Determine the heat of reaction for 2 OF2 (g) + 2 S (s) → SO₂ (g) + SF4 (9) given the heats of reaction for the following reactions OF2 (g) + H₂O (1)→ O₂ (g) + 2 HF (g) SF4 (9) + 2 H₂O (1) 4 HF (g) + SO₂ (8) S (s) + O₂(g) → SO₂ (g) ArxnHo = -276.6 kJ/mol ArxnH = -827.5 kJ/mol ArxnHo = -296.9 kJ/mol

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**Determine the Heat of Reaction**

Calculate the heat of reaction for the following chemical equation:

\[ 2 \text{OF}_2 (g) + 2 \text{S} (s) \rightarrow \text{SO}_2 (g) + \text{SF}_4 (g) \]

Given the heats of reaction for these related processes:

1. \(\text{OF}_2 (g) + \text{H}_2\text{O} (l) \rightarrow \text{O}_2 (g) + 2 \text{HF} (g) \)  
   \(\Delta_{rxn}H^\circ = -276.6 \, \text{kJ/mol}\)

2. \(\text{SF}_4 (g) + 2 \text{H}_2\text{O} (l) \rightarrow 4 \text{HF} (g) + \text{SO}_2 (g) \)  
   \(\Delta_{rxn}H^\circ = -827.5 \, \text{kJ/mol}\)

3. \(\text{S} (s) + \text{O}_2 (g) \rightarrow \text{SO}_2 (g) \)  
   \(\Delta_{rxn}H^\circ = -296.9 \, \text{kJ/mol}\)

**Explanation of Reactions:**

- The first reaction involves the decomposition of oxygen difluoride (\(\text{OF}_2\)) and water (\(\text{H}_2\text{O}\)) to produce oxygen (\(\text{O}_2\)) and hydrogen fluoride (\(\text{HF}\)), releasing \(-276.6 \, \text{kJ/mol}\) of energy.

- The second reaction describes the hydrolysis of sulfur tetrafluoride (\(\text{SF}_4\)), which reacts with water to form hydrogen fluoride and sulfur dioxide (\(\text{SO}_2\)), releasing \(-827.5 \, \text{kJ/mol}\).

- The third reaction depicts the combustion of sulfur (\(\text{S}\)) in oxygen to form sulfur dioxide, releasing \(-296.9 \, \text{kJ/mol}\).

These reactions are used to calculate the overall heat of reaction for the given chemical equation.
Transcribed Image Text:**Determine the Heat of Reaction** Calculate the heat of reaction for the following chemical equation: \[ 2 \text{OF}_2 (g) + 2 \text{S} (s) \rightarrow \text{SO}_2 (g) + \text{SF}_4 (g) \] Given the heats of reaction for these related processes: 1. \(\text{OF}_2 (g) + \text{H}_2\text{O} (l) \rightarrow \text{O}_2 (g) + 2 \text{HF} (g) \) \(\Delta_{rxn}H^\circ = -276.6 \, \text{kJ/mol}\) 2. \(\text{SF}_4 (g) + 2 \text{H}_2\text{O} (l) \rightarrow 4 \text{HF} (g) + \text{SO}_2 (g) \) \(\Delta_{rxn}H^\circ = -827.5 \, \text{kJ/mol}\) 3. \(\text{S} (s) + \text{O}_2 (g) \rightarrow \text{SO}_2 (g) \) \(\Delta_{rxn}H^\circ = -296.9 \, \text{kJ/mol}\) **Explanation of Reactions:** - The first reaction involves the decomposition of oxygen difluoride (\(\text{OF}_2\)) and water (\(\text{H}_2\text{O}\)) to produce oxygen (\(\text{O}_2\)) and hydrogen fluoride (\(\text{HF}\)), releasing \(-276.6 \, \text{kJ/mol}\) of energy. - The second reaction describes the hydrolysis of sulfur tetrafluoride (\(\text{SF}_4\)), which reacts with water to form hydrogen fluoride and sulfur dioxide (\(\text{SO}_2\)), releasing \(-827.5 \, \text{kJ/mol}\). - The third reaction depicts the combustion of sulfur (\(\text{S}\)) in oxygen to form sulfur dioxide, releasing \(-296.9 \, \text{kJ/mol}\). These reactions are used to calculate the overall heat of reaction for the given chemical equation.
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