ࡱ> 685:;  IbjbjVV 1X<<}}}8\%E((|||yE{E{E{E{E{E{E$GJE}|x|||EwE |l}yE |yE ADx1C8eEE0ED@K@KpD@K}D|| |||||EE0|||E||||@K||||||||| : The specific heat of iron is 0.451 J/g(K. When a 200.0 g iron slug is heated to 368oC and added to 60.0 g of water at 20.0oC, all of the heat lost by the iron is gained by the water. If the heat of vaporization of water is 2260 J/g, how many grams of water will vaporize? When gasoline burns in a car engine, the heat released causes the products CO2 and H2O to expand, which pushes the pistons outward. Excess heat is removed by the cars cooling system. If the expanding gases do 451 J of work on the pistons and the system loses 325 J to the surroundings as heat, calculate the change in energy ((E) in kcal. The standard enthalpy of combustion of liquid heptane (C7H16) is (4816.0 kJ/mol. The products of this combustion are liquid water and carbon dioxide gas. Calculate the standard enthalpy of formation of liquid n-heptane. Acetylene reacts with bromine according to the following equation: C2H2 + 2 Br2 (( C2H2Br4 From bond energies, calculate the standard enthalpy change for the reaction. Calculate the standard enthalpy of formation of solid magnesium hydroxide from the following data: 2 Mg(s) + O2(g) (( 2 MgO(s) (Ho = (1203.7 kJ MgO(s) + H2O(l) (( Mg(OH)2(s) (Ho = (36.7 kJ 2 H2O(l) (( 2 H2(g) + O2(g) (Ho = +571.6 kJ Ethanol is a major ingredient of a camping fuel called Sterno. If the energy released in the combustion of 5.00 g of ethanol (C2H6O) is transferred without loss to 200.0 g of liquid water at 22.0oC, what will be the final state and temperature of the water? (Combustion of one mole of ethanol yields 1235 kJ of energy) Aspirin is produced commercially from salicylic acid, C7O3H6. A large shipment of salicylic acid is contaminated with boric oxide, which like salicylic acid is a white powder. The heat of combustion of salicylic acid at constant volume is known to be 3.00 x 103 kJ/mol. Boric oxide, because it is fully oxidized, does not burn. When a 3.556 g sample of contaminated salicylic acid is burned in a bomb calorimeter, the temperature increases 2.556oC. From previous measurements, the heat capacity of the calorimeter is known to be 13.62 kJ/K. What is the amount of boric oxide in the sample, in terms of mass percent? A sample of neon gas has a volume of 3.15L and a pressure of 0.951 atm at 21(C. If the pressure increases to 1.564 atm and temperature remains constant, what is the final volume? Calculate the volume of O2 at 2.89 atm and 15oC required for the complete combustion of 125 g octane (C8H18) to CO2 and H2O. Consider the three boxes, all at 27oC, in the diagram below. Assuming the connecting tubes have negligible volumes, what is the partial pressure of each gas and the density of the final mixture when both of the stopcocks are opened?  EMBED PBrush  A 0.700 g sample of lithium metal is placed in an evacuated 1.00 L flask connected by a stopcock to a 1.00 L flask containing oxygen at a temperature of 25.0oC and 5.00 atm pressure. The stopcock is opened and the exothermic reaction allowed to proceed to completion. When the temperature of the system returns to 25.0oC, what will be the pressure? (assume that the volumes of Li(s) and Li2O(s) are negligible).  EMBED PBrush  The gaseous reaction below is followed by monitoring the total gas pressure in the reaction vessel. The temperature is held constant by a large water bath at 100oC. The initial pressure of CS2 and H2 was 0.558 torr. The final pressure was 0.480 torr. The limiting reactant, CS2 was entirely used up. Using Daltons Law of Partial Pressure, calculate the partial pressures of the other gases when the reaction was finished and the partial pressures of the two initial gases. Total PressureCS2(g) + 4 H2(g) ( CH4(g) + 2 H2S(g)Initial0.558 torr0 torr0 torr(Final0.480 torr0 torr One of the raw materials needed for the manufacture of sulfuric acid is the oxygen in the air, which is used to convert sulfur to sulfur trioxide. The sulfur trioxide can then be reacted with water to produce sulfuric acid. The reactions are 2 S(s) + 3 O2(g) ( 2 SO3(g) SO3(g) + H2O(l) ( H2SO4(l) What volume of air, measured at 1.10 atm and 500oC, would be needed to produce 1.000 x 103 kg of 98.9% sulfuric acid? Air is 20.9% oxygen by volume. If at a temperature T, the average speed of a CO2 molecule is 3.5 x 104 ms(1. What would be the average speed of a methane (CH4) molecule at the same temperature? A third gas has an average speed of 3.0 x 104 ms-1 and is composed of 40. %C, 6.7% H, and 53% O. Determine the molecular formula of this gas. Consider that you have three containers of a gas at the following conditions. Container A 800 mL CO2 @ 37oC and 1.00 atm pressure MW = 44 Container B 500 mL Ne @ 47oC and 1.80 atm pressure MW = 20 Container C 450 mL Ar @ 37oC and 1.20 atm pressure MW = 40 Identify The container with molecules possessing the highest kinetic energy. Why? The container with the largest number of molecules. Why? The container with the largest number of collisions per second. Why? The container with the fastest RMS (average) velocity. Why? The container with molecules possessing the highest average momentum (mass x velocity). Why? The container with the densest sample of gas. Why?     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