Concept explainers
Interpretation:
The final pressure when the gas, which initially occupied
Concept Introduction:
The final pressure of the gas at the constant temperature can be calculated using Boyle’s law, which states the relationship between pressure and volume of the gas. According to Boyle’s Law, the volume of fixed amount of gas is inversely proportional to the pressure of the gas at constant temperature. Mathematically, it is given as.
We two different sets of volume and pressure of the gas is considered, the above equation becomes as follows:
where
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Chapter 5 Solutions
Introduction to General, Organic and Biochemistry
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- TUTOR Using the Ideal Gas Law to Calculate Molar Mass A 1.61-g sample of an unknown gas has a volume of 651 mL and a pressure of 672 mmHg at 38.8 °C. Calculate the molar mass of this compound. 33.0 X g/mol Resubmit Show Approach Show Tutor Stepsarrow_forwardA sample of oxygen gas at a pressure of 1.16 atm and a temperature of 27.4 °C, occupies a volume of 13.3 liters. If the gas is allowed to expand at constant temperature to a volume of 21.2 liters, the pressure of the gas sample will be atm. Submit Answer Try Another Version 10 item attempts remainingarrow_forwardPart A A weather balloon is inflated to a volume of 25.5 L at a pressure of 738 mmHg and a temperature of 31.4 °C. The balloon rises in the atmosphere to an altitude where the pressure is 390. mmHg and the temperature is -15.6 °C. Assuming the balloon can freely expand, calculate the volume of the balloon at this altitude. a) ? Vballoon = L Submit Request Answer What is the pressure if the volume of the container is maintained constant and the temperature is raised to 331 °C? Express the pressure in atmospheres to three significant figures. ΑΣφ. P = atm Submit Request Answer What is the density (in g/L) of hydrogen gas at 20 °C and a pressure of 1655 psi? Express your answer in grams per liter to three significant figures. • View Available Hint(s) Πνα ΑΣφ d = g/L Submitarrow_forward
- QUESTION 8 At 16.29 °C and 2.869 atm, a gas occupies a volume of 15.98 L. What volume would it occupy at -66.66 °C and 2.047 atm? Assume ideal gas behavior. Key Concept:The ideal gas law states that PV = nRT, where R is a constant. Strategy: From ideal gas law we know P 1*V 1/T 1 = P 2*V 2/T 2arrow_forwardLReferences) Use the References to access important values if needed for this question. A sample of neon gas occupies a volume of 8.67 L at 56.0°C and 0.640 atm If it is desired to increase the volume of the gas sample to 10.6 L, while decreasing its pressure to 0.389 atm, the temperature of the gas sample at the new volume and pressure must be PC. Submit Answer Try Another Version 3 item attempts remainingarrow_forwardCheck m A sample of gas occuples 3.17 L at a pressure of 6.13 atm. Determine the new pressure (in atm) of the sample when the volume changes to 8.06 L at constant temperature. atmarrow_forward
- Attempt 2 A flexible container at an initial volume of 8.15 L8.15 L contains 7.51 mol7.51 mol of gas. More gas is then added to the container until it reaches a final volume of 12.5 L.12.5 L. Assuming the pressure and temperature of the gas remain constant, calculate the number of moles of gas added to the container.arrow_forwardA sample of methane gas at a pressure of 1.09 atm and a temperature of 262 °C, occupies a volume of 548 mL. If the gas is heated at constant pressure until its volume is 810 mL, the temperature of the gas sample will be °C. Submit Answer Retry Entire Group 9 more group attempts remainingarrow_forward[References] Use the References to access important values if needed for this question. A sample of neon gas occupies a volume of 8.84 L at 48.0°C and 1.28 atm. If it is desired to increase the volume of the gas sample to 10.1 L, while decreasing its pressure to 0.904 atm, the temperature of the gas sample at the new volume and pressure must be °C. Submit Answer Try Another Version 1 item attempt remaining Previous Next 10 MAR 10 27 étv 280 MacBook Airarrow_forward
- Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning