Multiple Choice
The following reaction is first order: C2H6 → 2 CH3. If the rate constant is equal to 5.5 × 10⁻⁴ s⁻¹ at 1000 K, how long will it take for 0.35 mol of C2H6 in a 1.00 L container to decrease to 0.10 mol in the same container?
15. Chemical Kinetics
Rate Law
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The overall order of a reaction is 2. The units of the rate constant for the reaction are ______.
A
M^-1 s^-1
B
M s^-1
C
s^-1
D
M^-2 s^-1
Verified step by step guidance1
Understand that the overall order of a reaction is the sum of the exponents of the concentration terms in the rate law. In this case, the overall order is 2.
Recall that the units of the rate constant depend on the overall order of the reaction. For a reaction of order n, the units of the rate constant k are given by: \( \text{M}^{1-n} \text{s}^{-1} \).
Substitute the overall order of the reaction (which is 2) into the formula for the units of the rate constant: \( \text{M}^{1-2} \text{s}^{-1} \).
Simplify the expression \( \text{M}^{1-2} \text{s}^{-1} \) to find the units of the rate constant. This simplifies to \( \text{M}^{-1} \text{s}^{-1} \).
Compare the simplified units \( \text{M}^{-1} \text{s}^{-1} \) with the given options to identify the correct answer.
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