SATHEE: Chemical Kinetics Question 56

Chemical Kinetics Question 56

Question: A hydrogenation reaction is carried out at 500 K. $C H_{2} = C H_{2} + H_{2} \to_{n o, c a t a l y s t}^{500 k} C H_{3} - C H_{3}$ Activation energy $-, E_{a}, K J, m o l^{- 1}$

$C H_{2} = C H_{2} + H_{2} \overset{p d, 400 k}{\to} C H_{3} - C H_{3}$ Activation energy = ( $E_{a} - 20$ ) KJ $m o l^{- 1}$ If rate remains constant, then $E_{a}$ is

Options:

A) $120 k J m o l^{- 1}$

B) $100 k J m o l^{- 1}$

C) $20 k J m o l^{- 1}$

D) $80 k J m o l^{- 1}$

Show Answer

Answer:

Correct Answer: B

Solution:

[b] $k = A e^{- E_{a} / R T}$

$k = A e^{- E_{a} / R \times 500}$

$k^{'} = A e^{- (E_{a} - 20) / R \times 400}$ Rates are equal, hence
$∴ A e^{- E_{a} / R \times 500} = A e^{- (E_{a} - 20) / R \times 400}$
$∴ \frac{E_{a}}{500} = \frac{E_{a} - 20}{400}$

$4 E_{a} = 5 E_{a} - 100$
$∴ E_{a} = 100 K J m o l^{- 1}$

Chemical Kinetics Question 56

Question: A hydrogenation reaction is carried out at 500 K. $C H_{2} = C H_{2} + H_{2} \to_{n o, c a t a l y s t}^{500 k} C H_{3} - C H_{3}$ Activation energy $-, E_{a}, K J, m o l^{- 1}$

Options:

Answer:

Solution:

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Chemical Kinetics Question 56

Question: A hydrogenation reaction is carried out at 500 K. CH2=CH2+H2→no,catalyst500kCH3−CH3 Activation energy −,Ea,KJ,mol−1

Options:

Answer:

Solution:

Engineering Preparation

Medical Preparation

NCERT Books & Solutions

Important Resources

Other Resources

Syllabus

Test Platform

Sample Mock Test

Mentorship

NCERT Exercise Video Solution

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Question: A hydrogenation reaction is carried out at 500 K. $C H_{2} = C H_{2} + H_{2} \to_{n o, c a t a l y s t}^{500 k} C H_{3} - C H_{3}$ Activation energy $-, E_{a}, K J, m o l^{- 1}$