- molar mass: 34,08 g
- density: 1,363 g/cm3
Mass of H2S: 1,363 x 9,36 = 12,758 g
34,08--------------------------1 mol
12,758-------------------------x
x = 0,374 moles
At STP? I must assume STP since you mention no temperature or pressure. The formula would be the same anyway, so.......
PV = nRT
(1 atm)(9.63 L) = n(0.08206 L*atm/mol*K)(298.15 K)
9.63/24.466 = n(moles H2)
0.394 moles of hydrogen gas
-------------------------------------
0.43 moles, since 1 mole of gas occupies 22.4 L at STP.
In 11.2 L gas (of any kind, even mixtures such as air) at STP contains always 0.50 mole gaseous particles.
There is a mole of H2 in 24dm3 (24 liters) of H2 in STP. So there will be 1/24 (0.0417, accurate to 3 sig fig) mole of H2 gas in 1 liter of H2 in STP.
0.460
.430 mol
.459 mol
152
0.25 moles
4 g of Helium = 1 mole.So, 56 g of helium = 14 moles
8,4 liters of nitrous oxide at STP contain 2,65 moles.
16,8 L of Xe gas at STP is equivalent to 0,754 moles.
152
The volume is 0.887 L.
1 mole occupies 22.414 liters So, 3.30 moles will occupy 73.966 liters.
0.25 moles
4 g of Helium = 1 mole.So, 56 g of helium = 14 moles
8,4 liters of nitrous oxide at STP contain 2,65 moles.
16,8 L of Xe gas at STP is equivalent to 0,754 moles.
The answer is 2,68 moles.
The answer is 0,2675 moles.
Approx 0.223 moles.
17.7
Assuming ideal behaviour, 1 mole of any gas occupies 22.4L at STP. So, moles of 10L = 10/22.4 moles = 0.4464 moles