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Answer :
The pressure in a 28.0- L cylinder filled with 36.6 g of oxygen gas at a temperature of 349 K is 31.5 atm.
To calculate the pressure in a 28.0- L cylinder filled with 36.6 g of oxygen gas at a temperature of 349 K is 31.5 atm, we use the ideal gas law relates the pressure, temperature, and volume of a gas using the equation PV = nRT, where P is the pressure of the gas, V is the volume of the gas, n is the number of moles of the gas, R is the universal gas constant, and T is the absolute temperature of the gas. We can rearrange the ideal gas law equation to solve for pressure. That is:
P = (nRT) / V
Given that the volume of the cylinder is 28.0 L and it is filled with 36.6 g of oxygen gas at a temperature of 349 K, we need to first find the number of moles of oxygen gas present using the ideal gas law equation, n = (m/M), where m is the mass of the gas and M is the molar mass of the gas. The molar mass of oxygen is 32.00 g/mol. That is:
n = (36.6 g)/(32.00 g/mol) = 1.144 mol
Now we can plug the values into the ideal gas law equation and solve for pressure.
P = (nRT) / V
= [(1.144 mol) (0.08206 L atm/mol K) (349 K)] / (28.0 L)
= 31.5 atm
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