Question
Use the information in the table to answer the question.%0D%0A%0D%0ABond%09Bond Energy (kJ/mol)%0D%0AH–Cl%09427%0D%0ACl–Cl%09242%0D%0AH–H%09435%0D%0AHydrogen and chlorine gases react to produce hydrochloric acid according to the reaction.%0D%0A%0D%0AH2+Cl2→2HCl%0D%0A%0D%0AHow much total bond energy, in kJ/mol, is in the products of the reaction?%0D%0A%0D%0A(1 point)%0D%0AResponses%0D%0A%0D%0A435%0D%0A435%0D%0A%0D%0A427%0D%0A427%0D%0A%0D%0A854%0D%0A854%0D%0A%0D%0A677
Answers
GPT-4o mini
To find the total bond energy in the products of the reaction \( H_2 + Cl_2 \rightarrow 2HCl \), we need to consider the bonds formed in the products.
Each molecule of \( HCl \) contains one \( H–Cl \) bond. Since the reaction produces 2 moles of \( HCl \), there will be a total of 2 \( H–Cl \) bonds formed.
The bond energy of the \( H–Cl \) bond is given as 427 kJ/mol. Therefore, for 2 moles of \( HCl \), the total bond energy in the products is calculated as follows:
\[
\text{Total Bond Energy} = 2 \times \text{Bond Energy of H–Cl}
\]
\[
\text{Total Bond Energy} = 2 \times 427 \, \text{kJ/mol} = 854 \, \text{kJ/mol}
\]
Thus, the total bond energy in the products of the reaction is **854 kJ/mol**.
Each molecule of \( HCl \) contains one \( H–Cl \) bond. Since the reaction produces 2 moles of \( HCl \), there will be a total of 2 \( H–Cl \) bonds formed.
The bond energy of the \( H–Cl \) bond is given as 427 kJ/mol. Therefore, for 2 moles of \( HCl \), the total bond energy in the products is calculated as follows:
\[
\text{Total Bond Energy} = 2 \times \text{Bond Energy of H–Cl}
\]
\[
\text{Total Bond Energy} = 2 \times 427 \, \text{kJ/mol} = 854 \, \text{kJ/mol}
\]
Thus, the total bond energy in the products of the reaction is **854 kJ/mol**.