Author: Anonymous

At 800 K, the equilibrium constant, Kp, for the following reaction is 3.2 × 10–7. 2 H2S(g) 2 H2(g) + S2(g) A reaction vessel at 800 K initially contains 3.00 atm of H2S. If the reaction is allowed to equilibrate, what is the equilibrium pressure of S2?

Which of the following statements is true if reaction quotient (Q) is greater than equilibrium constant (K)?

For a certain reaction of the general form aA → products, a plot of the experimental data of ln[A] versus time is linear. What is the reaction order with respect to the reactant (A)?

Below is a proposed mechanism for the decomposition of H2O2. H2O2 + I– → H2O + IO– slow H2O2 + IO– → H2O + O2 + I– fast Which of the following statements is incorrect?

The mechanism of a chemical reaction is given below.   (CH3)3CCl → (CH3)3C+ + Cl– (slow)   (CH3)3C+ + OH– → (CH3)3COH (fast) Which of the following statements concerning the reaction is/are correct?   1. The overall balanced reaction is: (CH3)3CCl + OH– → (CH3)3COH + Cl–   2. Hydroxide ion is a reaction intermediate.   3. The following rate law is consistent with the mechanism: rate = k[(CH3)3CCl]OH–].

For the equilibrium PCl5(g) PCl3(g) + Cl2(g), Kc = 2.0 × 101 at 240°C. If pure PCl5 is placed in a 1.00-L container and allowed to come to equilibrium, and the equilibrium concentration of PCl3(g) is 0.50 M, what is the equilibrium concentration of PCl5(g)?

What is the Kc equilibrium-constant expression for the following equilibrium? NiO(s) + H2(g) Ni(s) + H2O(g)

For the equilibrium PCl5(g) PCl3(g) + Cl2(g), Kc = 4.0 at 228°C. If pure PCl5 is placed in a 1.00-L container and allowed to come to equilibrium, and the equilibrium concentration of PCl5(g) is 0.19 M, what is the equilibrium concentration of PCl3?

The judge would have sent him to prison if he _______ (catch- passive)

You _______________ smoke inside the school.