Answers are given, please work through and explain **Reaction Analysis for Educational Purposes**Given Reaction:\[ \text{CO(g)} + 3 \text{H}_2\text{(g)} \rightarrow \text{CH}_4\text{(g)} + \text{H}_2\text{O(g)} \]**Table 1: Equilibrium Concentrations at Different Temperatures**| Trial / Temperature | \([\text{CO}]_{\text{eq}}\) | \([\text{H}_2]_{\text{eq}}\) | \([\text{CH}_4]_{\text{eq}}\) | \([\text{H}_2\text{O}]_{\text{eq}}\) ||----------------------|----------------------------|-----------------------------|-------------------------------|-------------------------------------|| Trial #1 / 298 K | \(3.02 \times 10^{-12}\) | \(4.30 \times 10^{-6}\) | 0.700 | 1.68 || Trial #2 / 1200 K | 0.00286 | 0.821 | 0.0952 | 0.0652 |**Questions and Analysis:**a. **Is the reaction endothermic or exothermic?** - Consider the value of \( K_c \) and Le Châtelier's Principle. - **Answer:** Exothermicb. **For a third trial at 1200 K, determine the shift in the reaction to achieve equilibrium.** - Data before equilibrium:| Trial / Temperature | \([\text{CO}]\) | \([\text{H}_2]\) | \([\text{CH}_4]\) | \([\text{H}_2\text{O}]\) ||----------------------|---------------|-----------------|-------------------|--------------------------|| Trial #3 / 1200 K | 2.00 | 2.95 | \(1.02 \times 10^{-4}\) | \(2.5 \times 10^{-4}\) | - **Direction of shift:** Towards the products**Overall Conclusion:**The reaction is exothermic, as indicated by a shift towards the products with an increase in temperature.

Given reaction: CO(g) + 3H2(g) ↔CH4(g) + H2O (g)

9) You are given the following information for the reaction: CO(g) + 3 H₂(g) → CH4 (g) + H₂O(g) Trial / Temperature Trial # 1/298 K Trial # 2/1200 K [CO] eq 3.02 x 10-12 2.86 x 10-3 Trial / Temperature Trial # 3/ 1200 K [CO] 2.00 [H₂]eq 4.30 x 10-6 0.821 a. Is the reaction endothermic or exothermic? (Hint: consider the value of Kc and Le Châtelier's Principle) b. A third trial was performed at 1200 K, and prior to reaching equilibrium, the data below was collected. Which way does the reaction need to shift in order to achieve equilibrium? Answer: exothermic, products [CH4]eq 0.700 0.0952 [H₂] 2.95 [H₂Oleq 1.68 0.0652 [CH4] 1.02 x 10-4 [H₂O] 2.5 x 10-4

9) You are given the following information for the reaction: CO(g) + 3 H₂(g) → CH4 (g) + H₂O(g) Trial / Temperature Trial # 1/298 K Trial # 2/1200 K [CO] eq 3.02 x 10-12 2.86 x 10-3 Trial / Temperature Trial # 3/ 1200 K [CO] 2.00 [H₂]eq 4.30 x 10-6 0.821 a. Is the reaction endothermic or exothermic? (Hint: consider the value of Kc and Le Châtelier's Principle) b. A third trial was performed at 1200 K, and prior to reaching equilibrium, the data below was collected. Which way does the reaction need to shift in order to achieve equilibrium? Answer: exothermic, products [CH4]eq 0.700 0.0952 [H₂] 2.95 [H₂Oleq 1.68 0.0652 [CH4] 1.02 x 10-4 [H₂O] 2.5 x 10-4

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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