JEE PYQ: Thermodynamics Question 23
Question 23 - 2019 (09 Apr Shift 2)
Consider the given plot of enthalpy of the following reaction between A and B, $\text{A} + \text{B} \to \text{C} + \text{D}$.
Identify the incorrect statement.
(1) Activation enthalpy to form C is 5 kJ mol$^{-1}$ less than that to form D.
(2) C is the thermodynamically stable product.
(3) D is kinetically stable product.
(4) Formation of A and B from C has highest enthalpy of activation.
Show Answer
Answer: (1)
Solution
As we can see from the graph that activation enthalpy to form D from A + B is $15 - 5 = 10$ kJ mol$^{-1}$, whereas, to form C from A + B is $20 - 5 = 15$ kJ mol$^{-1}$. Therefore, activation enthalpy to form C is 5 kJ more (not less) than that to form D.
BETA
