2icl + 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 , 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.

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

answer: c. the experiment shows that the red substance experienced a chemical change.

explanation: chemical change is the change in which chemical composition of the substance changes. physical change is the change in which there is no change in chemical composition.

chemical changes are accompanied by following changes:

a) precipitate formation

b) energy is released or absorbed

c) formation of bubbles

d) change in color

as it is given that the red color has disappeared and there is production of gas, it means the red substance has undergone a chemical change.

e