Which of the following occurs when a rigid container of gas is heated, assuming the amount of gas remains constant?

• A. The pressure of the gas increases.
• B. The pressure of the gas decreases.
• C. The volume of the gas increases.
• D. The number of moles of gas increases.

Answer: (A)

Verified step by step guidance

1. Identify the variables involved in the problem: pressure (P), volume (V), temperature (T), and amount of gas (n). The problem states the container is rigid, so volume (V) is constant, and the amount of gas (n) is constant.
2. Recall the ideal gas law: \(P \times V = n \times R \times T\), where \(R\) is the ideal gas constant.
3. Since the volume \(V\) and the number of moles \(n\) are constant, the relationship between pressure and temperature can be isolated as \(P \propto T\) (pressure is directly proportional to temperature).
4. When the gas is heated, the temperature \(T\) increases. Because \(P\) is directly proportional to \(T\) at constant \(V\) and \(n\), the pressure \(P\) must increase.
5. Therefore, the correct conclusion is that the pressure of the gas increases when a rigid container of gas is heated, assuming the amount of gas remains constant.