Chemistry 100. Assignment # 7. Gases, Liquids, and Solutions

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1 1. Define the following terms: a. Absolute temperature Chemistry 100 Assignment # 7 Gases, Liquids, and Solutions Absolute temperature, T, is the temperature reported using the absolute (or Kelvin) scale. To convert the Celsius temperature to the Kelvin scale, simply add 273 to the Celsius temperature. (Notice that the degree symbol in not used with the Kelvin scale) K = C b. STP conditions Standard Temperature and Pressure conditions (STP) are standard conditions of 0 C (273 K) and 760 mmg (1 atm or kpa). c. Molar volume of a gas Molar volume of a gas is the volume occupied by 1 mole of any gas molecules at STP. It is equal to 22.4 L. 2. a. What makes a gas gaseous? In gases, molecules are separated from each other by a relatively large amount of space. There is very little attractive force between gas molecules and, consequently, they are in constant motion. This attractive force is enough to cause gases to condense to liquids at lower temperatures and higher pressures but it is not strong enough to overcome molecular motions at normal conditions. b. ow can you make a substance a gas, a liquid, or a solid? A substance can be changed into a gas, a liquid, or a solid by changing its temperature and pressure. At higher temperatures and lower pressures, a substance is more likely to become a gas whereas at lower temperatures and higher pressures, a substance is more likely to become a solid. 3. Determine the density of ammonia gas, N 3, at STP (in grams per liter, remember the molar volume of a gas at STP is 22.4 L/mol).

2 The molar volume of ammonia gas at STP conditions is 22.4 L/mol. The molar mass of ammonia is 17.0 g/mol. density of ammonia gas is g/l 4. What is the molar mass for a gas with a density of 1.96 g/l at STP? The same formula from question # 3 can be used to calculate the molar mass of the gas. mass of one mole of the gas (molar mass of the gas) is 43.9 g/mol 5. What volume of 2 (g) is produced at 25 and normal pressure of 1 atm by electrolysis of 26.0 g of 2 O? 2 2 O (l) 2 2 (g) + O 2 (g) moles of water used = 1.44 mol. moles of 2 used = (2/2) x 1.44 mol = 1.44 mol At STP, the volume of 1 mole of 2 gas is 22.4 L. Therefore, the volume of 2 gas produced at STP is 1.44 mol x 22.4 L/mol = 32.3 L. Use the formula on next page to then calculate the volume produced at 25 and 1 atm.

3 P 1 = 1 atm P 2 = 1 atm V 1 = 32.3 L V 2 =? T 1 = 273 K T 2 = (273+25) K The volume of 2 gas at 25 and normal pressure of 1 atm is 35.3 L 6. Calcium carbide, CaC 2, reacts with water to produce acetylene gas, C 2 2, which is burned in miners lamps by spelunkers while cave exploring. CaC 2 (s) O (l) Ca(O) 2 (s) + C 2 2 (g) ow many milliliters of acetylene can be produced at a temperature of 20 and a pressure of 740 mmg by the complete reaction of 2.50 g of CaC2? molar mass of CaC 2 is 64.1 g/mol. Use the formula below to calculate the moles of CaC 2 moles of CaC 2 is mol moles of C 2 2 = moles of CaC 2 = mol At STP, the volume of C 2 2 gas = mol x 22.4 L/mol = L (or 874 ml) Use the formula below to then calculate the volume produced at 20 and 740 mmg. P 1 = 760 mmg P 2 = 740 mmg V 1 = L V 2 =? T 1 = 273 K T 2 = (273+20) K The volume of C 2 2 gas at 20 and pressure of 740 mmg is L (or 963 ml)

