**Thermochemistry Problem: Enthalpy Change Calculation****Problem Statement:**Consider the following chemical reaction:\[ \text{C(s) + O}_2\text{(g)} \rightarrow \text{CO}_2\text{(g)} \]The standard enthalpy change (\(\Delta H^\circ\)) for this reaction is \(-393.5 \, \text{kJ/mol}\).Calculate the heat change if 2.54 g of carbon (C) is reacted.**Solution Box:**[Type your answer here]**Explanation:**To solve this problem, you need to:1. Determine the number of moles of carbon in 2.54 g. - Use the molar mass of carbon, which is approximately 12.01 g/mol.2. Use the moles of carbon and the given enthalpy change to calculate the heat change for the reaction. This calculation will require you to set up a proportion since \(-393.5 \, \text{kJ}\) is released per mole of carbon reacted.

The given reaction is: C(s)+O2(g)→CO2(g) ∆H°=-393.5 kJ Calculation of no. of mol of C: No. of…

Answered: C (s) + 02 (g) → CO2 (g) AH° = -393.5…

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C (s) + 02 (g) → CO2 (g) AH° = -393.5 kJ Calculate the heat change if 2.54 g of C is reacted.

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

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Question

**Thermochemistry Problem: Enthalpy Change Calculation**

**Problem Statement:**
Consider the following chemical reaction:

\[ \text{C(s) + O}_2\text{(g)} \rightarrow \text{CO}_2\text{(g)} \]

The standard enthalpy change (\(\Delta H^\circ\)) for this reaction is \(-393.5 \, \text{kJ/mol}\).

Calculate the heat change if 2.54 g of carbon (C) is reacted.

**Solution Box:**
[Type your answer here]

**Explanation:**

To solve this problem, you need to:

1. Determine the number of moles of carbon in 2.54 g.
- Use the molar mass of carbon, which is approximately 12.01 g/mol.

2. Use the moles of carbon and the given enthalpy change to calculate the heat change for the reaction.

This calculation will require you to set up a proportion since \(-393.5 \, \text{kJ}\) is released per mole of carbon reacted.

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