g of CO 2 gas is at a temperature of 45 o C and a pressure of 125 kpa. What is the volume of the container? 11 L

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1 Name period AP Chemistry Unit 5 answers 1. A fixed quantity of gas at 23⁰C exhibits a pressure of 748 torr and occupies a volume of 10.3 L. Calculate the volume the gas will occupy if the temperature is increased to 145 ⁰C 15 L 2. A fixed quantity of gas at 21⁰C exhibits a pressure of 748 torr and occupies a volume of 10.3 L. Calculate the volume the gas will occupy if the temperature is increased to 36 ⁰C and the pressure is decreased to 700 torr. 12 L 3. Nitrogen and hydrogen gases react to form ammonia gas a. Write a balanced chemical equation N 2 + 3H 2 2NH 3 b. At a certain temperature and pressure 0.70 L of nitrogen gas reacts with 2.1 L of hydrogen gas. If all the nitrogen and hydrogen are consumed, what volume of ammonia, at the same temp. and pressure, will be produced? 1.4 L 4. Calculate the following for an ideal gas a. The volume of gas if 1.57 mol has a pressure of 0.86 atm at a temperature of -12 ⁰C. 39 L b. The temp. of a gas of which mol occupies 164 ml at 693 torr K c. The pressure, in atm, if mol occupies 255 ml at 115⁰C 10.3 atm d. The grams of nitrogen gas, if 5.49L at 35 ⁰C has a pressure of kpa g g of CO 2 gas is at a temperature of 45 o C and a pressure of 125 kpa. What is the volume of the container? 11 L 6. If 128g of a certain gas in a container with a volume of 21.5 L has a pressure of 132 kpa and a temperature of 45 o C, what is the molar mass of the gas? 120 g/mol 7. If 4.0 L of a gas were produced at STP and the mass of the gas was found to be 12.8g, then what is the molar mass of the gas? 72 g/mol 8. a. How many grams of hydrogen gas can be produced by reacting 32.8 g of magnesium according to the following balanced equation? Mg (s) + 2 HCl (aq) MgCl 2 (aq) + H 2 (g) 2.70 g b. What volume of hydrogen gas was produced if this reaction was carried out at STP? 30.2 L 9. Nitrogen gas can be produced by reacting Na 3N with chlorine gas. If the reaction was carried out at STP with 34.8 g of Na 3N, what volume of nitrogen gas can be produced? 4.70 L 10. In a certain combustion reaction involving propane, 34.4 L of CO 2 was produced. How many liters of propane (C 3H 8) were combusted? Assume the reaction took place at STP L 11. a. Examine the two containers below. Both contain gases that were collected over water. Which one was collected at the higher temperature gas A or gas B? Explain your answer. there is more water vapor Gas A = Gas B = Water vapor = Water vapor =

2 12. A container of gas with a pressure of 450 kpa contained three different gases hydrogen, oxygen and nitrogen. If the partial pressure of hydrogen was 210 kpa and the partial pressure of oxygen was 125 kpa, what was the partial pressure of nitrogen? 115 kpa 13. A tank held neon gas at a pressure of 3.1 atm, helium at a pressure of 2.7 atm and argon at a pressure of 4.1 atm What was the pressure in the tank? 9.9 atm 14. Oxygen gas was collected over water at 30 o C. The pressure in the 2.5 L container was 110 kpa. If the container was allowed to expand to 7.0 L and if the temperature was decreased to -30 o C, what is the final pressure of the dry oxygen gas? 30 kpa or 230 torr 15. A quantity of oxygen gas was collected over water at 30 o C in a 475 ml container. The pressure in the container was measured to be 750 torr. How many grams of oxygen gas were collected? 0.6 g 16. How many grams of sodium are required to produce 31.9 L of H 2 at 755 mmhg and 290 K according to the following balanced equation? 2 HNO Na 2 NaNO 3 + H 2 61 g 17. Which gas is most dense at 1.00 atm and 298 K? Explain. a. CO 2 b. N 2O c. Cl Calculate the density of NO 2 gas at atm and 35 ⁰C g/l 19. Calculate the molar mass of a gas if 2.50 g occupies L at 685 torr and 35 ⁰C 80.1 g/mol 20. Calculate the molar mass of a vapor that has a density of g/l at 12 ⁰C and 825 torr. 154 g/mol 21. 2Mg (s) + O 2(g) 2MgO (s) If L of oxygen is reacted and has a partial pressure of 3.5 x 10-6 torr at 27 ⁰C, what mass of magnesium will react? 3.5 x 10-9 g 22. Ammonium sulfate, an important fertilizer, can be prepared by the reaction of ammonia with sulfuric acid. a. Write a balanced reaction 2NH 3 + H 2SO 4 (NH 4) 2SO 4 b. Calculate the volume of ammonia needed at 20 ⁰C and 25.0 atm to react with 150 kg of sulfuric acid. 2,940 L 23. Hydrogen gas is produced when zinc reacts with sulfuric acid a. Write a balanced chemical reaction. Zn + H 2SO 4 ZnSO 4 + H 2 b. If 159 ml of wet hydrogen gas is collected over water at 24 ⁰C and a barometric pressure of 738 torr, how many grams of zinc has been consumed? g 24. A mixture containing mol of He gas, mol Ne gas, and mol Ar gas is confined in a 7.00 L vessel at 25 ⁰C. a. Calculate the partial pressure of each gas in the mixture atm He; 1.10 atm Ne; atm Ar b. Calculate the total pressure of the mixture atm 25. A mixture of gases contains 0.75 mol N 2, 0.30 mol O 2, and 0.15 mol of CO 2. If the total pressure of the mixture is 1.56 atm, what is the partial pressure of each component? 0.98 atm nitrogen; 0.39 atm oxygen; 0.20 atm carbon dioxide

