JEE Main 2015 · 11 Apr · Shift 1 · Chemistry Q35

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ChemistrySingle correct+4 / -1Question 35 of 90

For the equilibrium, $\ce{A(g) <=> B(g)}$ , ΔH is −40 kJ/mol. If the ratio of the activation energies of the forward ( $E_f$ ) and reverse ( $E_b$ ) reactions is $\dfrac23$ then :

E_f=60

kJ/mol ;

E_b=100

kJ/mol

E_f=30

kJ/mol ;

E_b=70

kJ/mol

E_f=80

kJ/mol ;

E_b=120

kJ/mol

E_f=70

kJ/mol ;

E_b=30

kJ/mol

Answer and worked solution

Official answer: C

$\Delta H=E_f-E_b=-40$ and $E_f=\frac23E_b$ , so $-\frac13E_b=-40$ : $E_b=120$ and $E_f=80$ kJ/mol.

Topics:Arrhenius equation

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JEE Main 2015 · 11 Apr · Shift 1, Chemistry question 35