For the reaction 2H₂S(g) 2H₂(g)+ S₂(g),K_c = 9.1 × 10² at 750 K.What will happen when 0.10 mol of H₂S,1.0 mol of H₂,and 1.5 mol of S₂ are added to a 1.0-L container and the system is brought to 750 K?

Question

Quizplus · Accepted Answer

According to the given equilibrium constant, the reaction favors the products. Therefore, when reactants are added to the system, the reaction will shift towards the products. As there are more moles of H₂ than S₂, the reaction will shift towards the side with fewer moles, which is the side with more H₂. Hence, more H₂ will be formed than S₂, and the answer is B.

For the Reaction 2H2S(g) 2H2(g)+ S2(g),Kc = 9

For the Reaction 2H₂S(g) 2H₂(g)+ S₂(g),K_c = 9