Calculate AHrxn for the following reaction: 5C(s) + 6H2 (g) → C;H12 (1) Use the following reactions and given AH values: C5 H12(1) + 802 (g) → 5CO2(g) +6H2O(g), C(s) + O2 (g) → CO2(g), 2H2 (g) + O2 (g) → 2H2O(g), ΔΗ -3244.8 kJ ΔΗ -393.5 kJ ΔΗ -483.5 kJ Express your answer to four significant figures in kilojoules.

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### Calculating the Enthalpy Change for a Chemical Reaction

#### Problem Statement
Calculate the \( \Delta H_{\text{rxn}} \) for the following reaction:
\[ 5C(s) + 6H_2(g) \rightarrow C_5H_{12}(l) \]

#### Given Data
Use the following reactions and their given \( \Delta H \) values:

1. \( C_5H_{12}(l) + 8O_2(g) \rightarrow 5CO_2(g) + 6H_2O(g) \)
   - \( \Delta H = -3244.8 \, \text{kJ} \)

2. \( C(s) + O_2(g) \rightarrow CO_2(g) \)
   - \( \Delta H = -393.5 \, \text{kJ} \)

3. \( 2H_2(g) + O_2(g) \rightarrow 2H_2O(g) \)
   - \( \Delta H = -483.5 \, \text{kJ} \)

#### Task
Express your answer to four significant figures in kilojoules.

#### Explanation Method
To find the enthalpy change for the desired reaction, we can use Hess's Law. Hess's Law states that if a reaction is carried out in a series of steps, the \( \Delta H \) for the overall reaction is the sum of the \( \Delta H \) values for each individual step.

The given reactions and \( \Delta H \) values can be used to form the target reaction. 

1. **Combustion of \( C_5H_{12} \)**:
   \[ C_5H_{12}(l) + 8O_2(g) \rightarrow 5CO_2(g) + 6H_2O(g) \]
   \[ \Delta H = -3244.8 \, \text{kJ} \]

2. **Formation of \( CO_2 \) from Carbon**:
   \[ 5C(s) + 5O_2(g) \rightarrow 5CO_2(g) \]
   \[ \Delta H = 5 \times (-393.5 \, \text{kJ}) = -1967.5 \, \text{kJ} \]

3. **Formation of
Transcribed Image Text:### Calculating the Enthalpy Change for a Chemical Reaction #### Problem Statement Calculate the \( \Delta H_{\text{rxn}} \) for the following reaction: \[ 5C(s) + 6H_2(g) \rightarrow C_5H_{12}(l) \] #### Given Data Use the following reactions and their given \( \Delta H \) values: 1. \( C_5H_{12}(l) + 8O_2(g) \rightarrow 5CO_2(g) + 6H_2O(g) \) - \( \Delta H = -3244.8 \, \text{kJ} \) 2. \( C(s) + O_2(g) \rightarrow CO_2(g) \) - \( \Delta H = -393.5 \, \text{kJ} \) 3. \( 2H_2(g) + O_2(g) \rightarrow 2H_2O(g) \) - \( \Delta H = -483.5 \, \text{kJ} \) #### Task Express your answer to four significant figures in kilojoules. #### Explanation Method To find the enthalpy change for the desired reaction, we can use Hess's Law. Hess's Law states that if a reaction is carried out in a series of steps, the \( \Delta H \) for the overall reaction is the sum of the \( \Delta H \) values for each individual step. The given reactions and \( \Delta H \) values can be used to form the target reaction. 1. **Combustion of \( C_5H_{12} \)**: \[ C_5H_{12}(l) + 8O_2(g) \rightarrow 5CO_2(g) + 6H_2O(g) \] \[ \Delta H = -3244.8 \, \text{kJ} \] 2. **Formation of \( CO_2 \) from Carbon**: \[ 5C(s) + 5O_2(g) \rightarrow 5CO_2(g) \] \[ \Delta H = 5 \times (-393.5 \, \text{kJ}) = -1967.5 \, \text{kJ} \] 3. **Formation of
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