Question

For the reaction R-->P, write the differential rate law.​

Answer 1

Answer:

answer is k[R]^1

Explanation:

Rate of a reaction -----> change in any one of the reactants are products per unit time

Answer 2

The differential rate law is -d[R]/dt = k[R]^m.

• The differential rate law is an equation that describes how the rate of a chemical reaction changes with the concentration of one or more reactants or products. For a general reaction A + B → C + D, the differential rate law can be written as:
• -d[A]/dt = k[A]^m[B]^n
• Where: -d[A]/dt is the change in the concentration of reactant A with respect to time (measured in mol/L*s) k is the rate constant of the reaction (measured in L^(m+n) mol^(-m-n) s^(-1)) and m and n are the reaction order for reactant A and reactant B respectively.

• In your case, as the reaction is R-->P and the reactant is R, the differential rate law can be written as: -d[R]/dt = k[R]^m
• Where m is the reaction order for reactant R, k is the rate constant of the reaction and -d[R]/dt is the change in the concentration of reactant R with respect to time.
• It's important to note that the differential rate law is based on the assumption that the reaction is taking place under pseudo-first-order conditions and the reactant concentrations are not changing significantly during the reaction.

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