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Question 1 (1 point) Given the following data: N2O(g) + 3H2(g) N2H4(l) + H2O(l) H = -317.0 kJ fH (N2O(g)) = 82.1 kJ fH (H2O(l)) = -285.
Question 1 (1 point) Given the following data:H° = –317.0 kJfH° (N2O(g)) = 82.1 kJfH° (H2O(l)) = –285.8 kJthe standard enthalpy of formation of hydrazine, fH° (N2H4(l)), isQuestion 1 options:A)317.0 + 82.1 – 285.8.B)–317.0 – 82.1 + 285.8.C)–317.0 + 82.1 – 285.8.D)–317.0 + 82.1 + 285.8.E)317.0 – 82.1 – 285.8.SaveQuestion 2 (1 point) What is the enthalpy change when 7.54 g of TiO(s) reacts with excess liquid bromine?2TiO(s) + 2Br2(l) → 2TiBr2(s) + O2(g)Ho = 235.4 kJ/molQuestion 2 options:A)27.8 kJB)1770 kJC)887 kJD)13.9 kJE)471 kJSaveQuestion 3 (1 point) Using the following thermochemical data, calculate fHo of Y2O3(s).4YCl3(s) + 3O2(g) → 2Y2O3(s) + 6Cl2(g)Ho = 189.4 kJ/mol2Y(s) + 3Cl2(g) → 2YCl3(s)Ho = –2000.0 kJ/molQuestion 3 options:A)–1905.3 kJ/molB)–3810.6 kJ/molC)94.7 kJ/molD)–1810.6 kJ/molE)–2189.4 kJ/molSaveQuestion 4 (1 point) The kinetic energy of a 2.50 kg ball rolling down a hill at 0.500 m/s would beQuestion 4 options:A)0.313 J.B)0.625 J.C)0.200 J.D)5.00 J.E)1.25 J.SaveQuestion 5 (1 point) In a calorimetry experiment, 0.0157 g of calcium metal are added to 42.8 mL of 0.706 M hydrochloric acid, initially at 22.78oC, in an insulated container. The temperature of the solution rises to 23.97oC. What is Ho for the following reaction? Assume the density and specific heat of the acid solution are the same as those of water, 1.00 g/mL and 4.184 J g-1 oC-1 respectively, and neglect the heat capacity of the container.Ca(s) + 2HCl(aq) → CaCl2(aq) + H2(g)Question 5 options:A)–14.1 kJ/molB)–6.95 kJ/molC)–543 kJ/molD)213 kJ/molE)–70.9 kJ/molSaveQuestion 6 (1 point) The specific heat of iron is 0.449 J g-1 oC-1. What is its molar heat capacity?Question 6 options:A)25.1 J mol-1 oC-1B)124 J mol-1 oC-1C)0.00804 J mol-1 oC-1D)4.18 J mol-1 oC-1E)0.0399 J mol-1 oC-1SaveQuestion 7 (1 point) The units for heat capacity areQuestion 7 options:A)(J • g).B)J/g.C)(J • °C).D)J/°C.E)J/(g • °C).SaveQuestion 8 (1 point) For which of the following reactions would H most nearly equal U?Question 8 options:A)B)C)D)E)SaveQuestion 9 (1 point) How much heat is liberated at constant pressure when 2.65 g of ethane, C2H6, are combusted in excess oxygen?2C2H6(g) + 7O2(g) → 4CO2(g) + 6H2O(l)SubstancefH°(kJ/mol)C2H6(g)–83.8CO2(g)-393.5H2O(l)-285.8Question 9 options:A)5.19 × 101 kJB)3.12 × 103 kJC)1.38 × 102 kJD)7.63 × 102 kJE)4.14 × 103 kJSaveQuestion 10 (1 point) Using the following thermochemical data, calculate fHo of Lu2O3(s).2LuCl3(s) + 3H2O(l) → Lu2O3(s) + 6HCl(g)Ho = 316.6 kJ/mol2Lu(s) + 3Cl2(g) → 2LuCl3(s)Ho = –1891.2 kJ/mol4HCl(g) + O2(g) → 2Cl2(g) + 2H2O(l)Ho = –202.4 kJ/molQuestion 10 options:A)–1777.0 kJ/molB)2410.2 kJ/molC)–1878.2 kJ/molD)1372.2 kJ/molE)–2005.4 kJ/molSaveQuestion 11 (1 point) Hawaiian macadamia nuts provide about 190 Cal of energy usable from the digestion of these nuts per 1.0 oz serving. If the usable energy in an 8.5 oz can were used to