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A student ran the following reaction in the laboratory at 375 K: CH4(g) + CCI4(g) = 2CH2CI2(g) When she introduced 4.58x10-2 moles of CH4(g) and 6.00x102 moles of CCI4(g) into a 1.00 liter container, she found the equilibrium concentration of CH2CI2(g) to be 1.68x10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction.

A student ran the following reaction in the laboratory at 375 K: CH4(g) + CCI4(g) = 2CH2CI2(g) When she introduced 4.58x10-2 moles of CH4(g) and 6.00x102 moles of CCI4(g) into a 1.00 liter container, she found the equilibrium concentration of CH2CI2(g) to be 1.68x10-2 M. Calculate the equilibrium constant, Kc, she obtained for this reaction.

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter15: Principles Of Chemical Reactivity: Equilibria
Section15.4: Using Equilibrium Constants In Calculations
Problem 15.5CYU: The decomposition of PCl5(g) to form PCl3(g) and Cl2(g) has Kc = 33.3 at a high temperature. If the...
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A student ran the following reaction in the laboratory at 375 K: CH4(g) + CC14(g) = 2CH2C22(g) When she introduced 4.58x10 2 moles of CH4(g) and 6.00x102 moles of CCI4(g) into a 1.00 liter container, she found the equilibrium concentration of CH2CI2(g) to be 1.68x10-2 M. Calculate the equilibrium constant, K, she obtained for this reaction. K. =
Transcribed Image Text:A student ran the following reaction in the laboratory at 375 K: CH4(g) + CC14(g) = 2CH2C22(g) When she introduced 4.58x10 2 moles of CH4(g) and 6.00x102 moles of CCI4(g) into a 1.00 liter container, she found the equilibrium concentration of CH2CI2(g) to be 1.68x10-2 M. Calculate the equilibrium constant, K, she obtained for this reaction. K. =
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