**Title: Calorimetry Calculation of Benzoic Acid Combustion****Experiment Overview:**A given sample of benzoic acid (C₇H₆O₂), weighing 2.03 grams, is combusted in a constant-volume calorimeter with a heat capacity of 5.93 kJ/°C. The temperature recorded in the calorimeter increases from 24.5 °C to 33.5 °C.**Tasks:**a) **Determining the Amount of Heat Released (in kJ):**To find the amount of heat (q) released, we use the formula:\[ q = C \times \Delta T \]Where:- \( C \) is the heat capacity of the calorimeter.- \( \Delta T \) is the change in temperature.Given:- \( C = 5.93 \) kJ/°C- \( \Delta T = (33.5 - 24.5) °C = 9 °C \)So,\[ q = 5.93 \times 9 = 53.37 \text{ kJ} \]b) **Determining the Molar Energy of Combustion of Benzoic Acid (in kJ/mol):**We need to calculate the molar energy of combustion for benzoic acid. - The molar mass of benzoic acid (C₇H₆O₂) is computed using the periodic table: \[ (\text{7 Carbon} \times 12.01) + (\text{6 Hydrogen} \times 1.01) + (\text{2 Oxygen} \times 16.00) \] \[ = 84.07 + 6.06 + 32.00 \] \[ = 122.13 \text{ g/mol} \]Using the heat released in the earlier calculation:Given sample weight = 2.03 gTo find the heat released per mole:\[ \text{Moles of benzoic acid} = \frac{2.03 \text{ g}}{122.13 \text{ g/mol}} \approx 0.0166 \text{ mol} \]The molar heat of combustion is then:\[ \text{Molar energy (kJ/mol)} = \frac{q}{\text{moles of benzo **Current Attempt in Progress****❌ Incorrect.**Determine the standard enthalpy change for the following reaction:\[ 2 \text{NO(g)} + \text{O}_2(\text{g}) \rightarrow 2 \text{NO}_2(\text{g}) \]\[ \Delta H = 114.14 \text{ kJ} \]**eTextbook and Media**[Save for Later] ### Explanation:The image shows a question from a chemistry problem set asking students to determine the standard enthalpy change for a chemical reaction. The reaction is given as:\[ 2 \text{NO(g)} + \text{O}_2(\text{g}) \rightarrow 2 \text{NO}_2(\text{g}) \]The user input the value "114.14 kJ" as the enthalpy change, but the system marked this answer as incorrect.**Note**: This transcription and analysis are provided for educational purposes to help students understand the type of feedback they might receive when solving enthalpy problems.

Answered: Image /qna-images/answer/a9f4abfa-7a9b-45f2-a5d5-0b8c98377266.jpg

Current Attempt in Progress Your answer is partially correct. A 2.03-g sample of benzoic acid (C,H,O₂) is burned in a constant-volume calorimeter that has a heat capacity of 5.93 kJ/°C. The temperature increases from 24.5 °C to 33.5 °C. a) Determine the amount of heat released (in kJ). 53.37 b) Determine the molar energy of combustion of benzoic acid (in kJ/mol). i 8.9 kJ eTextbook and Media kJ/mol

Current Attempt in Progress Your answer is partially correct. A 2.03-g sample of benzoic acid (C,H,O₂) is burned in a constant-volume calorimeter that has a heat capacity of 5.93 kJ/°C. The temperature increases from 24.5 °C to 33.5 °C. a) Determine the amount of heat released (in kJ). 53.37 b) Determine the molar energy of combustion of benzoic acid (in kJ/mol). i 8.9 kJ eTextbook and Media kJ/mol

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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