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For a reaction, what generally happens if the temperature is increased?

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?