Final answer:
Using Boyle's Law, the final pressure of Cl₂ when the volume of its container is increased from 0.175 L to 0.500 L is calculated to be 166.25 mmHg.
Step-by-step explanation:
The question is asking what the pressure of Cl₂ is after increasing the volume of its container from 0.175 L to 0.500 L at a constant temperature of 25°C. To answer this, we can apply Boyle's Law, which states that for a given mass of a gas at a constant temperature, the pressure of the gas is inversely proportional to its volume. The equation for Boyle's Law is P1V1 = P2V2, where P1 and V1 are the initial pressure and volume, and P2 and V2 are the final pressure and volume.
Starting with 475 mmHg as the initial pressure (P1) and 0.175 L as the initial volume (V1), and seeking the final pressure (P2) when the volume (V2) is increased to 0.500 L, the equation looks like this:
P1V1 = P2V2
475 mmHg × 0.175 L = P2 × 0.500 L
Solving for P2 gives us:
P2 = · (475 mmHg × 0.175 L) / 0.500 L
P2 = 166.25 mmHg
Therefore, the final pressure of Cl₂ when the volume is increased to 0.500 L is 166.25 mmHg.