4 7. Arrange the following compounds in the order of increasing boiling points (lowest first): C 2 6, C 2 5 O, C 3 F A higher degree of intermolecular attractive forces between molecules leads to a higher boiling point. Compounds whose molecules have higher molecular weights generally have more intermolecular forces, and consequently, have higher boiling points than compounds whose molecules have smaller molecular weights. Polar compounds generally have higher boiling points than nonpolar ones with the same approximate mass. ydrogen bonding between molecules will also lead to higher boiling points. Ethane, C 2 6, and fluoromethane, C 3 F, approximately have the same mass but C 3 F is polar. Therefore, C 3 F is expected to have a higher boiling point. Ethanol, C 2 5 O, on the other hand has a higher molecular weight than ethane or fuoromethane. It is polar and its molecules show hydrogen bonding interactions. Therefore, it is expected to have the highest boiling point of the three. C 2 6 < C 3 F < C 2 5 O 8. Which has a higher boiling point: water, 2 O, or methanol, C 3 O? Explain. Both compounds are polar and they both have molecules that show hydrogen bonding. owever, there is a more extensive degree of hydrogen bonding in water and, therefore, water is expected to have a higher boiling point than methanol. O O O 3 C O C 3 O 9. a. Why is sugar soluble in water whereas cooking oil is not? Sugar is soluble in water due to the presence of many O groups in the molecules of sugar. These O groups lead to the formation of many hydrogen bonds between water and the sugar molecules. Cooking oil is made up of a long chain of connected carbon atoms and is relatively nonpolar (it has a long hydrophobic tail that cannot form hydrogen bonds with water). The lack of attractive forces between oil molecules and water molecules make them insoluble in each other (they are immiscible).

5 b. Provide a reasonable explanation as to why iodine, I 2, is only slightly soluble in water. Iodine molecules are diatomic, with one covalent bond between the two iodine atoms. This makes the iodine molecules nonpolar. Nonpolar substances tend to be insoluble in water as their molecules lack favourable interactions with water molecules. 10. a. What is meant by the term normal boiling point? The normal boiling point is the temperature at which the vapour pressure of a liquid equals standard atmospheric pressure (1 atm). (when the external pressure is equal to 1 atm, the temperature at which the liquid boils is its normal boiling point) b. Do you expect water to boil slower or faster on top of Mt. Tolmie? Explain. Boiling can be speeded up if the external pressure is reduced. On top of Mt. Tolmie, the external pressure is lower than the pressure at sea level. Therefore, water is expected to boil faster on top of Mt. Tolmie. 11. What is the molarity of a solution that contains 2.50 g CaCl 2 in 987 ml of water? moles of CaCl 2 = mol Molarity of solution is mol/l (or 2.28x10-2 mol) 12. What is the mass of Na 2 SO 4 in 700 grams of a 3.50% (w/w) sodium sulfate solution? In a 3.50% (w/w) solution, there are 3.50 grams of sodium sulfate in 100 grams of solution. In 700 grams of solution, there are (700/100) x 3.50 g of sodium sulfate. mass of sodium sulfate is 24.5 g

6 13. ow many moles of Br are in 35.0 ml of 2.80 M Br? moles of Br = mol (or 9.80x10-2 mol) 14. To 15.0 ml of 11.8 M Cl was added 32.0 ml of water. What is the final concentration of the solution? The initial volume is 15.0 ml. The final volume is (15.0 ml ml) or 47.0 ml. Since both volumes are in ml, we need not convert these into liters in order to simplify the calculations. M 1 x V 1 = M 2 x V M x 15.0 ml = M 2 x 47.0 ml the final concentration of the solution is 3.77 M 15. Consider the following reaction: Ca (s) + 2 Cl (aq) CaCl 2 (aq) + 2 (g) What is the required mass of calcium metal if the reaction uses up 50.0 ml of M Cl? Volume of solution is (50.0 ml / 1000 L/mL) = L moles of Cl used is mol moles Ca metal used is (1/2) x mol = mol mass of Ca metal used is x 40.1 g/mol = g 16. a. Write the dissociation equation for potassium sulfate, K 2 SO 4. K 2 SO 4 2 K + + SO 4 2-

7 b. What is the K + ion concentration in 0.40 M K 2 SO 4? One mole of K 2 SO 4 gives two moles of potassium ions when dissociated. K + ion concentration is (2/1) x 0.40 M = 0.80 M c. What is the SO 4 2- ion concentration in 0.40 M K 2 SO 4? One mole of K 2 SO 4 gives one mole of sulfate ions when dissociated. SO 4 2- ion concentration is (1/1) x 0.40 M = 0.40 M 17. Are the following solutions acidic, basic, or neutral? If the p is < 7, the solution is acidic. If the p is > 7, the solution is basic. If the p is 7, the solution is neutral. a. p = 4 acidic b. [ + ] = 10-7 M p = -log [ + ] = - log 10-7 = 7 c. [ + ] = M p = -log [ + ] = - log = 11 d. [ + ] = 2.5 M p = -log [ + ] = - log 2.5 = 0.40 neutral basic acidic

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