How many moles are in 10.3 L of helium gas at STP?

Answer 1

- 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

Answer 2

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

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Answer 3

At STP (standard temperature and pressure), 1 mole of any gas occupies 22.4 liters. Therefore, in 10.3 L of helium gas at STP, the number of moles would be 10.3 L / 22.4 L/mol = 0.460 moles.

Answer 4

0.43 moles, since 1 mole of gas occupies 22.4 L at STP.

Answer 5

In 11.2 L gas (of any kind, even mixtures such as air) at STP contains always 0.50 mole gaseous particles.

Answer 6

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.

Answer 7

0.460

Answer 8

.430 mol

Answer 9

.459 mol