---### Calculations of Mole Fraction and Equilibrium Constant for a Reaction**Problem Statement:**A quantity of 0.29 moles of carbon dioxide (CO₂) was heated to a certain temperature with an excess of graphite in a closed container until the following equilibrium was reached:\[ \text{C(s)} + \text{CO}_2\text{(g)} \rightleftharpoons 2 \text{CO(g)} \]Under these conditions, the average molar mass of the gases was 34.5 g/mol.### Part (a): Calculate the mole fractions of CO and CO₂.**Solution:**#### The Mole Fraction of CO:\[ \text{The mole fraction of CO is} \]\[ \boxed{0.40625} \]#### The Mole Fraction of CO₂:\[ \text{The mole fraction of CO₂ is} \]\[ \boxed{0.59375} \]### Part (b): Calculate the equilibrium constant (\( K_p \)) if the total pressure is 10.5 atm.**Solution:**\[ \text{The value of } K_p \text{ is} \]\[ \boxed{9.12} \]**Note:** The red crosses next to the boxed values indicate these results were marked as incorrect. Review the problem statement and calculations to identify and correct possible mistakes.---### Potential Errors to Investigate:- Reassess the calculations involving mole fractions and molar masses.- Verify the equilibrium expression and calculations used to determine \( K_p \).Continue to the next part for further steps and explanation.---

Given : Moles of CO2 = 0.29 mole Average mole mass of gases at equilibrium= 34.5 g/mole Total…

Be sure to answer all parts. A quantity of 0.29 mole of carbon dioxide was heated to a certain temperature with an excess of graphite in a closed container until the following equilibrium was reached: C(s) + CO₂(g) 2 CO(g) Under these conditions, the average molar mass of the gases was 34.5 g/mol. (a) Calculate the mole fractions of CO and CO₂. The mole fraction of CO is 0.40625 The mole fraction of CO₂ is 0.59375X (b) What is Kp if the total pressure is 10.5 atm? 9.12

Be sure to answer all parts. A quantity of 0.29 mole of carbon dioxide was heated to a certain temperature with an excess of graphite in a closed container until the following equilibrium was reached: C(s) + CO₂(g) 2 CO(g) Under these conditions, the average molar mass of the gases was 34.5 g/mol. (a) Calculate the mole fractions of CO and CO₂. The mole fraction of CO is 0.40625 The mole fraction of CO₂ is 0.59375X (b) What is Kp if the total pressure is 10.5 atm? 9.12

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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