To determine how the temperature of the system changes when the pressure is changed from 745 mm Hg to 1 atm, we can use the combined gas law, which relates the pressure, volume, and temperature of a gas:
(P1V1)/T1 = (P2V2)/T2
where P1, V1, and T1 are the initial pressure, volume, and temperature, respectively, and P2 and V2 are the final pressure and volume, respectively.
We can assume that the volume of the container remains constant, so V1 = V2. We also need to convert the initial pressure from mm Hg to atm:
P1 = 745 mm Hg x (1 atm/760 mm Hg) = 0.980 atm
Then, we can rearrange the equation to solve for T2:
T2 = (P2/T1) * (V1/P1)
Substituting the values we know, we get:
T2 = (1 atm/0.980 atm) * (T1)
T2 = 1.02T1
Therefore, the temperature of the system will increase by 2% when the pressure is changed from 745 mm Hg to 1 atm, assuming the volume remains constant.