Question

A quantity of gas has a pressure of 1.39 atm and a volume of 6.95 L. What is the

volume of this gas when the pressure is changed to 740 mm Hg?

Answer 1

The volume of the quantity of gas when the pressure changes to 740 mm Hg is approximately 9.92 L

Step-by-step explanation:

The properties of the quantity of gas are;

The initial pressure of the gas, P₁ = 1.39 atm

The initial volume of the given volume of gas, V₁ = 6.95 L

The final pressure of the quantity of gas, P₂ = 740 mmHg

Boyle's Law states that at constant temperature, the pressure, P, of a given mass of gas is inversely proportional to its volume, V

Mathematically Boyle's Law can be written as follows;

`P \propto (1)/(V)`

Therefore, we have;

P₁·V₁ = P₂·V₂

Where;

V₂ = The final volume of the quantity of gas when the pressure changes to 740 mm Hg

`\therefore V_2 = (P_1 \cdot V_1)/(P_2)`

By substituting the known values, we have;

`V_2 = (1.39 \ atm * 6.95 \ L)/(740 \ mmHg) = (1.39 \ atm * 6.95 \ L)/(0.973521 \ atm) = 9.92159459459 \ L \approx 9.92 \ L`

The final volume of the quantity of gas when the pressure changes to 740 mm Hg = V₂ ≈ 9.92 L