JEE MAIN - Chemistry (2019 - 10th January Morning Slot - No. 8)
Consider the given plots for a reaction obeying Arrhenius equation (0oC < T < 300oC) : (K and Ea are rate constant and activation energy, respectively)
_10th_January_Morning_Slot_en_8_1.png)
Choose the correct option :
Choose the correct option :
I is right but II is wrong
Both I and II are correct
Both I and II are wrong
I is wrong but II is right
Explanation
Arrhenius Equation -
Arrhenius gave the quantitative dependence of rate constant on temperature by the Arrhenius equation.
- wherein
$$k = A{e^{ - {E_a}/RT}}$$
$${\mathop{\rm lnk}\nolimits} = lnA - {{{E_a}} \over {RT}}$$
k = Rate constant
as we have learned in Arrhenius equation when we increase Ea, K should decrease As T increases, power of exponential increases so k also increase.
Hence, both the plots are correct.
Arrhenius gave the quantitative dependence of rate constant on temperature by the Arrhenius equation.
- wherein
$$k = A{e^{ - {E_a}/RT}}$$
$${\mathop{\rm lnk}\nolimits} = lnA - {{{E_a}} \over {RT}}$$
k = Rate constant
as we have learned in Arrhenius equation when we increase Ea, K should decrease As T increases, power of exponential increases so k also increase.
Hence, both the plots are correct.
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