Given the equation: rate = k[H2O2]m[I-]n Which of the following statements is (are) true about the orders, m and n? A. m and n are independent from the molar coefficients of the reactants in the balanced chemical equation. B. m and n must be determined by experiment C. m and n are equal to each other in all cases. D. m and n are equal to the molar coefficients of H2O2 and I - in the balanced chemical reaction, respectively.

Question

Lexie Stanton

Chemistry

15 April, 04:09

Given the equation: rate = k[H2O2]m[I-]n Which of the following statements is (are) true about the orders, m and n? A. m and n are independent from the molar coefficients of the reactants in the balanced chemical equation. B. m and n must be determined by experiment C. m and n are equal to each other in all cases. D. m and n are equal to the molar coefficients of H2O2 and I - in the balanced chemical reaction, respectively.

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Answers (1)

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Brett Haas · Answer 1

A. m and n are independent from the molar coefficients of the reactants in the balanced chemical equation.

B. m and n must be determined by experiment.

Explanation:

rate = k[H2O2]^m * [I-]^n

The Order of Reaction refers to the power dependence of the rate on the concentration of each reactant.

Either the differential rate law or the integrated rate law can be used to determine the reaction order of reactants from experimental data.