Mixed Extra Gas Law Practice Problems (Ideal Gas, Dalton’s Law of Partial Pressures, Graham’s Law) 1. Dry ice is carbon dioxide in the solid state. 1.28 grams of dry ice is placed in a 5.00isLmaintained chamber that at 35.1oC. What is the pressure in the chamber after all of the dry ice has sublimed? ��=��� 1.28 � ��! 1 ���� ��! 44.0091 � ��!= 0.29�849 ����� ��! P = ? V = 5.00 L (3 significant figures) n = 0.290849 moles (3 significant figures) R = 0.0821 L*atm/mole*K (infinite significant figures) T = 35.1oC = 308.1 K (4 significant figures) 0.290849 �������� �308.1 � ��� �����0.0821 �−− �= �= 5.00 �=1.47 ��� If you used a different R, then the answers are: 1120 torr 1120 mm Hg 149 kPa 2. A sample of chlorine gas is loaded into a 0.25 L bottle at standard temperature of pressure. How many moles of bromine gas are in the container? How many grams? At STP 1 mole = 22.4 L Molar Mass of Chlorine (remember, it is a diatomic) = 70.906 g/mole Use factor label 0.25 � 1 ���� ��! 22.4 1 � � ��!=0.011 ����� ��! TRVP =–273 OR 1 use 0.25 0.0821 atmKLthe (infinite (2 ideal L*atm/mole*K significant gas significant law, (infinite figures) PV 0.25 1=figures) �nRT significant � 1122.4 ���� ����� ��! ��!=0.79 ��!� figures) 70.906 � ��! � ��! 906 � ��!= 1.7 Square both Rearrange andsides solve for mass of the �!=unknown 13.011 ���� ��! 70.0821 �−− �������� �(273 �) 0. What is the volume of 92.4 L*mm Hg/mole*K (infinite significant figures) T = 46oC = 319 K (3 significant figures) n – need to calculate 92.�= �� 1 ���(0.4 �−− ��������� �(319 �) �= 694 ����=37.4 �= � 4.19 13.80����� � ���� �!" �! .906 � ��! 1 ���� 1� ��!=0.011 ����� ��! ��= 0.303133 ��� �����62.69= �!" 13.69= 84. What is the molar mass of a gas that effuses 3.25 �) =0.7 ����! �!" ����!"=�!=3.7 ����!" �� ����!"=3.4 grams of chlorine gas that is at a temperature of 46oC and a pressure of 694 mmHg? P = 694 mmHg (3 significant figures) V = ? R = 62.4 ����� ��! 1 ���� ��! 70.3�3133 ����� ��! 1 �−������ ������ �� ���� ����������� ������ 1.78 � ��! 3.7 times faster than Krypton? ����! ����!= �! �! A is the unknown gas (it effuses faster) B is Krypton (it effuses slower) ����! ����!=3.69=6. 3 ��� 2.3 ���=0.3 ��� 6.20at kPa.64= ����! �!" �! �� �!"! .5. What is the molar mass of a gas that effuses 4.2 ����!"! �!=4.123 g/mole Molar mass of I2 = 253.021�1767 1 ���� �!"#$%& !"#$"!%= �!"!#$− �!"#$% !"#$%=1.2 times faster than bromine? ����! �! ����!=�! A is the unknown gas (it effuses faster) B is Bromine (it effuses slower) Square both Rearrange andsides solve for mass of the unknown ����!=4.3 ���−0.123����� 7. what is the pressure of the dry gas alone? �!"#$%=1. Carbon dioxide is collected over water at a temperature of 18oC. The pressure of water 18oC isvapor 2. If the pressure of the gas collected is 1.20 ���= 101.2 ����!"!= ����! ����!"!=4.808����� =2.3 atm.20 1��� ��� �!"#$% !"#$%=2.09 ����!= 58.808 g/mole Butane will effuse more quickly because it has a smaller molar mass ����! ����!= �! �! A – butane B – iodine ����! 253.02171767 ���=1.2 17. What diffuses more quickly: tetracarbon decahydride or iodine? By how much? C4H10 versus I2 Molar mass of C4H10 = 58. 50�63 ���+2.808 ������ �!"! 17. What is the temperature of 83.4 �−− ��������� � . If the partial pressure of oxygen is 3.06 17. what is the total pressure? �!!= 3.89�340 ����� ��! 1 −������� ������ �� ���� ����������� ������ �� 1830 ����(3. A mixture of gases contains oxygen.892340 �����)62.3�997 1 � ��� 143 �� �� 1 ��� �!"= 143 �� ��= 760 �� ��=0.64=9.3 ���=2.82 L (3 significant figures) R = 62.7 ���+0.82 L container? P = 1830 torr (3 significant figures) V = 3.2 � ��= (1.3�997 ���+0.�!= 159. water vapor.28 grams of carbon dioxide at a pressure of 1830 torr contained in a 3.28 ����� ��! 1 ���� ��! 44.64= ���� 8.50�63 1 ���� 234 ��� 1 ��� �!"!= 234 ���= 101.82 �) �= =59.18�157 ���=6. carbon dioxide.7 ��� 382 �� 1����� �!!!= 382 �� ��= 760 �� ��=0.4 L*torr/mole*K (infinite significant figures) T = ? n – need to calculate 83.7 ��� 9. and the partial pressure of the argon is 143 mmHg. and argon.7 atm.18�157 1 � ��� �!"!#$= �!!+�!!!+ �!"!+ �!"= 3. the partial pressure of the water vapor is 382 mmHg.009 � ��!= 1. the partial pressure of the carbon dioxide is 234 kPa.
Report "Extra Practice Mixed Gas Law Problems Answers"