1. The partial pressure of O2 in a sample of air on a mountain top is 115 mmHg.

Question

1. The partial pressure of O2 in a sample of air on a mountain top is 115 mmHg. The oxygen makes up 21% of the gas in the atmosphere. What is the total atmospheric pressure on the mountain top?

2. A gaseous mixture contains 54% N2, 39% O2, and 7% CO2 by volume. If the total pressure is 813 mmHg at STP, what is the partial pressure of each of the gases?

3. What volume would be occupied by 80 g of nitrogen gas at a pressure of 1.8 atm and a temperature of 25C?

4. A gas occupies 0.12 mL at 100 K. At what Celsius temperature will its volume be 2.00 mL? Assume the pressure remains constant.

Explanation / Answer

1) IT IS (115X100)/21=547.61mmHg

2)54% N2=813x54%=439.02mmHg, 39% O2=317.07mmHg and 7% CO2 =56.91mmHg

3)1 mole of gas occupies 22.4ltrs that means 28 grams occupies 22.4ltrs hence 80 grams =22.4x80/28=64

4)T2=V2T1/V1=2x100/0.12=1666.7kelvins=1666.7-273=1393.7degree celsius

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