### Thermochemical Equation and Heat Change Calculation#### Thermochemical Equation:\[ \text{C(s) + O}_2\text{(g)} \rightarrow \text{CO}_2\text{(g)} \quad \Delta H^\circ = -393.5 \, \text{kJ} \]#### Problem Statement:Calculate the heat change if 2.54 g of C is reacted.### ExplanationThis image provides a thermochemical equation representing the combustion of carbon (C) in the presence of oxygen (O₂) to form carbon dioxide (CO₂). The equation specifies that the reaction releases 393.5 kJ of energy per mole of carbon reacted, indicated by the negative sign in \(\Delta H^\circ = -393.5 \, \text{kJ}\).#### Strategy to Solve:1. **Find Molar Mass of Carbon (C):** \[ \text{Molar mass of C} = 12.01 \, \text{g/mol} \]2. **Calculate Moles of Carbon:** \[ \text{Moles of C} = \frac{\text{Mass of C}}{\text{Molar mass of C}} \] \[ \text{Moles of C} = \frac{2.54 \, \text{g}}{12.01 \, \text{g/mol}} \approx 0.2115 \, \text{mol} \]3. **Calculate the Heat Change:** \[ \Delta H = (\text{Moles of C}) \times (\Delta H^\circ \, \text{per mole of C}) \] \[ \Delta H = 0.2115 \, \text{mol} \times (-393.5 \, \text{kJ/mol}) \] \[ \Delta H \approx -83.25 \, \text{kJ} \]### ConclusionIf 2.54 g of carbon are reacted, the heat change for the reaction is approximately \(-83.25 \, \text{kJ}\). This indicates that 83.25 kJ of energy would be released.

Given information, ∆H° ( for 1 mole of C(s)) = -393.5 kJ Mass of C(s) reacted = 2.54 g Molar mass of…

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

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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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