Part 3: For each of the following questions, refer to the following balanced equation and the Data Table above. Give your answers to the first decimal place if the answer is greater than 1. Otherwise, use exponential format (e. g. 1.23E-10)2 HgO(s) = 2 Hg(l) + O2(g)f) Determine the value of Keq at 298 K (3 sig. figs.).R = 8.3145 J/moleKg) Determine the value of Grxn at 298 K when the partial pressure of O2(g) is 2.0 atm. Assume the equilibrium constant is Kp.R = 8.3145 J/moleK Use the following Data Table to answer the following questions:**Data Table**| Substance | \( H_f^\circ \) (kJ/mole) | \( S_f^\circ \) (J/mole·K) | \( G_f^\circ \) (kJ/mole) ||-----------|-------------------|-----------------|------------------|| \( \text{Hg}_{(l)} \) | 0 | 76.0 | 0 || \( \text{Hg}_{(g)} \) | 61.3 | 174.9 | 31.8 || \( \text{HgO}_{(s)} \) | -90.8 | 70.3 | -58.5 || \( \text{O}_2{(g)} \) | 0 | 205.0 | 0 |### Explanation:- **\( H_f^\circ \) (kJ/mole)**: Standard enthalpy of formation, which indicates the amount of energy either released or absorbed during the formation of one mole of a compound from its elements in their standard states. - **\( S_f^\circ \) (J/mole·K)**: Standard entropy, which measures the disorder or randomness in a system at the standard state. - **\( G_f^\circ \) (kJ/mole)**: Standard Gibbs free energy of formation, reflecting the spontaneity of a reaction at standard state conditions.

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Answered: Part 3: For each of the following…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Part 3:

For each of the following questions, refer to the following balanced equation and the Data Table above. Give your answers to the first decimal place if the answer is greater than 1. Otherwise, use exponential format (e. g. 1.23E-10)

2 HgO_(s) = 2 Hg_(l) + O_2(g)

f) Determine the value of K_eq at 298 K (3 sig. figs.).

R = 8.3145 J/moleK

g) Determine the value of G_rxn at 298 K when the partial pressure of O_2(g) is 2.0 atm. Assume the equilibrium constant is K_p.

R = 8.3145 J/moleK

Use the following Data Table to answer the following questions:

**Data Table**

| Substance | \( H_f^\circ \) (kJ/mole) | \( S_f^\circ \) (J/mole·K) | \( G_f^\circ \) (kJ/mole) |
|-----------|-------------------|-----------------|------------------|
| \( \text{Hg}_{(l)} \) | 0 | 76.0 | 0 |
| \( \text{Hg}_{(g)} \) | 61.3 | 174.9 | 31.8 |
| \( \text{HgO}_{(s)} \) | -90.8 | 70.3 | -58.5 |
| \( \text{O}_2{(g)} \) | 0 | 205.0 | 0 |

### Explanation:

- **\( H_f^\circ \) (kJ/mole)**: Standard enthalpy of formation, which indicates the amount of energy either released or absorbed during the formation of one mole of a compound from its elements in their standard states.

- **\( S_f^\circ \) (J/mole·K)**: Standard entropy, which measures the disorder or randomness in a system at the standard state.

- **\( G_f^\circ \) (kJ/mole)**: Standard Gibbs free energy of formation, reflecting the spontaneity of a reaction at standard state conditions.

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