A sample of gas under a pressure of 622 kPa has a volume of 233 mL. The pressure is increased to 988 kPa, while the temperature remains constant. What volume will the gas occupy at this pressure?
P1*V1 = P2*V2
V2 = (P1/P2) * V1.
147cm
To find the volume of the gas at the increased pressure, you can use Boyle's Law, which states that the pressure and volume of a gas are inversely proportional at constant temperature.
Boyle's Law equation can be written as:
P₁V₁ = P₂V₂
Where:
P₁ = Initial pressure (622 kPa)
V₁ = Initial volume (233 mL)
P₂ = Final pressure (988 kPa)
V₂ = Final volume
In this case, the temperature remains constant, so we can use Boyle's Law to solve for V₂.
Let's substitute the given values into the equation:
622 kPa * 233 mL = 988 kPa * V₂
Now, we can solve for V₂:
V₂ = (622 kPa * 233 mL) / 988 kPa
Calculating this, we get:
V₂ ≈ 146.9 mL
Therefore, at the increased pressure of 988 kPa, the gas will occupy a volume of approximately 146.9 mL.