In the equation below,
PCl3(g) + Cl2(g) « PCl5(g)
the forward reaction is first order in both PCl3 and Cl2 and the reverse reaction is first order in PCl5.
(a) Suppose that 2 moles of PCl3 and 1 mole of Cl2 are mixed in a closed 1.0 L container at constant temperature. Draw a graph that shows how the concentrations of PCl3, Cl2, and PCl5 change with time until after equilibrium has been firmly established. Indicate the numerical values on the concentration axis.
(b) Give the initial rate law for the forward reaction.
(c) Provide a molecular explanation for the dependence of the rate of the forward reaction on the concentrations of the reactants.
(d) Provide a molecular explanation for the dependence of the rate of the forward reaction on temperature. Remember to include the Maxwell-Boltzmann graph in your answer.
(a) exact values of concentrations can not be calculated because the value of Keq is not given . See the graph below.
(b) Initial rate of forward reaction = kf[PCl3][Cl2]
= kf (2M)(1M) = 2k mol/L.sec-1
(Where kf is rate constant of forward reaction).
(c)
As PCl3 and Cl2 molecules collide , it might form the product PCl5. The number of collisions would depends on the number density of that particular molecules. Hence higher the number of molecules of reactants per unit volume , higher will be number of collisions and higher would be the rate of reaction. Hence rate of reaction would depends upon the concentration of both PCl3 and Cl2 .
(d) As the temperature of reactants is increased the average kinetic energy (& total energy) of molecules also increases . The fraction of molecules having energy higher that activation energy also increases . Hence number of successful collision would also increases . See the picture below for Maxwell Boltzmann distribution of speed graph.
In the equation below, PCl3(g) + Cl2(g) « PCl5(g) the forward reaction is first order in...
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