Kinetics

1 For the hypothetical reaction A+B=> products, the rate law is first order in A and first order in B. When the initial concentrations of A and B are .05 M and .08 M respectively, the initial rate is 1.6x10-3 M/s.

a) What is the form of the rate equation? b) What is the value and units of the rate constant? c) If the initial concentration of A were tripled what would happen to the rate? d) If the initial concentration of A and B were both tripled what would happen to the rate? e) If the initial concentration of A and B were both tripled what would happen to the rate constant? f) What would the initial rate be if the initial concentrations of A and B are .035 M and .098 M? respectively

2. If the concentration of A drops from 0.93 to 0.23 in 28.4 min and the

reaction is second order, what is the rate constant for the reaction?

3. Explain what the term pseudo first order means and give an example.

4. Graphically (Using MathCad) show what order the following reaction is and determine the rate constant. Show the graph for both first and second order plots.

5. The following data were obtained on the rate of hydrolysis of 17% sucrose in .099 M HCl aqueous solutions at 35 C.

Graphically (using MathCad) show what order this reaction is and determine the rate constant. Show the graph for both first and second order plots.