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3 years ago

At atmospheric pressure a balloon contains 2.00 l of nitrogen gas how would the volume change \

1 answer:

3 0

The complete question; At atmospheric pressure a balloon contains 2.00 l of nitrogen gas, how would the volume change if the kelvin temperature was only 75 % of its original value?
The change in volume would be;
original volume × percentage
= 2 ×0.75 = 1.5 L
Thus the volume would change by 1.5 L

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Explanation:

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Pressure = $125 kPa = 125 kPa \times \frac{0.01 atm}{1 kPa} = 1.25 atm$

According to the ideal gas equation, the volume of given nitrogen gas is calculated as follows.

PV = nRT

where,

P = pressure

V = volume

n = number of moles

R = gas constant = 0.0821 L atm/mol K

T = temperature

Substitute the values into above formula as follows.

$1.25 atm \times V = 1 mol \times 0.0821 L atm/mol K \times 343 K\\V = \frac{1 mol \times 0.0821 L atm/mol K \times 343 K}{1.25 atm}\\= \frac{28.1603}{1.25} L\\= 22.53 L$

Hence, volume of the gas at STP is 22.53 L.

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