A sample of gas initially occupies 3.50 L at a pressure of 795 torr at 32.0°C. What will the temperature be if the pressure is changed to 4.00 atm, and the volume is changed to 1.50 L?

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Quizplus · Accepted Answer

To solve this problem, we use the combined gas law, which is $P_1V_1/T_1 = P_2V_2/T_2$, where $P$ is pressure, $V$ is volume, and $T$ is temperature in Kelvin. First, we need to convert all units to the standard units: pressure in atm, volume in liters, and temperature in Kelvin. The initial pressure is 795 torr, which converts to atm by dividing by 760 (since 1 atm = 760 torr), so $P_1 = 795 \, \text{torr} \times (1 \, \text{atm} / 760 \, \text{torr}) = 1.046 \, \text{atm}$. The initial temperature in Kelvin is $32.0°C + 273.15 = 305.15 \, K$. Now, we can plug in the values into the combined gas law equation and solve for $T_2$:$1.046 \, \text{atm} \times 3.50 \, \text{L} / 305.15 \, \text{K} = 4.00 \, \text{atm} \times 1.50 \, \text{L} / T_2$Solving for $T_2$ gives us a temperature in Kelvin, which we then convert back to Celsius. After solving, we find that $T_2$ in Kelvin corresponds to a temperature of 225°C, making choice B the correct answer.

A Sample of Gas Initially Occupies 3