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10) A tank of nitrogen has a volume of 10.0 L and a pressure of 760.0 mm Hg. Find the volume of the nitrogen when its pressure is changed to 0.526 atm while the temperature is held constant. a) 1L b) 19L c) 14,449L d) 0.0526 L

10) A tank of nitrogen has a volume of 10.0 L and a pressure of 760.0 mm Hg. Find the volume of the nitrogen when its pressure is changed to 0.526 atm while the temperature is held constant. a) 1L b) 19L c) 14,449L d) 0.0526 L

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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--- ### Ideal Gas Law Application **Problem 10:** A tank of nitrogen has a volume of 10.0 L and a pressure of 760.0 mm Hg. Find the volume of the nitrogen when its pressure is changed to 0.526 atm while the temperature is held constant. **Options:** a) 1L b) 19L c) 14.449L d) 0.0526L This problem can be solved using Boyle's Law, which states that for a given mass of gas at constant temperature, the product of the pressure and volume remains constant (P1V1 = P2V2). **Explanation for Solving the Problem:** 1. Convert the initial pressure into the same units as the final pressure if needed: - Initial pressure P1 = 760.0 mm Hg - 1 atm = 760 mm Hg - Therefore, P1 = 1 atm 2. Identify the known values: - Initial pressure, P1 = 1 atm - Initial volume, V1 = 10.0 L - Final pressure, P2 = 0.526 atm - Final volume, V2 = ? 3. Use Boyle’s Law (P1V1 = P2V2): - (1 atm) * (10.0 L) = (0.526 atm) * V2 - V2 = (1 * 10.0) / 0.526 - V2 ≈ 19 L So the answer is **b) 19L**. --- Make sure to consider the units you’re working with and apply the correct gas laws based on the problem context, ensuring consistency with constants and derived formulae.
Transcribed Image Text:--- ### Ideal Gas Law Application **Problem 10:** A tank of nitrogen has a volume of 10.0 L and a pressure of 760.0 mm Hg. Find the volume of the nitrogen when its pressure is changed to 0.526 atm while the temperature is held constant. **Options:** a) 1L b) 19L c) 14.449L d) 0.0526L This problem can be solved using Boyle's Law, which states that for a given mass of gas at constant temperature, the product of the pressure and volume remains constant (P1V1 = P2V2). **Explanation for Solving the Problem:** 1. Convert the initial pressure into the same units as the final pressure if needed: - Initial pressure P1 = 760.0 mm Hg - 1 atm = 760 mm Hg - Therefore, P1 = 1 atm 2. Identify the known values: - Initial pressure, P1 = 1 atm - Initial volume, V1 = 10.0 L - Final pressure, P2 = 0.526 atm - Final volume, V2 = ? 3. Use Boyle’s Law (P1V1 = P2V2): - (1 atm) * (10.0 L) = (0.526 atm) * V2 - V2 = (1 * 10.0) / 0.526 - V2 ≈ 19 L So the answer is **b) 19L**. --- Make sure to consider the units you’re working with and apply the correct gas laws based on the problem context, ensuring consistency with constants and derived formulae.
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