The diagram illustrates the energy change of a set of reactions.
Which of the following statement are correct?

see full answer

Talk to JEE/NEET 2025 Toppers - Learn What Actually Works!

Real Strategies. Real People. Real Success Stories - Just 1 call away

An Intiative by Sri Chaitanya

The enthalpy change for the transformation $R \to Q$ will be endothermic

The enthalpy change for the reaction $P \to R i s - 33 k J m o l^{- 1}$

The enthalpy change for the transformation $R \to Q$ will be exothermic

The enthalpy change for the transformation $S \to P$ will be + 42 kJ $m o l^{- 1}$

answer is C, D.

(Unlock A.I Detailed Solution for FREE)

Ready to Test Your Skills?

Check your Performance Today with our Free Mock Test used by Toppers!

Take Free Test

Detailed Solution

${ΔH}_{PR} {= ΔH}_{PQ} {+ ΔH}_{QS} {+ ΔH}_{SR} = (- 134) + 92 - (-75) {kJ mol}^{-1}$

$Δ H_{R Q} = Δ H_{R S} + Δ H_{S Q} = (- 75) - (+ 92) = - 168 k J m o l^{- 1} < 0 E x o t h e r m i c$

${ΔH}_{SP} {= ΔH}_{SQ} {+ ΔH}_{QP}$

Watch 3-min video & get full concept clarity

JEE

NEET

Foundation JEE

Foundation NEET

CBSE