Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Concept explainers

Thermochemistry
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Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energ…
Question
Sure! Below is a transcription of the image content suitable for an educational website: --- ### Balancing Chemical Equations and Calculating Enthalpy Change **Question a:** Write a balanced chemical equation for the formation of 1 mol of \( \text{Cr}_2\text{O}_3(s) \) from Cr and \( \text{O}_2 \) in their standard states. > **Instructions:** Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank. If no reaction occurs, leave all boxes blank and click on Submit. **Balanced Equation:** \[ 2\text{Cr (s)} + \frac{3}{2} \text{O}_2 \text{(g)} \rightarrow \text{Cr}_2\text{O}_3 \text{(s)} \] **Status:** Correct The equation of the formation of \( \text{Cr}_2\text{O}_3(s) \) from the elements: \[ 2 \text{Cr (s)} + \frac{3}{2} \text{O}_2 \text{(g)} \rightarrow \text{Cr}_2\text{O}_3 \text{(s)} \] --- **Question b:** What is the enthalpy change if 3.1 g of chromium is oxidized to \( \text{Cr}_2\text{O}_3(s) \)? > \(\Delta_f H^\circ\) for \( \text{Cr}_2\text{O}_3 \text{(s)} = -1134.7 \, \text{kJ/mol} \) **Enthalpy Change:** \[ \text{Enthalpy change} = \_\_\_ \, \text{kJ} \] **Options:** - **Submit** - **Submit Answer** - **Try Another Version** - **10 item attempts remaining** *Controls:* - Previous - Next - Email Instructor - Save and Exit --- This exercise involves balancing a chemical reaction and calculating the enthalpy change based on the given data. Ensure to input your calculations accurately to determine the enthalpy change.
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Transcribed Image Text:Sure! Below is a transcription of the image content suitable for an educational website: --- ### Balancing Chemical Equations and Calculating Enthalpy Change **Question a:** Write a balanced chemical equation for the formation of 1 mol of \( \text{Cr}_2\text{O}_3(s) \) from Cr and \( \text{O}_2 \) in their standard states. > **Instructions:** Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank. If no reaction occurs, leave all boxes blank and click on Submit. **Balanced Equation:** \[ 2\text{Cr (s)} + \frac{3}{2} \text{O}_2 \text{(g)} \rightarrow \text{Cr}_2\text{O}_3 \text{(s)} \] **Status:** Correct The equation of the formation of \( \text{Cr}_2\text{O}_3(s) \) from the elements: \[ 2 \text{Cr (s)} + \frac{3}{2} \text{O}_2 \text{(g)} \rightarrow \text{Cr}_2\text{O}_3 \text{(s)} \] --- **Question b:** What is the enthalpy change if 3.1 g of chromium is oxidized to \( \text{Cr}_2\text{O}_3(s) \)? > \(\Delta_f H^\circ\) for \( \text{Cr}_2\text{O}_3 \text{(s)} = -1134.7 \, \text{kJ/mol} \) **Enthalpy Change:** \[ \text{Enthalpy change} = \_\_\_ \, \text{kJ} \] **Options:** - **Submit** - **Submit Answer** - **Try Another Version** - **10 item attempts remaining** *Controls:* - Previous - Next - Email Instructor - Save and Exit --- This exercise involves balancing a chemical reaction and calculating the enthalpy change based on the given data. Ensure to input your calculations accurately to determine the enthalpy change.
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