In an experiment, a sample of butane gas occupies 1.50 L at a pressure of 1.00 atm and temperature of 298 K. What volume would the butane gas sample occupy at a pressure of 2.350 atm, assuming temperature remains constant and the gas behaves ideally?

• A. 2.35 L
• B. 0.64 L
• C. 1.50 L
• D. 3.53 L

Answer: (B)

Verified step by step guidance

1. Identify the known variables from the problem: initial volume \(V_1 = 1.50\ \text{L}\), initial pressure \(P_1 = 1.00\ \text{atm}\), final pressure \(P_2 = 2.350\ \text{atm}\), and constant temperature \(T\) (298 K, but since temperature is constant, it will not change the calculation).
2. Recognize that this is a problem involving Boyle's Law, which states that for a given amount of gas at constant temperature, the pressure and volume are inversely proportional. Mathematically, this is expressed as: \(P_1 \times V_1 = P_2 \times V_2\)
3. Rearrange the Boyle's Law equation to solve for the unknown final volume \(V_2\): \(V_2 = \frac{P_1 \times V_1}{P_2}\)
4. Substitute the known values into the equation: \(V_2 = \frac{1.00\ \text{atm} \times 1.50\ \text{L}}{2.350\ \text{atm}}\)
5. Calculate the value of \(V_2\) to find the new volume the butane gas occupies at the increased pressure, keeping temperature constant.