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Given the following rate law, how does the rate of reaction change if the concentration of Y is doubled?

Consider the following reaction at equilibrium.  What effect will adding more H2S have on the system                       (H2S(g) + 3 O2(g)  ⇌  2 H2O(g) + 2 SO2(g)

Consider the following reaction:                         CuS(s) + O2(g)  ⇌  Cu(s) + SO2(g)   A reaction mixture initially contains 2.9 M O2.  Determine the equilibrium concentration of O2 if Kc for the reaction at this temperature is 1.5.

The second-order decomposition of NO2 has a rate constant of 0.255 M-1s-1. How much NO2 decomposes in 8.00 s if the initial concentration of NO2 (1.00 L volume) is 1.33 M?

In which of the following reactions will Kc = Kp?

Which of the following is/are true concerning equilibrium constants?   1. When an equilibrium constant is very large, the equilibrium mixture contains more reactants than products.   2. When an equilibrium constant is very small, the equilibrium mixture contains more products than reactants.   3. When an equilibrium constant is neither large nor small, the equilibrium mixture contains approximately equal amounts of reactants and products.

For which of the following values of the equilibrium constant does the reaction mixture contain mostly reactants?

What is the overall order of the following reaction, given the rate law?

Consider the following reaction at equilibrium.  What effect will removing H2O have on the system?                         2 H2S(g) + 3 O2(g)  ⇌  2 H2O(g) + 2 SO2(g)

What is the overall order of the following reaction, given the rate law?2