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.
Sulfur dioxide is SO2, so there are 2 moles of oxygen for each mole of sulfur. In 25 moles of SO2, there are 25 moles of S, so there must be 50 moles of oxygen, or 25 moles of diatomic oxygen gas (O2).
6moles
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.