First find moles hydrogen gas.
20 grams H2 (1 mole H2/2.016 grams)
= 9.921 moles H2
Now, the ideal gas equation.
PV = nRT
(1 atm)(volume L) = (9.921 moles H2)(0.08206 L*atm/mol*K)(298.15 K)
Volume of hydrogen gas = 243 Liters
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3.61g/L D=m/v
bukkake
10.0 L
nitros oxide N2O
# This is a stoichiometry problem and requires a balanced chemical equation. N2 + 3 H2 ----> 2 NH3 If we assume that this reaction occurs at STP, then the number of moles of any gas at STP is equal to the volume (in litres) divided by 22.4 This will get you started.1500ml
3.61g/L D=m/v
0.48 liters at STP (standard temperature and pressure)
bukkake
At STP, 1 mole of any ideal gas occupies 22.4 liters. Therefore, 5 liters of NO2 at STP will represent 0.22 moles (5/22.4), and this is the case for any other ideal gas. So, the answer is that 5 liter of ANY ideal gas will have the same number of molecules as 5 liters of NO2.
0.67 mol
10.0 L
10.0 L
60 grams.
1 mole occupies 22.414 liters So, 3.30 moles will occupy 73.966 liters.
Hydrogen? You need the conditions, pressure and temperature, of the gas. 1 mole of the gas occupies 22.4 liters at STP. The molar mass of hydrogen is 2.0 g/ mole. So the density at STP is 2.0 / 22.4 = 0.0893 g/liter. At any other pressure and temperature you can use the ideal gas law to find the volume of one mole and then find the density.
How many molecules are in 30 liters of methane (CH4) at STP
152