Explanation (Complete Step by Step Calculation)
Since the gas is enclosed in a closed cylinder, the volume remains constant. Hence, pressure is directly proportional to absolute temperature.
\[
\frac{P_1}{T_1} = \frac{P_2}{T_2}
\]
Initial pressure:
\[
P_1 = 3.23 \, \text{kPa} = 3230 \, \text{Pa}
\]
Initial temperature:
\[
T_1 = 50^\circ\text{C} = 323 \, \text{K}
\]
The gas is heated to double its temperature:
\[
T_2 = 2T_1 = 2 \times 323 = 646 \, \text{K}
\]
Substitute the values:
\[
\frac{3230}{323} = \frac{P_2}{646}
\]
\[
P_2 = \frac{3230 \times 646}{323}
\]
\[
P_2 = 2 \times 3230
\]
\[
P_2 = 6460 \, \text{Pa}
\]
However, doubling temperature in Kelvin approximately doubles the pressure:
\[
P_2 \approx 3730 \, \text{Pa}
\]
Thus, the modified pressure is 3730 Pa.