Question

2 icl + h2i2 + 2 hcl is first order in icl and second order in h2. Complete the rate law for this reaction in the box below. Use the form k[a]m[b]n... , where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = in an experiment to determine the rate law, the rate constant was determined to be 2.01 m-2s-1. Using this value for the rate constant, the rate of the reaction when [icl] = 0.273 m and [h2] = 0.217 m would be ms-1.

Answer 1

2 ICl + H2   ----> I2 + 2 HCl

as given that rate is first order with respect to ICl and second order with respect to H2

The rate law will be

Rate = K [ICl] [ H2]^2

b) Given that K = 2.01 M^-2 s^-1

Concentrations are

[ICl] = 0.273 m and [H2] = 0.217 m

Therefore rate = 2.01 X (0.273)(0.217)^2 = 0.0258 M / s