{eq}=2x=(2\times 0.143)=0.286M

[N_2O_4]_{eq}=0.057M

Putting values in above expression, we get:

K_c=\frac{(0.286)^2}{0.143}\\\\K_c=1.435

Hence, the value of K_c for the given reaction is 1.435

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3 years ago
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