Author: Anonymous

Phosphorus pentachloride decomposes to phosphorus trichloride at high temperatures according to the equation: At 250° 0.125 M PCl5 is added to the flask. If Kc = 1.80, what are the equilibrium concentrations of each gas?

The first-order decomposition of N2O at 1000 K has a rate constant of 0.76 s-1. If the initial concentration of N2O is 10.9 M, what is the concentration of N2O after 9.6 s?

Which of the following represents the equation for a second-order half-life?

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?