A student ran the following reaction in the laboratory at 318 K: 2CH₂Cl₂(9) CH4(9) + CCl4(9) ? es if needed for this question. When he introduced CH₂Cl₂(9) at a pressure of 0.524 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of CH₂Cl₂(g) to be 5.27x10-² atm. Calculate the equilibrium constant, Kp, he obtained for this reaction. Kp = Submit Answer Retry Entire Group 9 more group attempts remaining

A student ran the following reaction in the laboratory at 318 K: 2CH₂Cl₂(9) CH4(9) + CCl4(9) ? es if needed for this question. When he introduced CH₂Cl₂(9) at a pressure of 0.524 atm into a 1.00 L evacuated container, he found the equilibrium partial pressure of CH₂Cl₂(g) to be 5.27x10-² atm. Calculate the equilibrium constant, Kp, he obtained for this reaction. Kp = Submit Answer Retry Entire Group 9 more group attempts remaining

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter12: Gaseous Chemical Equilibrium

Section: Chapter Questions

Problem 36QAP: At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s),...

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