At 298 K temperature the activation energy for the reaction x2+y2 arrow 2 x y+20 kJ is 15 kJ. What will be the activation energy for the reaction 2 x y arrow x2+y2 ?

Question

At 298 K temperature the activation energy for the reaction x2+y2 arrow 2 x y+20 kJ is 15 kJ. What will be the activation energy for the reaction 2 x y arrow x2+y2 ? (A) -15 kJ (B) +35 kJ (C) -5 kJ (D) -35 kJ

Tardigrade Admin · Accepted Answer

ΔR H = activation energy of forward reaction - activation energy of backward reaction. ⇒ -20=15-? So, +35 kJ .

Q. At $298 K$ temperature the activation energy for the reaction $x_{2} + y_{2} \to 2 x y + 20 k J$ is $15 k J$ . What will be the activation energy for the reaction $2 x y \to x_{2} + y_{2} ?$

-15 kJ

+35 kJ

-5 kJ

-35 kJ

$Δ_{R} H =$ activation energy of forward reaction - activation energy of backward reaction.
$\Rightarrow - 20 = 15 - ?$
So, $+ 35 k J .$

Q. At 298K temperature the activation energy for the reaction x2​+y2​→2xy+20kJ is 15kJ. What will be the activation energy for the reaction 2xy→x2​+y2​?