The rate constant for the first order decomposition of H-2 O-2 is given by the following equation- log- k - 14-2 - 1-0 - 10-4 K-T Calculate E-a for this reaction and rate constant k of its half-life period be 200 minutes- - Given- R- 8-314 - JK-1 mol-1

According to Arrhenius equation, k= Ae^ E_a / RT lnk = ln A E_a/RT logk = log A E_a/ 2.303 RT Comparing with the given equation, E_a/2.303 RT = 1.0 × 10^4 K ...

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Standard XII

Physics

Alpha Decay

The rate cons...

Question

The rate constant for the first order decomposition of $H_{2} O_{2}$ is given by the following equation:

$l o g k = 14.2 - \frac{1.0 \times 10^{4} K}{T}$

Calculate $E_{a}$ for this reaction and rate constant k of its half-life period be 200 minutes. ( Given: R= $8.314 J K^{- 1} m o l^{- 1}$

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Solution

According to Arrhenius equation,
$k = A e^{- E_{a} / R T}$
$l n k = l n A - \frac{E_{a}}{R T}$
$l o g k = l o g A - \frac{E_{a}}{2.303 R T}$
Comparing with the given equation,
$\frac{E_{a}}{2.303 R T} = \frac{1.0 \times 10^{4} K}{T}$
$E_{a} = 2.303 R \times 1.04 \times 10^{4} K$
$E_{a} = 2.303 (8.314 J K^{- 1} m o l^{- 1}) \times 1.0 \times 10^{4} K$
$E_{a} = 191.47 k J m o l^{- 1}$
Half-life period, $t_{(} 1 / 2) = 200 minutes$
Rate constant, $k = \frac{0.693}{t_{(} 1 / 2)}$
$k = \frac{0.693}{200}$
$k = 0.3465 m i n^{- 1}$

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The rate constant for the first order decomposition of H2O2 is given by the following equation: log k=14.2−1.0×104KT Calculate Ea for this reaction and rate constant k of its half-life period be 200 minutes. ( Given: R= 8.314 JK−1mol−1

The rate constant for the first order decomposition of $H_{2} O_{2}$ is given by the following equation:

$l o g k = 14.2 - \frac{1.0 \times 10^{4} K}{T}$

Calculate $E_{a}$ for this reaction and rate constant k of its half-life period be 200 minutes. ( Given: R= $8.314 J K^{- 1} m o l^{- 1}$