To solve this problem, we need to convert the pressure from psi (pounds per square inch) to atm (atmosphere) and apply Charles's law, which states that for a fixed amount of gas at a constant volume, the pressure is directly proportional to the temperature.
First, let's convert the initial pressure of 35.0 psi to atm.
1 atm is approximately equal to 14.7 psi.
Initial pressure (P1) = 35.0 psi / 14.7 psi/atm ≈ 2.38 atm
Since the volume is constant, we can use the equation:
P1 / T1 = P2 / T2
Where: P1 = Initial pressure (2.38 atm) T1 = Initial temperature (25.0 °C + 273.15 K) P2 = Final pressure (unknown) T2 = Final temperature (100.0 °C + 273.15 K)
Now, let's solve for P2:
P2 = P1 * (T2 / T1)
P2 = 2.38 atm * (373.15 K / 298.15 K)
P2 ≈ 2.97 atm
Therefore, the pressure of the gas at 100.0 °C would be approximately 2.97 atm.