Calculate AH for the reaction NH3 (g) + CH4 (g) → HCN (g) + 3 H2 (g), from the following data. N2 (g) + 3 H2 (g) → 2 NH3 (g) / mol AH 91.8 kJ C (s, graphite) + 2 H2 (g) → CH, (g) - 74. 9 kJ / mol ΔΗ- 2 C (s, graphite) + H2 (g) + N2 (g) → 2 HCN (g) ΔΗ 270. 3 kJ / mol

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The image consists of a multiple-choice selection with four options, each indicating a value in kilojoules (kJ):

- ○ 437.0 kJ
- ○ 256.0 kJ
- ○ 103.6 kJ
- ○ -103.6 kJ

There are no graphs or diagrams present in the image.
Transcribed Image Text:The image consists of a multiple-choice selection with four options, each indicating a value in kilojoules (kJ): - ○ 437.0 kJ - ○ 256.0 kJ - ○ 103.6 kJ - ○ -103.6 kJ There are no graphs or diagrams present in the image.
**Calculate ΔH for the reaction:**

\[ \text{NH}_3 \, (g) + \text{CH}_4 \, (g) \rightarrow \text{HCN} \, (g) + 3 \, \text{H}_2 \, (g) \]

Using the following data:

1. \[ \text{N}_2 \, (g) + 3 \, \text{H}_2 \, (g) \rightarrow 2 \, \text{NH}_3 \, (g) \quad \Delta H = -91.8 \, \text{kJ/mol} \]

2. \[ \text{C} \, (s, \, \text{graphite}) + 2 \, \text{H}_2 \, (g) \rightarrow \text{CH}_4 \, (g) \quad \Delta H = -74.9 \, \text{kJ/mol} \]

3. \[ 2 \, \text{C} \, (s, \, \text{graphite}) + \text{H}_2 \, (g) + \text{N}_2 \, (g) \rightarrow 2 \, \text{HCN} \, (g) \quad \Delta H = 270.3 \, \text{kJ/mol} \]

**Explanation:**

The goal is to calculate the enthalpy change (ΔH) for the reaction between ammonia \((\text{NH}_3)\) and methane \((\text{CH}_4)\) to form hydrogen cyanide \((\text{HCN})\) and hydrogen gas \((\text{H}_2)\), using the provided thermochemical data for related reactions.

To determine ΔH for the target reaction, you may need to manipulate and combine the given equations using Hess's law.
Transcribed Image Text:**Calculate ΔH for the reaction:** \[ \text{NH}_3 \, (g) + \text{CH}_4 \, (g) \rightarrow \text{HCN} \, (g) + 3 \, \text{H}_2 \, (g) \] Using the following data: 1. \[ \text{N}_2 \, (g) + 3 \, \text{H}_2 \, (g) \rightarrow 2 \, \text{NH}_3 \, (g) \quad \Delta H = -91.8 \, \text{kJ/mol} \] 2. \[ \text{C} \, (s, \, \text{graphite}) + 2 \, \text{H}_2 \, (g) \rightarrow \text{CH}_4 \, (g) \quad \Delta H = -74.9 \, \text{kJ/mol} \] 3. \[ 2 \, \text{C} \, (s, \, \text{graphite}) + \text{H}_2 \, (g) + \text{N}_2 \, (g) \rightarrow 2 \, \text{HCN} \, (g) \quad \Delta H = 270.3 \, \text{kJ/mol} \] **Explanation:** The goal is to calculate the enthalpy change (ΔH) for the reaction between ammonia \((\text{NH}_3)\) and methane \((\text{CH}_4)\) to form hydrogen cyanide \((\text{HCN})\) and hydrogen gas \((\text{H}_2)\), using the provided thermochemical data for related reactions. To determine ΔH for the target reaction, you may need to manipulate and combine the given equations using Hess's law.
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