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3 years ago

There are 0.3 moles of xenon gas in a 0.5-liter container at 30 degrees C. What is the pressure exerted by the xenon gas

Chemistry

2 answers:

zhenek [66]3 years ago

4 0

Answer : The pressure of the gas is, 14.925 atm

Solution :

using ideal gas equation,

$PV=nRT$

where,

n = number of moles of gas = 0.3 mole

P = pressure of the gas = ?

T = temperature of the gas = $30^oC=273+30=303K$

R = gas constant = 0.0821 Latm/moleK

V = volume of the gas = 0.5 L

Now put all the given values in the above equation, we get the pressure of the gas.

$P\times (0.5L)=(0.3mole)\times (0.0821L.atm/mole.K)\times (303K)$

$P=14.925atm$

Therefore, the pressure of the gas is, 14.925 atm

Kaylis [27]3 years ago

3 0

PV = nRT
P = (nRT)/V
P = (0.3 mol × 0.08206 atm-l/(mol-K) × (273.15 + 30) K)/(0.5 l)
P = 14.9258934 atm

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