PV = nRT
V = nRT/P = (2.00 mol)(0.08206 Latm/kmol)(573K)/(2.62 atm)
V = 35.9 liters (to 3 sig. figs.)
The volume is 35,9 L.
The volume is 13,64 L.
At STP, 1 mole of gas occupies a volume of 22.4 liters. Thus, 4/5 moles of gas will occupy .8*22.4 liters.
3.8 kPa
The partial pressure of the hydrogen will be 0.853 atmospheres.
At standard temperature and pressure, 1 mole of any gas will occupy 22.4 liters. Set up a direct proportion of 22.4 liters/1 mole = 1 liter/x moles and solve for x. You get 0.045 moles.
The volume is 13,64 L.
0.48 liters at STP (standard temperature and pressure)
This volume is 79,79 litres.
At STP, 1 mole of gas occupies a volume of 22.4 liters. Thus, 4/5 moles of gas will occupy .8*22.4 liters.
The volume is approx. 15,35 litres.
PV = nRTV = nRT/P = (2.00 mol)(0.08206 Latm/kmol)(573K)/(2.62 atm)V = 35.9 liters (to 3 sig. figs.)
Approx. 774 litres.
What you need to know to work this out is that:- Moles of gases at standard temperature pressure (With P and T constant) are proportional to the volume they occupy, divided by their specific gas constant.
Since hydrogen is a gas, we would need more information to answer it. As chance wrote, you will need twice as much hydrogen as oxygen. However, in order to know what the volume of that hydrogen is, we also need to know the temperature and pressure so that we can use the universal gas law to get the answer.
The answer is 0,19 moles.
3.8 kPa
The partial pressure of the hydrogen will be 0.853 atmospheres.