At standard temperature and pressure (STP), one mole of an ideal gas occupies 22.4 liters. Therefore, to find the volume occupied by 0.685 mol of gas at STP, you can multiply the number of moles by the volume per mole:
0.685 mol × 22.4 L/mol = 15.34 liters.
Thus, 0.685 mol of gas occupies approximately 15.34 liters at STP.
1 mole gas = 22.4L 1.5mol C2H4 x 22.4L/mol = 33.6L ethane gas (C2H4)
The volume of any gas at STP (standard temperature and pressure) is 22.4 L/mol. The molar mass of helium is 4.0026 g/mol. So, 84.6 grams of helium would be 84.6/4.0026 = 21.1 mol. Therefore, the volume of 84.6 grams of helium at STP would be 21.1 mol * 22.4 L/mol = 472.64 L.
Using the ideal gas law, V = (nRT)/P, where V is volume, n is moles, R is the gas constant, T is temperature in Kelvin, and P is pressure, we can calculate the volume to be 7.34 L.
To find the volume of 2.5 mol of hydrogen gas, we can use the Ideal Gas Law equation: PV = nRT. We are given the pressure (152 kPa), temperature (-20.0 degrees Celsius which is equivalent to 253.15 K), and the number of moles (2.5 mol). We can rearrange the equation to solve for volume (V), V = (nRT)/P. Plugging in the values, V = (2.5 mol x 8.314 J/mol·K x 253.15 K) / 152 kPa = 3.51 L. Therefore, 2.5 mol of hydrogen gas will occupy a volume of 3.51 liters at -20.0 degrees Celsius and 152 kPa.
The volume of gas molecules is negligible compared to the total gas volume. Gas molecules themselves occupy a very small fraction of the total volume of the gas, with the majority of the volume being empty space between the molecules.
The volume is 22,1 L.
The molar volume of an ideal gas at standard temperature and pressure (STP) is 22.4 L/mol. Therefore, 0.75 mol of methane gas would occupy 16.8 liters (0.75 mol x 22.4 L/mol = 16.8 L).
1 mole gas = 22.4L 1.5mol C2H4 x 22.4L/mol = 33.6L ethane gas (C2H4)
To find the volume of 19.87 mol of NH₄Cl at STP (standard temperature and pressure), we can use the ideal gas law. At STP, 1 mol of gas occupies 22.4 L. Therefore, 19.87 mol of NH₄Cl will occupy 19.87 mol x 22.4 L/mol = 445.888 L.
This statement is true. According to the ideal gas law, at 0°C and 1 atm pressure, 1 mol of any ideal gas occupies 22.4 L of volume. Therefore, 1.0 mol of nitrogen would occupy 22.4 L and 2.0 mol of hydrogen would occupy 44.8 L in a 22.4 L box.
The volume of any gas at STP (standard temperature and pressure) is 22.4 L/mol. The molar mass of helium is 4.0026 g/mol. So, 84.6 grams of helium would be 84.6/4.0026 = 21.1 mol. Therefore, the volume of 84.6 grams of helium at STP would be 21.1 mol * 22.4 L/mol = 472.64 L.
Using the ideal gas law, V = (nRT)/P, where V is volume, n is moles, R is the gas constant, T is temperature in Kelvin, and P is pressure, we can calculate the volume to be 7.34 L.
The volume of 0.0100 mol of CH4 gas at STP (Standard Temperature and Pressure) is 224 mL. This is based on the ideal gas law and the molar volume of a gas at STP, which is 22.4 L/mol. Converting this to milliliters gives 224,000 mL/mol.
125 mol.
1mol of a gas occupies 24 dm3 at STP, so 2.2mol X 24 mol/dm3 =52.8dm3 or 5280cm3
To find the volume of 2.5 mol of hydrogen gas, we can use the Ideal Gas Law equation: PV = nRT. We are given the pressure (152 kPa), temperature (-20.0 degrees Celsius which is equivalent to 253.15 K), and the number of moles (2.5 mol). We can rearrange the equation to solve for volume (V), V = (nRT)/P. Plugging in the values, V = (2.5 mol x 8.314 J/mol·K x 253.15 K) / 152 kPa = 3.51 L. Therefore, 2.5 mol of hydrogen gas will occupy a volume of 3.51 liters at -20.0 degrees Celsius and 152 kPa.
The volume of gas molecules is negligible compared to the total gas volume. Gas molecules themselves occupy a very small fraction of the total volume of the gas, with the majority of the volume being empty space between the molecules.