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- A waste heat exchanger is used to absorb the energy from the complete combustion of hydrogen sulfide gas. What volume of water undergoing a temperature change of 52 degrees Celsius is required to absorb all of the energy from the burning of 12 kg of hydrogen sulfide? * 0.85 mL 0.84 L 840 g 0.85 g please explain and give correct answerUsing car miles per gallon and the miles you drive in 1 week calculate the liters of carbon dioxide you produce when using your car. Compare your miles in February (pre-covid) versus June (post-covid). Assume that your engine combusts at 1.00 atm and 25.0 celsius. Assume that your gasoline is 100% octane (C8H18). You will also need to balance the combustion reaction that occurs in your car engine. You will need to use PV=nRTEthanol Fuel C2H6O is burned with atmospheric air in a stoichiometric ratio. The coefficient of air is:Select one:a. 13.8b. 14.28c. 12.8d. 13.3
- The citizens of the world burn the fossil fuel equivalent of 7 * 1012 kg of petroleum per year. Assume that all of this petroleum is in the form of octane (C8H18) and calculate how much CO2 (in kg) the world produces from fossil fuel combustion per year. (Hint: Begin by writing a balanced equation for the combustion of octane.) If the atmosphere currently contains approximately3 * 1015 kg of CO2, how long will it take for the world’s fossil fuel combustion to double the amount of atmospheric carbon dioxide?Isooctane (2,2,4-trimethylpentane), one of the many hydrocarbons that make up gasoline, burns in air to give carbon dioxide and water. 2C8H18(l)+25O2(g)⟶16CO2(g)+H2O(l)2C8H18(l)+25O2(g)⟶16CO2(g)+H2O(l) ΔH=−10,922kJΔH=−10,922kJ Calculate the mass, in g, of C8H18C8H18 that reacts if 6112.23 kJ of heat is released in the process.How many moles of O2 are needed to burn 1.45 mol of C8H18? Express the amount in moles to three significant digits. The complete combustion of octane, C8H18, a component of gasoline, proceeds as follows: 2C8H18(l)+25O2(g)→16CO2(g)+18H2O(g) Relevant volumetric equivalencies 1 gal = 3.785 L 1 L = 1000 mL
- Calculate the number of pounds of CO2 released into the atmosphere when a 10.0 gallon tank of gasoline is burned in an automobile engine. Assume that gasoline is primarily octane, C8H18,C8H18, and that the density of gasoline is 0.692 g⋅mL−1. This assumption ignores additives. Also, assume complete combustion.The emission of NO2 by fossil fuel combustion can be prevented by injecting gaseous urea into the combustion mixture. The urea reduces NO (which oxidizes in air to form NO2) according to the reaction:2 CO(NH2)2( g) + 4 NO( g) + O2( g)------------->4 N2( g) + 2 CO2( g) + 4 H2O( g)Suppose that the exhaust stream of an automobile has a flow rate of 2.55 L/s at 655 K and contains a partial pressure of NO of 12.4 torr. What total mass of urea is necessary to react completely with the NO formed during 8.0 hours of driving?What volume of CH4(g), measured at 25 ºC and 745 mmHg, must be burned in excess oxygen to release 1.00 x 106kJ of heat to the surroundings? (PV=nRT, R=0.08206 ?∙??????∙?, 1 atm = 760mmHg) CH4(g) + 2O2(g) → CO2(g) + 2H2O(l) ∆Hrxn = -890.3kJ/mol
- Hi, I need help how to solve this problem in attached file. “ ammonia can be generated according to the balanced chemical equation: N2(g) + 3H2 (g) -> 2NH3 (g) if the reaction begins with 2.00kg of H2 as the limiting reactant, what size tank will be required to store the ammonia at STP conditions?”  I know the answer is 14,800 L, but I am struggling to know step-by-step on how to find that answer.The enthalpy of combustion of methane is -890 kJ . The volume of methane at 0 degrees Celsius and 1 atm to be burnt to produce 2670 kJ heat is? Choices : 33.6 L, 67.2L, 7.47 L, 11.2 LButane gas, C4H10, is sold to campers as bottled fuel. Its density at 258C and 1.00 atm is 2.38 g/L. What volume of butane gas at 258C and 1.00 atm is required to heat one gallon of water (d 5 1.00 g/mL) from 258C to 988C? The reaction for the combustion of butane (DHf 8 5 2125.6 kJ/mol) is C H (g)113O (g)9:4CO (g)15H O(g)