A sample of CO2 occupies a volume of 3.50l at 125 kPa pressure,What pressure would the gas exert if the volume was decreased to 2.00l?
According to Boyle's Law
P1V1=P2V2
P1 = 125 kPa P2 = ?
V1 = 3.50 L V2 = 2.00
P2=P1V1/V2
=125*3.50/2
P2=219kPa
To solve this problem, we'll use Boyle's Law, which states that the pressure and volume of a gas are inversely proportional at a constant temperature.
Boyle's Law equation: P₁V₁ = P₂V₂
Given:
P₁ = 125 kPa (initial pressure)
V₁ = 3.50 L (initial volume)
V₂ = 2.00 L (final volume)
We need to determine P₂ (final pressure).
Let's plug in the values into Boyle's Law equation and solve for P₂:
125 kPa * 3.50 L = P₂ * 2.00 L
Now, let's solve this equation step by step:
Step 1: Multiply the initial pressure and volume:
125 kPa * 3.50 L = 437.5 kPa·L
Step 2: Divide both sides of the equation by the final volume:
437.5 kPa·L / 2.00 L = P₂
Step 3: Simplify the equation:
218.75 kPa = P₂
Therefore, if the volume of the CO2 sample is decreased to 2.00 L, the gas would exert a pressure of 218.75 kPa.