Consider the following reaction where K_c = 10.5 at 350 K: 2 CH_2C1_2 (g) CH_4 (
ID: 494470 • Letter: C
Question
Consider the following reaction where K_c = 10.5 at 350 K: 2 CH_2C1_2 (g) CH_4 (g) + CCl_4 (g) A reaction mixture was found to contain 1.17 times 10^-2 moles of CH_2C1_2 (g), 2.64 times 10^-2 moles of CH_4 (g), and 4.04 times 10^-2 moles of CCl_4(g), a 1.00 liter container. Indicate True (T) or False (F) for each of the following: In order to reach equilibrium CH_2Cl_2(g) must be produced. In order to reach equilibrium K_c must decrease. In order to reach equilibrium CH_4 must be consumed. Q_c is greater than K_c. The reaction is at equilibrium. No further reaction will occur.Explanation / Answer
Qc = [CH4][CCl4]/[CH2Cl2]^2
= (2.64*10^-2)(4.04*10^-2)/(1.17*10^-2)^2
= 7.79
1. False. Amount of CH2Cl2 is high. It has to break down to product
2. false . Kc is a constant
3. False . If Ch4 is consumed to form CH2Cl2, amount of Ch2Cl2 will increse and the equilibrium will be distured.
4.False. Qc is less than Kc as calculated above
5. False . The reaction is not at equilibrium. As, Qc< Kc, forward reaction is favored