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A student ran the following reaction in the laboratory at 326 K: CH4(9) + CCl4(9)=2CH₂Cl₂(9) When she introduced CH4(9) and CCl4(9) into a 1.00 L evacuated container, so that the initial partial pressure of CH4 was 0.722 atm and the initial partial pressure of CCl4 was 0.2 found that the equilibrium partial pressure of CCl4 was 0.208 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Kp = Submit Answer Retry Entire Group 8 more group attempts remaining

A student ran the following reaction in the laboratory at 326 K: CH4(9) + CCl4(9)=2CH₂Cl₂(9) When she introduced CH4(9) and CCl4(9) into a 1.00 L evacuated container, so that the initial partial pressure of CH4 was 0.722 atm and the initial partial pressure of CCl4 was 0.2 found that the equilibrium partial pressure of CCl4 was 0.208 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Kp = Submit Answer Retry Entire Group 8 more group attempts remaining

Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter16: Spontaneity, Entropy, And Free Energy
Section: Chapter Questions
Problem 83AE: Consider the following system at equilibrium at 25C: PCl3(g)+Cl(g)PCl5(g)G=92.50KJ What will happen...
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A student ran the following reaction in the laboratory at 326 K: CH4(g) + CCl4(9) —2CH₂Cl₂(g) When she introduced CH4(g) and CCl4(g) into a 1.00 L evacuated container, so that the initial partial pressure of CH4 was 0.722 atm and the initial partial pressure of CCl4 was 0.254 atm, she found that the equilibrium partial pressure of CCl4 was 0.208 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Kp Submit Answer Retry Entire Group 8 more group attempts remaining
Transcribed Image Text:A student ran the following reaction in the laboratory at 326 K: CH4(g) + CCl4(9) —2CH₂Cl₂(g) When she introduced CH4(g) and CCl4(g) into a 1.00 L evacuated container, so that the initial partial pressure of CH4 was 0.722 atm and the initial partial pressure of CCl4 was 0.254 atm, she found that the equilibrium partial pressure of CCl4 was 0.208 atm. Calculate the equilibrium constant, Kp, she obtained for this reaction. Kp Submit Answer Retry Entire Group 8 more group attempts remaining
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