The moles in 410 g of hydrogen gas : <u><em>201.67</em></u>
<h3>Further explanation</h3>
Some of the laws regarding gas can apply to ideal gas (volume expansion does not occur when the gas is heated), :
Boyle's law at constant T,
Charles's law, at constant P,
Avogadro's law, at constant P and T,
So that the three laws can be combined into a single gas equation, the ideal gas equation
In general, the gas equation can be written
where
P = pressure, atm
V = volume, liter
n = number of moles
R = gas constant = 0.082 l.atm / mol K
T = temperature, Kelvin
Hydrogen gas has a density of 0.090, and at normal pressure (1 atm) and 2.57 °C (273+ 2.57 = 275.57K), one mole of it takes up 22.4 l
From here we can input into the ideal gas equation to find an unknown value, molar mass
(M)
we have to manipulate this ideal gas equation to find molar mass,
molar mass is the ratio between mass and mole
.... equation 1
Whereas density is the ratio between mass and volume
.... equation 2
The ideal gas equation becomes
We input the known values
moles in 410 g of hydrogen gas :
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Keywords: mole, hydrogen gas, density, normal pressure