Question

Question #e9969

Answer 1

The final pressure will be `P_2 = 0.39 atm`.

Using the ideal gas law `PV = nRT` and knowing that your initial state is defined by a volume `V_1 = 225 mL`, a pressure `P_1 = 1 atm`, and a temperature of `T = (0+273.15) = 273.15K`, you can determine that

`(P_1V_1)/T_1 = (P_2V_2)/T_2` ,

keeping in mind that the number of moles, `n`, remains constant. Your final values for temperature and volume are

`V_2 = 625 mL` and `T_2 = (25+273.15) = 298.15K`, respectively.

Therefore,

`P_2 = (V_1)/(V_2) * (T_2)/(T_1) * P_1` , which yields `P_2 = 0.39 atm`.

The answer makes sense, since an increasing volume would be correlated with a drop in pressure, given that the number of moles are constant.