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The pressure of 5.0 l of gas increases from 1.50 atm to 1240 mmhg. what is the final volume of the gas, assuming constant temperature?

User Dzior
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1 Answer

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First we need to convert everything into SI units.

The initial volume of the gas is (keeping in mind that
1 L = 0.001 m^3:

V_i = 5.0 L = 0.005 m^3

The initial pressure of the gas is (keeping in mind that
1 atm = 1.01 \cdot 10^5 Pa:

p_i = 1.50 atm=1.52 \cdot 10^5 Pa

The final pressure of the gas is (keeping in mind that
760 mmHg = 1 atm=1.01 \cdot 10^5 Pa)

p_f = 1240 mmHg = 1.65 \cdot 10^5 Pa

At constant temperature, the product between pressure and volume of the gas is constant, so we can write

p_i V_i = p_f V_f

from which we find the final volume of the gas:

V_f = (p_i V_i)/(p_f) = ((1.52 \cdot 10^5 Pa)(0.005 m^3))/(1.65 \cdot 10^5 Pa) =0.0046 m^3 = 4.6 L
User Hasankzl
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