3 26. Place the following gases in order of increasing average molecular speeds at 300 K: CO 2, N 2O, HF, F 2, H 2 CO 2=N 2O < F 2<HF <H Under what conditions of temp. and pressure do gases usually behave nonideally? Low temp and high pressure 28. Would you expect water or carbon dioxide to behave more like an ideal gas at high pressures? Carbon dioxide 29. How do viscosity and surface tension change as intermolecular forces become stronger? More viscose and higher surface tension 30. How do viscosity and surface tension change as temperature increases? Less viscose and less surface tension 31. Explain why the heat of fusion of any substance is generally lower than its heat of vaporization less bonds are being broken when melting than vaporizing so it takes less energy 32. Explain how each of the following affects the vapor pressure of a liquid a. Volume of the liquid b. surface area c. intermolecular attractive forces d. temperature No affect no affect higher IMF = lower vapor pressure higher temp=higher vapor pressure 33. Phosphorus trichloride is more volatile than arsenic trichloride. a. Which substance has greater intermolecular forces? Arsenic trichloride b. Which substance as a higher vapor pressure at 25 C? phosphorus trichloride c. Which substance will have the higher boiling point? Arsenic trichloride 34. Two pans of water are on different burners of a stove. One pan of water is boiling vigorously, while the other is boiling gently. What can be said about the temperature of the water in the two pans? They are the same 35. Mt. McKinley in Alaska is the tallest peak in the United States. If the barometric pressure at the top is 340 torr, at what temperature will water boil there? Between ⁰C (closer to 80⁰C) 36. As the intermolecular attractive forces between molecules increases, do you expect each of the following to increase or decrease? a. Vapor pressure b. heat of vaporization c. boiling point d. freezing point Decrease increase increase increase b. Viscosity f. surface tension g. critical temperature Increase increase increase 37. A sample of a pure, gaseous hydrocarbon is introduced into a previously evacuated rigid 1.00 L vessel. The pressure of the gas is atm at a temperature of 127 o C. a) Calculate the number of moles of the hydrocarbon in the vessel x 10-3 mol (1 point earned for showing the setup and a second point earned for correct answer) b) O 2(g) is introduced into the same vessel containing the hydrocarbon. After the addition of the O 2(g), the total pressure of the gas mixture in the vessel is 1.40 atm at 127 o C. Calculate the partial pressure of O 2(g) in the vessel atom atm = 1.20 atm ( 1 point earned for correct answer) The mixture of the hydrocarbon and oxygen is sparked so that a complete combustion reaction occurs, producing CO 2(g) and H 2O(g). The partial pressures of these gases at 127 o C are atm for CO 2(g) and atm for H 2O(g). There is O 2(g) remaining in the container after the reaction is complete.

4 c) Use the partial pressures of CO 2(g) and H 2O(g) to calculate the partial pressure of the O 2(g) consumed in the combustion mol O 2 are used to make water; moles of O 2 are used to make CO 2 so mol of O 2 moles are consumed which has a pressure of 1.00 atm 1 point is earned for the correct stoichiometry in O2 consumption. 1 point is earned for the calculated result. d) On the basis of your answers above, write the balanced chemical equation for the combustion reaction and determine the formula of the hydrocarbon atm : 1.00 atm : atm : atm = 1 : 5 : 3 : 4 C3H8 + 5 O2 3 CO2 + 4 H2O 1 point is earned for the formula of the hydrocarbon. 1 point is earned for a balanced equation with the correct proportions among reactants and products. e) Calculate the mass of the hydrocarbon that was combusted. (6.09 x 10-3 mol)(44.1 g/mol) = g 1 point is earned for using the number of moles combusted from part (a). 1 point is earned for the calculated mass. 38. A sample of C 2H 4(g) is placed in a previously evacuated, rigid 2.0 L container and heated from 300 K to 450 K. The pressure of the sample is measured and plotted in the graph below. Describe TWO reasons why the pressure changes as the temperature of the C 2H 4(g) increases. Your descriptions must be in terms of what occurs at the molecular level. Two reasons are: (1) As the temperature increases, the average speed of the molecules increases and the molecules collide more frequently with the container walls. (2) As the temperature increases, the average kinetic energy of the molecules increases and the molecules strike the walls of the container with greater force. 39. A rigid 8.20 L flask contains a mixture of 2.50 moles of H 2, mole of O 2, and sufficient Ar so that the partial pressure of Ar in the flask is 2.00 atm. The temperature is 127 o C. a. calculate the total pressure in the flask atm b. calculate the mole fraction of H 2 in the flask

