If the pressure of 1.50 L of hydrogen gas at 100°C decreases from 0.500 atm to 0.115 atm, what is the final volume? Assume temperature remains constant.

• A. 1.50 L
• B. 3.00 L
• C. 6.52 L
• D. 0.345 L

Answer: (C)

Verified step by step guidance

1. Identify the initial and final conditions of the gas. The initial volume (V1) is 1.50 L, the initial pressure (P1) is 0.500 atm, and the final pressure (P2) is 0.115 atm. The temperature is constant at 100°C.
2. Recognize that this problem involves Boyle's Law, which states that for a given amount of gas at constant temperature, the pressure of the gas is inversely proportional to its volume. The formula is: $\frac{P}{V}=\; ext\{constant\}$.
3. Rearrange Boyle's Law to solve for the final volume (V2): $P_1{V}_1=P_2{V}_2$. Therefore, .
4. Substitute the known values into the equation: .
5. Calculate the final volume using the substituted values. This will give you the final volume of the gas under the new pressure conditions.