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Q.

This reaction is first order with respect to $N_{2} O_{5}$ .
$2 N_{2} O_{5} (g) ⟶ 4 {NO}_{2} (g) + O_{2} (g)$
If the half-life for this reaction is 19.0 minutes, what is the rate constant, k for $r = k [N_{2} O_{5}]$ _?

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a

$0.0182 \min^{- 1}$

b

$0.0365 \min^{- 1}$

c

$0.0526 \min^{- 1}$

d

$0.0263 \min^{- 1}$

answer is A.

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Detailed Solution

For the half life,

$t_{1 / 2} = \frac{\ln 2}{2 K}$

The rate constant is,

$\Rightarrow K = \frac{0.693}{2 \times 19} = 0.0182 \min^{- 1}$

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This reaction is first order with respect to N2O5.2N2O5(g)⟶4NO2(g)+O2(g)If the half-life for this reaction is 19.0 minutes, what is the rate constant, k for r=kN2O5?