Please help with number 8. Thank you the total gas mixture is compressed to a pressure of 5.2 atm before combustion, calculate the totalvolume of the gas mixture at this point in time.6.Consider that the average lung can hold about 6 liters of air and the composition of air is78% nitrogen and 22% oxygen. If you breathe in 3.2 grams of air at 1.3 atm and 26 °C, do youcompletely fill your lungs with air?7.Calculate the partial pressure of nitrogen and oxygen in a mixture of 35.8 grams ofnitrogen gas and 28.3 grams s of oxygen gasin a 1.65 L container at 42 °C.8)atm. TheAn unsealed 450.0 mL beaker contains 320mL of a very dense gas at 52 °C and 3.12gas is much denser than the surrounding air, so it does not disperse into the air.At constant pressure, what would the temperature have to reach for the gas to fill thea.beaker?b.At constant temperature, what pressure is required for the gas to fill the beaker?

Answer-8 When at constant pressure, temperature of the gas is increased its volume also increases…

8) An unsealed 450.0 mL beaker contains 320mL of a very dense gas at 52 °C and 3.12 atm. The gas is much denser than the surrounding air, so it does not disperse into the air. At constant pressure, what would the temperature have to reach for the gas to fill the a. At constant temperature, what pressure is required for the gas to fill the beaker? beaker? b.

8) An unsealed 450.0 mL beaker contains 320mL of a very dense gas at 52 °C and 3.12 atm. The gas is much denser than the surrounding air, so it does not disperse into the air. At constant pressure, what would the temperature have to reach for the gas to fill the a. At constant temperature, what pressure is required for the gas to fill the beaker? beaker? b.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter8: Gases

Section: Chapter Questions

Problem 31Q

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