Author: Anonymous

The equilibrium constant is given for one of the reactions below. Determine the value of the missing equilibrium constant.

The rate constant for a first-order reaction is 0.54 M-1s-1.  What is the half-life of this reaction if the initial concentration is 0.27 M?

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?