Which of the following is the most likely cause for the increase in pressure observed in the container as the reaction reaches equilibrium? (A) A decrease in the strength of intermolecular attractions among molecules in the flask (B) An increase in the strength of intermolecular attractions among molecules in the flask (C) An increase in the number of molecules, which increases the frequency of collisions with the walls of the container (D) An increase in the speed of the molecules that then collide with the walls of the container with greater force

A mixture of 0.009482 mol of CH4, 0.02708 mol of H2S, 0.02785 mol of CS2, and 0.02860 mol of H2 is placed in a 1.0-L steel pressure vessel at 3918 K. The following equilibrium is established: 1 CH4(g) + 2 H2S(g)  1 CS2(g) + 4 H2(g) At equilibrium 0.001533 mol of CH4 is found in the reaction mixture.(a) Calculate the equilibrium partial pressures of CH4, H2S, CS2, and H2.Peq(CH4).Peq(H2S).Peq(CS2).Peq(H2).(b) Calculate KP for this reaction.KP.

A sample of H,S(g) at 0.495 atm is placed in a container and the following reaction reaches equilibrium. What is the total pressure of all gases in the container? 2H2S(g) = 2H2(g) + S2(g) K, = 3.85 x 10-7 0.497 atm 0.215 atm 0.793 atm 0.624 atm 0.387 atm O O O

#3

Why are the terms of reactant and product arbitrary in systems that are in equilibrium?

Which of the following would lead to an increased rate of reaction for gaseous reactants? (A) Increasing the volume of the reaction container (B) Decreasing the concentration of reactants (C) Increasing the temperature of the reactants (D) Decreasing the partial pressure of reactants (E) Running the reaction in front of a picture of Prof. Schwartz