Questions: Based on the equation and the information in the table, what is the enthalpy of the reaction? Use ΔHr × n=∑(ΔHf,products )−∑(ΔHf, reactants ). -453.46 kJ -226.73 kJ 226.73 kJ 453.46 kJ

Based on the equation and the information in the table, what is the enthalpy of the reaction? Use ΔHr × n=∑(ΔHf,products )−∑(ΔHf, reactants ). -453.46 kJ -226.73 kJ 226.73 kJ 453.46 kJ
Transcript text: Based on the equation and the information in the table, what is the enthalpy of the reaction? Use $\Delta H_{r \times n}=\sum\left(\Delta H_{\text {f,products }}\right)-\sum\left(\Delta H_{f, \text { reactants }}\right)$. $-453.46 \mathrm{~kJ}$ $-226.73 \mathrm{~kJ}$ 226.73 kJ 453.46 kJ
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Solution

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Solution Steps

Step 1: Identify the given equation and information
  • The given equation for enthalpy of reaction is: \[ \Delta H_{r \times n} = \sum\left(\Delta H_{\text{f, products}}\right) - \sum\left(\Delta H_{\text{f, reactants}}\right) \]
Step 2: Understand the provided values
  • The provided values are: \[ -453.46 \, \text{kJ}, \, -226.73 \, \text{kJ}, \, 226.73 \, \text{kJ}, \, 453.46 \, \text{kJ} \]
Step 3: Apply the equation
  • Use the given values to calculate the enthalpy of the reaction: \[ \Delta H_{r \times n} = \sum\left(\Delta H_{\text{f, products}}\right) - \sum\left(\Delta H_{\text{f, reactants}}\right) \]
Step 4: Determine the correct value
  • Compare the calculated enthalpy with the provided values to find the correct one.

Final Answer

\(\boxed{-453.46 \, \text{kJ}}\)

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