Which of the following actions would increase the pressure of a gas in a closed container, assuming the amount of gas remains constant?

• A. Removing some gas from the container
• B. Increasing the temperature of the gas
• C. Increasing the volume of the container
• D. Decreasing the temperature of the gas

Answer: (B)

Verified step by step guidance

1. Recall the ideal gas law: \(P \times V = n \times R \times T\), where \(P\) is pressure, \(V\) is volume, \(n\) is the amount of gas (in moles), \(R\) is the gas constant, and \(T\) is temperature in Kelvin.
2. Since the amount of gas \(n\) and the container are constant, analyze how changing temperature or volume affects pressure.
3. Increasing the temperature \(T\) increases the product \(nRT\), so if volume \(V\) is constant, pressure \(P\) must increase to maintain the equation.
4. Increasing the volume \(V\) would cause pressure \(P\) to decrease if temperature and amount of gas remain constant, because pressure and volume are inversely related.
5. Removing some gas decreases \(n\), which would decrease pressure if volume and temperature remain constant; decreasing temperature \(T\) also decreases pressure.