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 ...

309

You visited us 309 times! Enjoying our articles? Unlock Full Access!

Byju's Answer

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= $8.314 J K^{- 1} m o l^{- 1}$

Open in App

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, $k = \frac{0.693}{t_{(} 1 / 2)}$
$k = \frac{0.693}{200}$
$k = 0.3465 m i n^{- 1}$

Suggest Corrections

Similar questions

The rate constant for the first order decomposition of H₂O₂ is given by the following equation:

log k = 14.34 − 1.25 × 10⁴K/T

Calculate E_a for this reaction and at what temperature will its half-period be 256 minutes?

Q. The rate constant for the first order decomposition of

H_{2} O_{2}

is given by the following equation:

log k = 14.2 - \frac{1.0 \times 10^{4}}{T}

Calculate

E_{a}

for this reaction and rate constant

k

if its half-life period be

200

minutes. (Given:

R = 8.314 J K^{- 1} {m o l}^{- 1}

)

The rate constant for the first order decomposition of $H_{2} O_{2}$ is given by the following equation, $l o g k = 14.34 - 1.25 \times 10^{4} K / T$ . Calculate $E_{a}$ for this reaction and at what temperature will its half-life period be 256 minutes?

Q. For a first order reaction with rate constant k and initial concentration a, the half-life period is given by:

Q. For a first-order reaction with the rate constant '

k

' and initial concentration '

a

', the half-life period is given by:

Join BYJU'S Learning Program

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= $8.314 J K^{- 1} m o l^{- 1}$