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The rate law for a hypothetical reaction is rate = k [A]2. When the concentration is 0.10 moles/liter, the rate is 2.7 × 10-5 M*s-1. What is the value of k?

Verified Answer :

Hagrid

Given:

rate = k [A]2

concentration is
0.10 moles/liter

rate is 2.7 × 10-5 Ms-1

Required:

Value of k

Solution:

rate = k [A]2

2.7 × 10-5 Ms-1
= k (0.10 moles/liter)^2

k = 2.7 x 10^-3
liter per mole per second

Answer:The value of rate constant is \(2.7\times 10^{-3} Ls^{-1} mol^{-1}\).

Explanation:

Concentration of [A]=0.10 mol/L

The rate of the reaction = \(2.7\times 10^{-5} M/s\)

Rate constant = k

The given rate law:

\(R=k[A]^2\)

\(2.7\times 10^{-5} M/s=k\times (0.10 mol/L)^2\)

\(k=\frac{2.7\times 10^{-5} mol/L s}{0.10 mol/L\times 0.10 mol/L}=2.7\times 10^{-3} Ls^{-1} mol^{-1}\)

The value of rate constant is \(2.7\times 10^{-3} Ls^{-1} mol^{-1}\).

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