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Answers to Gas Laws Practice Problems

1.  molar mass of Cl2 = 2(35.45)  =  70.90 g/mole

     \(\mathrm{d=\dfrac{mm}{mV}=\dfrac{70.9\:g}{22.4\:L}=3.17\: g/L}\)

 

2.  Molar volume is the volume when n = 1.00 mole.

      V = ?;  n = 1.00 mol; T = 78°C + 273 = 351 K;  P = 1.20 atm

      \(\mathrm{V=\dfrac{nRT}{P}=\dfrac{(1.00\:mol)(0.08206)(351\:K)}{1.20\:atm}=24.0\: L}\)

 

3.  V1 = 6.66 L;    STP:  T1 = 0°C = 273 K;    P1 = 1.00 atm = 760 torr;

      T2 = 546 °C + 273 = 819 K;   P2 = 684 torr;    V2 = ?

      \(\mathrm{\dfrac{P_1V_1}{T_1}=\dfrac{P_2V_2}{T_2}}\)       \(\mathrm{V_2=V_1\times\dfrac{P_1}{P_2}\times\dfrac{T_2}{T_1}=6.66\:L\times\dfrac{760\:torr}{684\:torr}\times\dfrac{819\:K}{273\:K}=22.2\:L}\)

 

4.  mass of CO2 = ?;  V = 5.60 L; T = 273K; P = 2.00 atm

     \(\mathrm{n=\dfrac{PV}{RT}=\dfrac{(2.00\:atm)(5.60\:L)}{(0.08206)(273\:K)}=0.500\:moles}\);  \(\mathrm{0.500\: moles\times\dfrac{44.0\:g\:CO_2}{1\:mole\:CO_2} =22.0\: g\: CO_2}\)

 

5.  From the Table, \(\mathrm{P_{H_2O}}\) at 21°C = 19 mm Hg; You can subtract in atm or torr.

      For torr:  \(\mathrm{P_T = 1.02\: atm\times\dfrac{760\:torr}{1\:atm} = 775\: torr}\);  \(\mathrm{P_{N_2} = P_T - P_{H_2O} = 775 - 19 = 756\: torr}\)

      For atm:  \(\mathrm{P_{H_2O} = 19\: torr\times\dfrac{1\:atm}{760\:torr} = 0.025\: atm}\);  \(\mathrm{P_{N_2} = P_T - P_{H_2O} = 1.02 - 0.025 = 0.99\: atm}\)

 

6.  \(\mathrm{P_{N_2}=0.50\: atm}\);  \(\mathrm{P_{O_2} = 0.30\: atm}\);  \(\mathrm{28.0\: g\: N_2}\); \(\mathrm{n_T = ?}\)

      \(\mathrm{P_T = P_{N_2} + P_{O_2} = 0.50\: atm + 0.30\: atm = 0.80\: atm}\);

      \(\mathrm{moles\: N_2 = 28.0\: g\: N_2 \times\dfrac{1\:mole\:N_2}{28.0\:g\:N_2} = 1.00\: mol\: N_2}\)

      \(\mathrm{P_{N_2}=\left(\dfrac{n_{N_2}}{n_T} \right )P_T}\)        \(\mathrm{n_T=\left(\dfrac{P_T}{P_{N_2}}\right)n_{N_2}=\left(\dfrac{0.80}{0.50}\right)1.00\:mol=1.6\:moles}\)

 

7. 

  1. \(\mathrm{2.80\: L \times\dfrac{1\:mole\:O_2}{22.4\:L\:O_2}\times\dfrac{4\:mole\:Na}{1\:mole\:O_2}\times\dfrac{23.0\:g\:Na}{1\:mole\:Na}=11.5\: g\: Na}\)
  2. First find molar volume at 25°C and 2.00 atm:

        \(\mathrm{V=\dfrac{nRT}{P}=\dfrac{(1.00\:mol)(0.08206)(298\:K)}{2.00\:atm}=12.2\:L}\)

        \(\mathrm{4.60\: g\: Na \times\dfrac{1\:mole\:Na}{23.0\:g\:Na}\times\dfrac{1\:mole\:O_2}{4\:mole\:Na}\times\dfrac{12.2\:L\:O_2}{1\:mole\:O_2}= 0.610\: L\: O_2}\)

 

8.  First find molar volume at 78°C and 1.20 atm.  See problem 2:  at 78°C and 1.20 atm, molar volume is 24.0 L/mole.

      molar mass of ethane (C2H6) = 2(12.0) + 6(1.0) =  30.0 g/mole

      \(\mathrm{d=\dfrac{mm}{mV}=\dfrac{30.0\:g}{24.0\:L}= 1.25\: g/L}\)