Explain the reaction proceeds with a constant half-life

Reference no: EM13489002

The inversion of compound B is experimentally determined to follow the rate law: d[B]/dt = -k[B]a[H+]b. At 25 °C and a constant pH of 3.00, the reaction proceeds with a constant half-life of 40.0 min. At this same temperature, but at a constant pH of 1.00, the half-life is constant at 4.00 min. What are the exponents (orders) a and b in the above rate law?

Reference no: EM13489002

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