If a gas system at 25°C has a pressure of 23.0 atm, what pressure will the system change to if the temperature rises to 35.0°C?

Question

Quizplus · Accepted Answer

The pressure change due to temperature change in a gas system can be calculated using the ideal gas law, assuming volume and amount of gas remain constant. The relationship between pressure and temperature is given by $P_1/T_1 = P_2/T_2$, where $P_1$ and $P_2$ are the initial and final pressures, and $T_1$ and $T_2$ are the initial and final temperatures in Kelvin. Converting the temperatures to Kelvin: $T_1 = 25°C + 273.15 = 298.15 K$ and $T_2 = 35°C + 273.15 = 308.15 K$. Solving for $P_2$, $P_2 = P_1 \times (T_2/T_1) = 23.0 \text{ atm} \times (308.15/298.15) \approx 23.0 \text{ atm} \times 1.0336 \approx 23.8 \text{ atm}$. The correct answer is not explicitly listed, indicating a possible mistake in the calculation or the options provided. Based on the given options and the correct approach, none of the options accurately match the expected calculation, suggesting a need for clarification or correction in the question or answer choices.

If a Gas System at 25°C Has a Pressure of 23.0