What volume of hydrogen would be required to produce 0.400 mole of HCl at STP?
H2(g) + Cl2 (g) → 2HCl(g)
each mole of H2 produces two moles of HCl
moles of H2 needed ... 0.400 / 2
each mole of gas has a volume of 22.4 L
Thank you!!!
To determine the volume of hydrogen gas (H2) required to produce 0.400 moles of hydrogen chloride (HCl) gas at standard temperature and pressure (STP), we can use the balanced equation:
H2(g) + Cl2(g) → 2HCl(g)
According to the stoichiometry of the balanced equation, 1 mole of H2 reacts to produce 2 moles of HCl.
Therefore, 0.400 moles of H2 would produce (0.400 moles H2) × (2 moles HCl / 1 mole H2) = 0.800 moles of HCl.
At STP, 1 mole of any ideal gas occupies a volume of 22.4 liters. Therefore, we can calculate the volume of H2 using the ideal gas law:
Volume (V) = (moles of gas) × (molar volume)
V = (0.400 moles) × (22.4 L/mol)
V = 8.96 liters
So, the volume of hydrogen gas required to produce 0.400 moles of HCl at STP is 8.96 liters.
To determine the volume of hydrogen gas (H2) required to produce 0.400 moles of hydrogen chloride (HCl) at standard temperature and pressure (STP), we can use the balanced chemical equation:
H2(g) + Cl2(g) → 2HCl(g)
According to the stoichiometry of the equation, 1 mole of H2 reacts to produce 2 moles of HCl. Therefore, the stoichiometric ratio is 1:2.
Given that you have 0.400 moles of HCl, we need to convert this amount to moles of H2 to determine the required volume.
First, divide the number of moles of HCl by the stoichiometric ratio (2 moles of HCl per 1 mole of H2):
0.400 mol HCl / (2 mol HCl/1 mol H2) = 0.200 mol H2
Now, we have 0.200 moles of H2. At STP, 1 mole of any ideal gas occupies 22.4 liters. Hence, we can multiply the number of moles by the molar volume to find the volume of H2:
0.200 mol H2 * 22.4 L/mol = 4.48 L
Therefore, to produce 0.400 moles of HCl at STP, you would require approximately 4.48 liters of hydrogen gas.