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.

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Chapter1: Chemical Foundations
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Please help with number 8. Thank you
the total gas mixture is compressed to a pressure of 5.2 atm before combustion, calculate the total
volume 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 is
78% nitrogen and 22% oxygen. If you breathe in 3.2 grams of air at 1.3 atm and 26 °C, do you
completely fill your lungs with air?
7.
Calculate the partial pressure of nitrogen and oxygen in a mixture of 35.8 grams of
nitrogen gas and 28.3 grams s of oxygen gas
in a 1.65 L container at 42 °C.
8)
atm. The
An unsealed 450.0 mL beaker contains 320mL of a very dense gas at 52 °C and 3.12
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.
beaker?
b.
At constant temperature, what pressure is required for the gas to fill the beaker?
Transcribed Image Text:the total gas mixture is compressed to a pressure of 5.2 atm before combustion, calculate the total volume 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 is 78% nitrogen and 22% oxygen. If you breathe in 3.2 grams of air at 1.3 atm and 26 °C, do you completely fill your lungs with air? 7. Calculate the partial pressure of nitrogen and oxygen in a mixture of 35.8 grams of nitrogen gas and 28.3 grams s of oxygen gas in a 1.65 L container at 42 °C. 8) atm. The An unsealed 450.0 mL beaker contains 320mL of a very dense gas at 52 °C and 3.12 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. beaker? b. At constant temperature, what pressure is required for the gas to fill the beaker?
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