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Calculate the heat, in kJ, that would be involved in condensing 18.5 g of CH3OH. (AHvap = 38.0 kJ/mol)

Calculate the heat, in kJ, that would be involved in condensing 18.5 g of CH3OH. (AHvap = 38.0 kJ/mol)

Chemistry
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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**Problem Statement:** Calculate the heat, in kJ, that would be involved in condensing 18.5 g of CH₃OH. (ΔHvap = 38.0 kJ/mol) --- **Explanation:** This problem requires calculating the heat released when a certain amount of methanol (CH₃OH) is condensed from its gaseous form to its liquid form. The heat of vaporization (ΔHvap) of methanol is given as 38.0 kJ/mol. **Steps to Solve:** 1. **Determine Moles of CH₃OH:** - Find the molar mass of CH₃OH: - C = 12.01 g/mol - H = 1.01 g/mol × 4 = 4.04 g/mol - O = 16.00 g/mol - Total = 12.01 + 4.04 + 16.00 = 32.05 g/mol - Calculate moles of CH₃OH: - Moles = mass (g) / molar mass (g/mol) - Moles = 18.5 g / 32.05 g/mol 2. **Calculate Heat Involved:** - Use the formula: Heat (kJ) = moles × ΔHvap (kJ/mol)
Transcribed Image Text:**Problem Statement:** Calculate the heat, in kJ, that would be involved in condensing 18.5 g of CH₃OH. (ΔHvap = 38.0 kJ/mol) --- **Explanation:** This problem requires calculating the heat released when a certain amount of methanol (CH₃OH) is condensed from its gaseous form to its liquid form. The heat of vaporization (ΔHvap) of methanol is given as 38.0 kJ/mol. **Steps to Solve:** 1. **Determine Moles of CH₃OH:** - Find the molar mass of CH₃OH: - C = 12.01 g/mol - H = 1.01 g/mol × 4 = 4.04 g/mol - O = 16.00 g/mol - Total = 12.01 + 4.04 + 16.00 = 32.05 g/mol - Calculate moles of CH₃OH: - Moles = mass (g) / molar mass (g/mol) - Moles = 18.5 g / 32.05 g/mol 2. **Calculate Heat Involved:** - Use the formula: Heat (kJ) = moles × ΔHvap (kJ/mol)
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