3.00 moles x 6.02x10^23 molecules/mole = 1.81x10^24 molecules
The number of molecules is 18,066.10e23.
H2S 63.1 g H2S * 1 mol H2S / 34.076 g H2S = 1.85 mol H2S
No of molecules in 18000 cm3 of H2S
H2S (g) + 2 O2 (g) --> H2SO4 (l) 1 mole + 2 mole --> 1 mole You will need 2 moles of O2
Balanced equation: 2H2S + 302 = 2SO2 + 2H20
The oxidation number of sulphur in H2S is 2.
H2S 63.1 g H2S * 1 mol H2S / 34.076 g H2S = 1.85 mol H2S
FeS+2HCl-->FeCl2+H2S Moles of H2S produced equal to moles of FeS used. Moles of H2S=12\34=0.353mol Grams of Fes=0.353*88=31.05g
No of molecules in 18000 cm3 of H2S
There are no moles.There are 2 atoms in one molecule.
H2S (g) + 2 O2 (g) --> H2SO4 (l) 1 mole + 2 mole --> 1 mole You will need 2 moles of O2
Balanced equation: 2H2S + 302 = 2SO2 + 2H20
The oxidation number of sulphur in H2S is 2.
H2S stands for Hydrogen Sulphide.It is a gas.
The molar ratio of oxygen to dihydrogen sulfide in the reaction is 3:1. First, find the number of moles of dihydrogen sulfide by dividing its mass by its molar mass. Then, use the mole ratio to calculate the moles of oxygen needed. Finally, convert the moles of oxygen to grams.
The balanced chemical equation for the reaction between Al2S3 and H2O to produce H2S is: Al2S3 + 6 H2O -> 2 Al(OH)3 + 3 H2S From the balanced equation, 1 mol of Al2S3 produces 3 mol of H2S. Therefore, if 4.0 mol of Al2S3 is reacted, the theoretical yield of H2S would be 3 * 4.0 mol = 12.0 mol.
One mole of hydrogen sulfide (H2S) has 34 g (2+32) and 6.022 x 10^23 molecules (Avogadro Constant). Therefore 17.04g is equal to 0.5012 moles (17.04/34), which is equivalent to 3.0182 x 10^23 molecules (0.5012 x 6.022 x 10^23).
Hydrogen reacts with sulfur in the proportions dictated by this equation:H2 + S --> H2S. The reactants are in a 1:1 proportion with each other, so 1.72 moles of hydrogen will react with 1.72 moles of sulfur.