In the hydrogenation of ethylene using a nickel catalyst, the initial concentration of ethylene is 1.50 mol * L-1 and its rate constant (k) is 0.0016 mol * L-1 * s-1.

a. Determine the rate of reaction if it follows a zero-order reaction mechanism.

Question

Chemistry

Jared Anderson

11 May, 08:51

In the hydrogenation of ethylene using a nickel catalyst, the initial concentration of ethylene is 1.50 mol * L-1 and its rate constant (k) is 0.0016 mol * L-1 * s-1.

a. Determine the rate of reaction if it follows a zero-order reaction mechanism.

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Answers (1)

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Jeffrey Mcclure · Answer 1

0.0016 mol / (L. s)

Explanation:

The rate of a reaction (r) can be calculated by the initial concentration of the reagent, by the expression:

-r = k*[reagent]ⁿ

Where the minus sign represents that the reagent is disappearing, k is the rate constant, which depends on the temperature, and n is the order of the reaction. For the reaction with more than 1 reagent, each reagent will have its order, which is determined by experiments. So, for n = 0:

-r = 0.0016 * (1.50) ⁰

-r = 0.0016 mol / (L. s)

In the hydrogenation of ethylene using a nickel catalyst, the initial concentration of ethylene is 1.50 mol * L-1 and its rate constant (k) is 0.0016 mol * L-1 * s-1.a. Determine the rate of reaction if it follows a zero-order reaction mechanism.

In the hydrogenation of ethylene using a nickel catalyst, the initial concentration of ethylene is 1.50 mol * L-1 and its rate constant (k) is 0.0016 mol * L-1 * s-1.

a. Determine the rate of reaction if it follows a zero-order reaction mechanism.