Question #29668

How many grams of water vapor (H2O) are in a 10.2 liter sample at 0.98 atmospheres and 26°C? Show all work used to solve this problem.

Expert's answer

For solving that task we shall use the equation:

pV = nRT,

where p-pressure, V-volume, n - amount of moles, n - gas constant (n = 0.080206)

n = pV/RT

The amount of moles can be found by the equation:

n = m/M

where m - mass, M - molar mass

So the mass could be calculated as:

m = n*M

M(H_{2}O) = 18 grams/mole

n(H_{2}O) = 0.98*10.2/0.08206*(26 + 273) = 0.43 moles

m(H_{2}O) = 0.43*18 = 7.3 grams

pV = nRT,

where p-pressure, V-volume, n - amount of moles, n - gas constant (n = 0.080206)

n = pV/RT

The amount of moles can be found by the equation:

n = m/M

where m - mass, M - molar mass

So the mass could be calculated as:

m = n*M

M(H

n(H

m(H

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