Consider the following reaction where K_c = 0.5 at 350 K: 2CH_2Cl_2(g) CH_4(g) +

Question

Consider the following reaction where K_c = 0.5 at 350 K: 2CH_2Cl_2(g) CH_4(g) + CCl_4(g) A reaction mixture was found to contain 1.23 times 10^-2 moles of 2CH_2Cl_2(g), 2.65 times 10^-2 moles of CH_4(g), and 4.38 times 10^-2 moles of 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 = The reaction: A. must run in the forward direction to reach equilibrium. B. must run in the reverse direction to reach equilibrium. C. is at equilibrium.

Explanation / Answer

first calculate the Qc to deside weather it is in equilibrium or not

Qc = [CCl4] [CH4] / [CH2Cl2]2

Qc = [0.0438] [0.0265] / [0.0123]2

Qc = 0.0011607 / 0.00015129

Qc = 7.67

Kc = 10.5

Kc > Qc so reaction is not at equilibrium

so reaction proceeds to right

forward direction to reach equilibrium.

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