A sample of O2 under 2.00 atm occupies 500 ml at 25.0˚C. What pressure will the sample have at 0.0˚C ?

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Answer 1 · 2014-07-02T06:30:40

In this question we will use the ideal gas equation.

#P_1# x #V_1# / #T_1# = #P_2# x #V_2# / #T_2#

#P_1# = 2 atm
#V_1# = 500 mL
#T_1# = 25 + 273 = 298 K

#P_2# = ?
#V_2# = 500 mL
#T_2# = 0 + 273 = 273 K

substituting values;

2 atm x 500 mL / 298 K = #P_2# x 500 mL / 273

rearranging we get,

1000 atm mL x 273 K / 500 mL x 298 K = #P_2#

#P_2# = 1.83 atm.