Consider the following reaction where K_c = 10.5 at 350 K. 2CH_2Cl_2(g) CH_4(g)
ID: 969744 • Letter: C
Question
Consider the following reaction where K_c = 10.5 at 350 K. 2CH_2Cl_2(g) CH_4(g) + CCI_4(g) A reaction mixture was found to contain 1.22 times 10^-2 moles of CH_2Cl_2(g), 2.38 times 10^2 moles of CH_4(g), and 4.26 times 10 moles CCl_4(g), in a 1.00 liter container. Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction quotient, Q_c, equals The reaction must run in the forward direction to reach equilibrium. must run in the reverse direction to reach equilibrium. is at equilibrium.Explanation / Answer
Qc = [CCl4][ch4]/[CH2CL2]
= 0.0426*0.0238/0.0122
= 0.0831
Qc < Kc . so that forwardward reaction is favourable.
Answer: A