**Chemical Reaction and Enthalpy Change**A chemist measures the enthalpy change \(\Delta H\) during the following reaction:\[ 2 \text{Na}(s) + \text{Cl}_2(g) \rightarrow 2 \text{NaCl}(s) \]\[\Delta H = -822 \, \text{kJ}\]**Task:**Use this information to complete the table below. Round each of your answers to the nearest kJ/mol.| Reaction | \(\Delta H\) ||-----------------------------------------------------|----------------|| \(2 \text{Na}(s) + \text{Cl}_2(g) \rightarrow 2 \text{NaCl}(s)\) | \(\text{[ ] kJ}\) || \(4 \text{Na}(s) + 2 \text{Cl}_2(g) \rightarrow 4 \text{NaCl}(s)\) | \(\text{[ ] kJ}\) || \(\text{NaCl}(s) \rightarrow \text{Na}(s) + \frac{1}{2} \text{Cl}_2(g)\) | \(\text{[ ] kJ}\) |**Calculation Explanation:** To solve this, consider the stoichiometry of each reaction compared to the initial reaction and apply it to the given \(\Delta H\).

Answered: A chemist measures the enthalpy change…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

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**Chemical Reaction and Enthalpy Change**

A chemist measures the enthalpy change \(\Delta H\) during the following reaction:

\[ 2 \text{Na}(s) + \text{Cl}_2(g) \rightarrow 2 \text{NaCl}(s) \]

\[\Delta H = -822 \, \text{kJ}\]

**Task:**

Use this information to complete the table below. Round each of your answers to the nearest kJ/mol.

| Reaction | \(\Delta H\) |
|-----------------------------------------------------|----------------|
| \(2 \text{Na}(s) + \text{Cl}_2(g) \rightarrow 2 \text{NaCl}(s)\) | \(\text{[ ] kJ}\) |
| \(4 \text{Na}(s) + 2 \text{Cl}_2(g) \rightarrow 4 \text{NaCl}(s)\) | \(\text{[ ] kJ}\) |
| \(\text{NaCl}(s) \rightarrow \text{Na}(s) + \frac{1}{2} \text{Cl}_2(g)\) | \(\text{[ ] kJ}\) |

**Calculation Explanation:**

To solve this, consider the stoichiometry of each reaction compared to the initial reaction and apply it to the given \(\Delta H\).

Expert Solution

Step 1

The thermochemical equations can be treated as algebraic equation which can be added, subtracted, multiplied or divided.

i.e.

If the coefficient of the substances are multiplied or divided by some number then the value of ∆H is multiplied or divided by the same number.
If the reaction is reversed then the sign of ∆H changes but the magnitude remains the same.

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