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2) A piece of dry ice (solid CO,) with a mass of 28.8 g sublimes (converts from solid to gas) into a large balloon. Assuming that all of the CO, ends up in the balloon, what is the volume of the balloon at 22°C at a pressure of 742 mm Hg?

2) A piece of dry ice (solid CO,) with a mass of 28.8 g sublimes (converts from solid to gas) into a large balloon. Assuming that all of the CO, ends up in the balloon, what is the volume of the balloon at 22°C at a pressure of 742 mm Hg?

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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**Gas Law Problems** **Problem 1:** An 8.50 L tire contains 0.552 mol of gas at a temperature of 305 K. What is the pressure (in atm) of the gas in the tire? **Problem 2:** A piece of dry ice (solid CO₂) with a mass of 28.8 g sublimes (converts from solid to gas) into a large balloon. Assuming that all of the CO₂ ends up in the balloon, what is the volume of the balloon at 22°C at a pressure of 742 mm Hg? (Note: For both problems, the Ideal Gas Law \(PV = nRT\) may be used, where: - P = Pressure - V = Volume - n = Number of moles - R = Ideal Gas Constant (0.0821 atm·L/mol·K) - T = Temperature in Kelvin) Feel free to click on the links for detailed step-by-step solutions and explanations for each problem. --- The page does not contain any graphs or diagrams.
Transcribed Image Text:**Gas Law Problems** **Problem 1:** An 8.50 L tire contains 0.552 mol of gas at a temperature of 305 K. What is the pressure (in atm) of the gas in the tire? **Problem 2:** A piece of dry ice (solid CO₂) with a mass of 28.8 g sublimes (converts from solid to gas) into a large balloon. Assuming that all of the CO₂ ends up in the balloon, what is the volume of the balloon at 22°C at a pressure of 742 mm Hg? (Note: For both problems, the Ideal Gas Law \(PV = nRT\) may be used, where: - P = Pressure - V = Volume - n = Number of moles - R = Ideal Gas Constant (0.0821 atm·L/mol·K) - T = Temperature in Kelvin) Feel free to click on the links for detailed step-by-step solutions and explanations for each problem. --- The page does not contain any graphs or diagrams.
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