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

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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.

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Detailed Solution

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

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

${ΔH}_{SP} {= ΔH}_{SQ} {+ ΔH}_{QP}$

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