Difficult
$A$ reaction takes place in three steps with individual rate constant and activation energy as follows: $Step$ $Rate \ constant$ $Activation \ energy$ $Step-1$ $k_1$ $E_{a1} = 180 \ kJ/mol$ $Step-2$ $k_2$ $E_{a2} = 80 \ kJ/mol$ $Step-3$ $k_3$ $E_{a3} = 50 \ kJ/mol$
If overall rate constant,$k = (\frac{k_1 k_2}{k_3})^{2/3}$,then overall activation energy of the reaction will be .......... $kJ/mol$.
| $Step$ | $Rate \ constant$ | $Activation \ energy$ |
| $Step-1$ | $k_1$ | $E_{a1} = 180 \ kJ/mol$ |
| $Step-2$ | $k_2$ | $E_{a2} = 80 \ kJ/mol$ |
| $Step-3$ | $k_3$ | $E_{a3} = 50 \ kJ/mol$ |
- A$140$
- B$150$
- C$130$
- D$120$
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An exothermic reaction $X \rightarrow Y$ has an activation energy of $30 \ kJ \ mol^{-1}$. If the energy change $\Delta E$ during the reaction is $-20 \ kJ \ mol^{-1}$,then the activation energy for the reverse reaction in $kJ \ mol^{-1}$ is $...$.
According to the Arrhenius equation, which of the following statements is correct?
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View SolutionConsider the following statements:
$(i)$ Increase in concentration of reactant increases the rate of a zero order reaction
$(ii)$ Rate constant $k$ is equal to $A$ if $E_a = 0$
$(iii)$ Rate constant $k$ is equal to $A$ if $E_a = \infty$
$(iv)$ $\log_e k$ vs $T$ is a straight line
$(v)$ $\log_e k$ vs $1/T$ is a straight line
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$(i)$ Increase in concentration of reactant increases the rate of a zero order reaction
$(ii)$ Rate constant $k$ is equal to $A$ if $E_a = 0$
$(iii)$ Rate constant $k$ is equal to $A$ if $E_a = \infty$
$(iv)$ $\log_e k$ vs $T$ is a straight line
$(v)$ $\log_e k$ vs $1/T$ is a straight line
Which of the following statements are correct?
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View SolutionThe rate of a reaction quadruples when the temperature changes from $293 \ K$ to $313 \ K$. Calculate the energy of activation of the reaction assuming that it does not change with temperature.
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