Medium
At $527 \, ^{\circ}C$ temperature,the activation energy is $54.7 \, kJ/mol$. The value of the Arrhenius factor is $4 \times 10^{10}$. The rate constant will be:
- A$12.28 \times 10^{11}$
- B$10.7 \times 10^{6}$
- C$12.28 \times 10^{17}$
- D$14.58 \times 10^{-13}$
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Similar Questions
The first order rate constant $k$ is related to temperature $T$ as $\log \, k = 15.0 - (10^{6} / T)$. Which of the following pairs of values for the Arrhenius factor $A$ and activation energy $E_a$ is correct?
Medium
View SolutionFor the reaction,$A \rightleftharpoons B$,$E_a = 50 \ kJ \ mol^{-1}$ and $\Delta H = -20 \ kJ \ mol^{-1}$. When a catalyst is added,$E_a$ decreases by $10 \ kJ \ mol^{-1}$. What is the $E_a$ for the backward reaction in the presence of the catalyst?
MediumKCET 2024
View SolutionIn the given graph,$E_{a}$ for the reverse reaction will be (in $kJ$)
For a first order chemical reaction,
Catalysts are used to increase the rate of a chemical reaction. Because it
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