ΔH for the reaction IF₅ (g)→ IF₃(g)+ F₂(g) Is ________ kJ,give the data below. IF (g)+ F₂(g)→ IF₃(g)ΔH = -390 kJ IF (g)+ 2F₂ (g)→ IF₅ (g)ΔH = -745 kJ A)+355 B)-1135 C)+1135 D)+35 E)-35

Question

Quizplus · Accepted Answer

To find the ΔH for the given reaction, we can manipulate the given reactions to match the target reaction. The target reaction is the decomposition of $\text{IF}_5$ into $\text{IF}_3$ and $\text{F}_2$. Given reactions:1. $\text{IF} + \text{F}_2 \rightarrow \text{IF}_3; \Delta H = -390 \, \text{kJ}$2. $\text{IF} + 2\text{F}_2 \rightarrow \text{IF}_5; \Delta H = -745 \, \text{kJ}$To get the target reaction from the given ones, we can reverse reaction 2 and subtract reaction 1 from it:- Reverse reaction 2 (to decompose $\text{IF}_5$): $\text{IF}_5 \rightarrow \text{IF} + 2\text{F}_2; \Delta H = +745 \, \text{kJ}$- Subtract reaction 1: $\text{IF} + \text{F}_2 \rightarrow \text{IF}_3; \Delta H = -390 \, \text{kJ}$So, the net reaction is: $\text{IF}_5 \rightarrow \text{IF}_3 + \text{F}_2$, and the net $\Delta H$ is $+745 \, \text{kJ} - 390 \, \text{kJ} = +355 \, \text{kJ}$.

ΔH for the Reaction IF5 (G)→ IF3 (g)+ F2 (g)

ΔH for the Reaction IF₅ (G)→ IF₃(g)+ F₂(g)