The rate of decomposition of hydrogen peroxide is first order in $H_{2} O_{2} .$ At $[H_{2} O_{2}] = 0.150 M$ , the decomposition rate was measured to be $4.83 \times 10^{- 6} M \cdot s^{- 1} .$ What is the rate constant for the reaction?

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$4.83 \times 10^{- 6} s^{- 1}$

$3.22 \times 10^{- 5} g^{- 1}$

$2.15 \times 10^{- 4} s^{- 1}$

$7.25 \times 10^{- 7} s^{- 1}$

answer is B.

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Detailed Solution

Rate constant for the reaction,

$4.83 \times 10^{- 6} = k \times 0.15$

$\Rightarrow k = 3.22 \times 10^{- 5} s^{- 1}$

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