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NEET CHEMISTRYMedium

The slope of Arrhenius Plot (lnk\ln k v/s 1/T1/T) of the first-order reaction is 5×103 K-5 \times 10^3 \text{ K}. The value of EaE_a of the reaction is: [Given R=8.314 J K1 mol1R = 8.314 \text{ J K}^{–1} \text{ mol}^{–1}]

A

166 kJ mol1166 \text{ kJ mol}^{–1}

B

83 kJ mol1–83 \text{ kJ mol}^{–1}

C

41.5 kJ mol141.5 \text{ kJ mol}^{–1}

D

83.0 kJ mol183.0 \text{ kJ mol}^{–1}

Step-by-Step Solution

According to the Arrhenius equation, k=AeEa/RTk = A e^{-E_a/RT} Taking the natural logarithm on both sides yields: lnk=EaR(1T)+lnA\ln k = -\frac{E_a}{R} \left(\frac{1}{T}\right) + \ln A Comparing this with the equation of a straight line, y=mx+cy = mx + c, the plot of lnk\ln k versus 1/T1/T gives a straight line with slope m=EaRm = -\frac{E_a}{R}. Given slope =5×103 K= -5 \times 10^3 \text{ K} EaR=5×103 K-\frac{E_a}{R} = -5 \times 10^3 \text{ K} Ea=5×103×RE_a = 5 \times 10^3 \times R Ea=5×103 K×8.314 J K1 mol1=41570 J mol1=41.57 kJ mol141.5 kJ mol1E_a = 5 \times 10^3 \text{ K} \times 8.314 \text{ J K}^{-1} \text{ mol}^{-1} = 41570 \text{ J mol}^{-1} = 41.57 \text{ kJ mol}^{-1} \approx 41.5 \text{ kJ mol}^{-1}.

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