A scuba diver’s tank contains 0.29 kg of O₂ compressed into a volume of 2.3 L. (a) Calculate the gas pressure inside the tank at 9 °C. (b) What volume would this oxygen occupy at 26 °C and 0.95 atm?

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Casey DurganLv2

21 May 2020

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<p>A scuba diver's tank contains 0.29 kg of <imgsrc="http://session.masteringchemistry.com/render?tex=%7B%5Crm%7BO%7D%7D_2"alt="{\rm{O}}_2" align="middle" /> compressed into a volume of2.3 L. The gas pressure inside the tank at <spanstyle="white-space: nowrap;">9</span><imgsrc="http://session.masteringchemistry.com/render?units=%5E%5Ccirc+C"alt="^\circ C" align="middle" /> is 91 atm. What volume wouldthis oxygen occupy at <span style="white-space:nowrap;">23</span><imgsrc="http://session.masteringchemistry.com/render?units=%5E%5Ccirc+C"alt="^\circ C" align="middle" /> and <spanstyle="white-space: nowrap;">0.93</span> atm?</p>

Many gases are shipped in high-pressure containers. Consider a steel tank whose volume is 55.0 gallons that contains O₂ gas at a pressure of 16,500 kPa at 23 °C. (a) What mass of O₂ does the tank contain? (b) What volume would the gas occupy at STP? (c) At what temperature would the pressure in the tank equal 150.0 atm? (d) What would be the pressure of the gas, in kPa, if it were transferred to a container at 24 °C whose volume is 55.0 L?

olivecaribou314

Mixtures of helium and oxygen are used in scuba diving tanks to help prevent "the bends". For a particular dive, 18.6 L of oxygen gas at and 1.79 atm, and 7.55 L of helium gas at and 2.68 atm were pumped into a tank with a volume of 6.00 L at .