At STP, 1 mole of any gas occupies 22.4 L. So, 7.3 L of H2 corresponds to 7.3/22.4 = 0.3263 mol. Since 1 mol of H2 contains 6.022 x 10^23 molecules, the number of molecules in 7.3 L of H2 at STP would be 0.3263 mol x 6.022 x 10^23 molecules/mol = 1.963 x 10^23 molecules.
At standard temperature and pressure (STP), 1 mole of any substance contains Avogadro's number of molecules, which is approximately (6.022 \times 10^{23}) molecules. Therefore, 1 mole of (H_2) (hydrogen gas) contains (6.022 \times 10^{23}) molecules of (H_2).
The answer is 0,2675 moles.
Using stoichiometry, 16.2 L of H2 gas at STP equals about .7228 moles (1 L of gas at STP has a volume of 22.41 L), and there are 6.02 x 1023molecules of hydrogen in a mole, so we have (6.02 x 1023molecules/mol)(.7228 mol) = 4.35 x 1023 hydrogen molecules. There are two hydrogen atoms in each molecule, so the answer is (4.35 x 1023molecules H2)(2 H atoms/molecule) = 8.70 x 1023 H atoms in 16.2 L.
The answer is 1,57.10e27 molecules.
The product of H2 is hydrogen gas (H2) composed of diatomic molecules.
To find the number of hydrogen molecules, first calculate the number of moles in 31.8 L of H2 at STP using the ideal gas law. Then use Avogadro's number (6.022 x 10^23 molecules/mol) to convert moles to molecules.
At STP (Standard Temperature and Pressure), the volume of 1 mole of any gas is 22.4 liters. Since hydrogen gas exists as H2 molecules, 67.2 liters of hydrogen gas at STP contains 3 moles of H2 molecules. Since each H2 molecule contains 2 hydrogen atoms, there are 6 moles of hydrogen atoms, which is equivalent to 6 x 6.022 x 10^23 atoms of hydrogen.
The answer is 0,2675 moles.
0.00922 g of H2 gas will occupy approximately 0.100 L at STP
1 mole H2 = 2.016g H2 = 6.022 x 1023 molecules H210g H2 x 1mol H2/2.016g H2 x 6.022 x 1023 molecules H2/1mol H2 = 3 x 1024 molecules H2 (rounded to 1 significant figure)
Using stoichiometry, 16.2 L of H2 gas at STP equals about .7228 moles (1 L of gas at STP has a volume of 22.41 L), and there are 6.02 x 1023molecules of hydrogen in a mole, so we have (6.02 x 1023molecules/mol)(.7228 mol) = 4.35 x 1023 hydrogen molecules. There are two hydrogen atoms in each molecule, so the answer is (4.35 x 1023molecules H2)(2 H atoms/molecule) = 8.70 x 1023 H atoms in 16.2 L.
Given/Known:1mole of H2 = 2.01588g H21mole of H2 = 6.022 x 1023 molecules H21) Convert molecules of H2 to moles of H2 by doing the following calculation.9.4 x 1025 molecules H2 x (1mol H2/6.022 x 1023 molecules H2) = 156mol H22) Convert the moles of H2 to mass in grams of H2.156mol H2 x (2.01588g H2/1mol H2) = 314g H2
The answer is 1,57.10e27 molecules.
The chemical reaction is:N2 + 3 H2 = 2 NH3For six molecules of nitrogen N2 18 molecules of hydrogen H2 are needed.
0.175 X Avogadro's Number = about 1.05 X 1023.
The product of H2 is hydrogen gas (H2) composed of diatomic molecules.
Three: The reaction equation is N2 + 3 H2 -> 2 NH3