1
NEET 2024 (Re-Examination)
+4
-1

Rate constants of a reaction at $$500 \mathrm{~K}$$ and $$700 \mathrm{~K}$$ are $$0.04 \mathrm{~s}^{-1}$$ and $$0.14 \mathrm{~s}^{-1}$$, respectively; then, activation energy of the reaction is :

(Given: $$\log 3.5=0.5441, \mathrm{R}=8.31 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}$$)

A
182310 J
B
18500 J
C
18219 J
D
18030 J
2
NEET 2024
+4
-1

Activation energy of any chemical reaction can be calculated if one knows the value of

A
rate constant at standard temperature
B
probability of collision
C
orientation of reactant molecules during collision
D
rate constant at two different temperatures
3
NEET 2024
+4
-1

Which plot of $$\ln \mathrm{k}$$ vs $$\frac{1}{\mathrm{~T}}$$ is consistent with Arrhenius equation?

A
B
C
D
4
NEET 2024
+4
-1

The rate of a reaction quadruples when temperature changes from $$27^{\circ} \mathrm{C}$$ to $$57^{\circ} \mathrm{C}$$. Calculate the energy of activation.

Given $$\mathrm{R}=8.314 \mathrm{~J} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}, \log 4=0.6021$$

A
$$38.04 \mathrm{~kJ} / \mathrm{mol}$$
B
$$380.4 \mathrm{~kJ} / \mathrm{mol}$$
C
$$3.80 \mathrm{~kJ} / \mathrm{mol}$$
D
$$3804 \mathrm{~kJ} / \mathrm{mol}$$
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