For the equilibrium system; CO_2(g) + H_2(g) doubleheadarrow CO (g) + H_2 O (g)
ID: 493186 • Letter: F
Question
For the equilibrium system; CO_2(g) + H_2(g) doubleheadarrow CO (g) + H_2 O (g) delta H = + 42 kJ/mol K equals 1.6 at 1260 K. If 0.15 mol each of CO_2, H_2, CO, and H_2 O (all at 1260 K) were placed in a 1.0-L thermally insulated vessel that was also at 1260 K, then as the system came to equilibrium: The temperature would decrease and the mass of CO would decrease. The temperature would decrease and the mass of CO would increase. The temperature would remain constant and the mass of CO would increase. The temperature would increase and the mass of CO would increase. The temperature would increase and the mass of CO would decrease.Explanation / Answer
Kc = [CO]{H2O]/[CO2][H2] = 0.15 x 0.15/0.15 x 0.15 = 1
K > Kc K=1.6
The reaction favoured towords to the forword direction.
In the forword direction , Concentration of CO would increasesa and temperature increases due to endothermic reaction.
The answer is D.