5 c. Calculate the density (in g L -1 ) of the mixture in the flask g L - The mixture in the flask is ignited by a spark, and the reactions represented below occurs until one of the reactants is entirely consumed. 2H 2(g) + O 2(g) 2H 2O(g) d. Give the mole fraction of all species present in the flask at the end of the reaction H 2: O 2: 0 (not necessary) Ar: H 2O: Review: 40. Write a balanced net ionic reaction a. Silver nitrate + sodium phosphate 3Ag + + PO 4 3- Ag 3PO 4 Label all the strong electrolytes silver nitrate, sodium phosphate, sodium nitrate b. Hydrogen gas + potassium carbonate H 2 + K + + CO 3 2- CO 2 + H 2O + K Label all the nonelectrolytes H 2, CO 2, H 2O 41. How many protons, neutrons, and electrons are in the following a. 65 Zn 2+ b. 40 Ar c. 14 N 3- d. 23 Na + 30, 35, 28 18, 22, 18 7,7,10 11, 12, Arrange the following substances according to their expected lattice energies, listed them from lowest lattice energy to highest: LiCl, KCl, KBr, CaO KBr, KCl, LiCl, CaO 43. Which member of the following pairs of substances would you expect to have a higher boiling point? a. N 2 or O 2 b. NaCl or CH 3Cl c. CH 3Cl or CH Which of the following factors most directly determines the number of peaks in a photoelectron spectrum? a. The number of electrons b. The number of shells c. The number of subshells containing electrons d. The number of orbitals containing electrons 45. Using principles of chemical bonding and molecular geometry, explain each of the following observations. Lewis electron-dot diagrams and sketches of molecules may be helpful as part of your explanations. For each observation, your answer must include references to both substances. a. The bonds in nitrite ion, NO 2-, are shorter than the bonds in nitrate ion, NO 3-. According to the Lewis electron-dot diagram, two resonance structures are required to represent the bonding in the NO 2 ion. The effective number of bonds between N and O is 1.5. Three resonance structures are required to represent the bonding in the NO 3 ion. The effective number of bonds between N and O is The greater the effective number of bonds, the shorter the N O bond length. b. The CH 2F 2 molecule is polar, whereas the CF 4 molecule is not. The molecular geometry in both CH 2F 2 and CF 4 is tetrahedral (or the same). The C-F bond is polar. In CF 4, the molecular geometry arranges the C-F dipoles so that they cancel out and the molecule is nonpolar. The C-H bond is less polar than the C-F bond. The two C-H dipoles do not cancel the two C-F dipoles in CH 2F 2.

6 c. The atoms in a C 2H 4 molecule are located in a single plane, whereas those in a C 2H 6 molecule are not. The carbon atoms in C 2H 4 have a molecular geometry around each carbon atom that is trigonal planar, so all six atoms are in the same plane. The carbon atoms in C 2H 6 have a molecular geometry that is tetrahedral, so the atoms are not all in the same plane. OR The carbon-carbon double bond in C 2H 4 results in a planar molecule whereas the carbon-carbon single bond in C 2H 6 results in a non-planar (tetrahedral) site at each carbon atom. d. The shape of a PF 5 molecule differs from that of an IF 5 molecule In PF 5, the molecular geometry is trigonal bipyramidal because the phosphorus atom has five bonding pairs of electrons and no lone pairs of electrons. IF 5 has square pyramidal molecular geometry. The central iodine atom has five bonding pairs of electrons and one lone pair of electrons. The presence of the additional lone pair of electrons on the central iodine atom means the molecular geometry is different. 46. A compound that contains only C and H was burned in excess oxygen. The following masses were obtained after the complete combustion of the compound in oxygen: 22.0 g of CO 2 and 18.0 g H 2O produced by the combustion. Identify the correct empirical formula for the hydrocarbon. a. CH b. CH 2 c. CH 3 d. CH 4

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