A ball of clay with air inside it is sealed at 25.0°C and 1.00 atm. The ball is heated steadily until it explodes at 60.0°C. What is the pressure inside the ball of clay before it explodes?

Question

Quizplus · Accepted Answer

The pressure inside the ball before it explodes can be calculated using the ideal gas law and assuming the volume and the amount of gas remain constant. The relationship between pressure and temperature for a given amount of gas in a constant volume is given by $P_1/T_1 = P_2/T_2$, where $P_1$ and $T_1$ are the initial pressure and temperature, and $P_2$ and $T_2$ are the final pressure and temperature. Temperatures must be in Kelvin. Converting the temperatures to Kelvin: $T_1 = 25.0°C + 273.15 = 298.15 K$ and $T_2 = 60.0°C + 273.15 = 333.15 K$. Solving for $P_2$, $P_2 = P_1 \times (T_2/T_1) = 1.00 \text{ atm} \times (333.15/298.15) = 1.12 \text{ atm}$.

A Ball of Clay with Air Inside It Is Sealed