PV = nRT
V = nRT/P = (2.00 mol)(0.08206 Latm/kmol)(573K)/(2.62 atm)
V = 35.9 liters (to 3 sig. figs.)
Using the ideal gas law, V = (nRT)/(P), where n = moles, R = gas constant, T = temperature in Kelvin, and P = pressure in atm. Plug in the values to find the volume: V = (2.00 moles * 0.0821 L.atm/mol.K * 300 K) / (2.62 atm) = 49.22 L. Therefore, 2.00 moles of hydrogen gas at 2.62 ATM and 300.C will occupy 49.22 liters of volume.
The volume is 35,9 L.
At STP (Standard Temperature and Pressure), 1 mole of any gas occupies 22.4 L. Therefore, 2.88 moles of hydrogen would occupy: Volume = 2.88 moles * 22.4 L/mole = 64.51 L. So, 2.88 moles of hydrogen at STP would occupy 64.51 liters.
At standard temperature and pressure, 2.3 grams of sulfur dioxide will occupy approximately 1.8 L of volume.
0.50 moles of NH3 at STP (Standard Temperature and Pressure) occupies 11.2 liters of volume.
The volume of 0.8 moles of a gas at Standard Temperature and Pressure (STP) is 17.6 liters. This is because at STP, one mole of any ideal gas occupies 22.4 liters.
Assuming complete reaction, 0.91 grams of Mg will produce 0.0455 moles of hydrogen gas. At standard temperature and pressure (STP), 1 mole of any gas occupies 22.4 liters, so 0.0455 moles will occupy approximately 1.02 liters.
You can use the ideal gas law formula: PV = nRT, where P is pressure, V is volume, n is moles, R is the gas constant, and T is temperature in Kelvin. Convert the temperature to Kelvin by adding 273.15 (141 + 273.15 = 414.15 K). Plug in the values: (7.77 ATM) V = (3.12 moles) (0.0821 LATM/molK) (414.15 K). Solve for V to find the volume of the gas.
0.48 liters at STP (standard temperature and pressure)
This volume is 79,79 litres.
The volume of 0.8 moles of a gas at Standard Temperature and Pressure (STP) is 17.6 liters. This is because at STP, one mole of any ideal gas occupies 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 total moles of gas in the mixture is 0.220 + 0.350 + 0.640 = 1.210 moles. To find the pressure of H2, we need to consider the mole fraction of H2, which is 0.350/1.210 = 0.289. So, the pressure of H2 is 0.289 * 2.95 Atm = 0.852 Atm.