light a 100-watt (W) light bulb (1 W = 1 J⋅s), how many hours would the light bulb run from one can of these snacks?Question 11 options:A)1.1 x 103 hrB)1.9 x 10-2 hrC)1.9 x 101 hrD)6.8 x 104 hrE)2.2 x 101 hrSaveQuestion 12 (1 point) When the space shuttle lifts off on a mission from Cape Canaveral, the chemical potential energy of the fuel is converted intoQuestion 12 options:A)sound energy.B)kinetic energy.C)heat.D)all of the above.E)light energy.SaveQuestion 13 (1 point) A gas expands from 1.12 L to 5.53 L against a constant external pressure of 8.33 atm. What is the value of w? (1 L atm = 101.3 J)Question 13 options:A)–3.72 × 103 JB)–36.7 JC)3.72 × 103 JD)36.7 JE)–4.47 × 102 JSaveQuestion 14 (1 point) For the following unbalanced reaction, when the rHº value is calculated using only fHº values, which of the following would correctly represent the term used for the fHº of N2O(g) which would be substituted into the rHº summation equation?Question 14 options:A)3B)1/3C)D)-E)-3SaveQuestion 15 (1 point) Calculate U of a gas for a process in which the gas absorbs 18 J of heat and does 6 J of work by expanding.Question 15 options:A)–12 JB)+12 JC)–24 JD)+24 JE)None of the aboveSaveQuestion 16 (1 point) A flask contains 22.5 g of an unknown liquid, initially at 14.0oC. After 2.34 kJ of heat are added to the liquid, its final temperature is 56.3oC. What is the specific heat of the liquid?Question 16 options:A)2.46 J g-1 oC-1B)7.43 J g-1 oC-1C)0.407 J g-1 oC-1D)4.18 J g-1 oC-1E)42.3 J g-1 oC-1SaveQuestion 17 (1 point) Consider the following specific heats of metals.MetalSpecific Heatcopper0.385 J/(g · °C)magnesium1.02 J/(g · °C)mercury0.138 J/(g · °C)silver0.237 J/(g · °C)lead0.129 J/(g · °C)If the same amount of heat is added to 25.0 g of each of the metals, which are all at the same temperature, which metal will have the highest temperature?Question 17 options:A)MercuryB)SilverC)LeadD)MagnesiumE)CopperSaveQuestion 18 (1 point) A 34.9-g sample of an unknown metal, initially at 232.8oC, is immersed in a 17.0-g sample of water (specific heat = 4.184 J g-1 oC-1), initially at 15.4oC, in an insulated cup. Once equilibrium is reached, the final temperature of the water-metal mixture is 28.2oC. What is the identity of the metal?MetalSpecific Heat (J g-1 oC-1)Copper0.385Lead0.128Silver0.235Aluminum0.902Question 18 options:A)copperB)silverC)leadD)aluminumE)None of the aboveSaveQuestion 19 (1 point) Which of the following equations represents the equation for the fH° for N, N-diethyl-m-toluamide, C12H17NO(l), the active ingredient in some insect repellents?Question 19 options:C12H17NO(l)C12H17NO(g)C12H17NO(l)C12H17NO(l)C12H17NO(l)SaveQuestion 20 (1 point) Consider the following specific heats of metals.MetalSpecific Heatcopper0.385 J/(g • °C)cobalt0.418 J/(g • °C)chromium0.447 J/(g • °C)gold0.129 J/(g • °C)silver0.237 J/(g • °C)100-g samples of each of the metals at 95°C are added to 100 mL of water at 25°C. Which element will increase the temperature of the water the least?Question 20 options:A)ChromiumB)CopperC)CobaltD)GoldE)SilverSave