A deep-sea diver uses a gas cylinder with a volume of 10.0 L and a content of 51

Question

A deep-sea diver uses a gas cylinder with a volume of 10.0 L and a content of 51.7g of O2 and 32.4g of He. Calculate the partial pressure of each gas and the total pressure if the temperature of the gas is 19 degree C. The ideal gas law (PV - nRT) describes the relationship among pressure P, volume V, temperature T, and molar amount n. When n and V are fixed, the equation can be rearranged to take the following form where k is a constant: P/T = nR/V = k or (P T)initial = (P T)final When n and P are fixed, the expression becomes V/T = nR/P = k or (V T)initial = (V T)final The pressure inside a hydrogen-filled container was 2.10 atm at 21 degree C. What would the pressure be if the container was heated to 88 degree C? Express your answer with the appropriate units. The pressure of a fixed amount of gas at constant volume is directly proportional to its temperature: the higher the temperature, the greater the pressure. That is why warnings on many household containers read: ''Contents under pressure. Do not place near sources of heat.'' If such a container is overheated, it might explode. As standard temperature and pressure (0 degree C and 1.00 atm), 1.00 mol of an ideal gas occupies a volume of 22.4 L. What volume would the same amount of gas occupy at the same pressure and 95 degree C? Express your answer with the appropriate units.

Explanation / Answer

PO2, PHe, Ptotal=3.87, 19.42, 23.29 atm

Part B.

30.2 L

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