Question 2 Calculate the amount of heat released in the complete combustion of 8.17 grams of Al to form Al2O3(s) at 25°C and 1 atm. A for Al2O3(s)=-1676 kJ/mol OA. 237 kJ OB. 127 kJ OC.203 kJ OD. 101 KJ E. 254 kJ 4Al(s)+302(9)→2A1203(3)
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- What would be the heat of combustion of C4H10(g) if the heats of formation of C4H10(g), CO2(g), and H2O(l) are -124.73 kJ/mol, -393.5 kJ/mol, and -285.8 kJ/mol, respectively.C4H10(g) + 13/2O2(g) ↔ 4CO2(g) + 5H2O(l)(a) Calculate the standard enthalpy change for the combustion of 1 mol of benzene, C6H6(l), to CO2(g) and H2O(l).(b) Compare the quantity of heat produced by combustion of 1.00 g propane with that produced by 1.00 g benzene.A student performed the procedure described in the lab manual using 48.9 mL of 1.0 M HCl and 49.9 mL of 1.0 M NaOH. Reaction caused the temperature inside the calorimeter to increase from 17.9 oC to 24.7 oC. What is the value of the enthalpy change for this reaction (ΔHaqueous) in units of kJ/mol? (Enter your answer as a number without units.)
- Using the following equation for conversion of octane, calculate the heat associated with the combustion of 150.0g of the octane assuming complete combustion. The molar mass of octane is 114.33 g/mol. The molar mass of oxygen is 31.9988 g/ mole 2 C8H18+25O2 —> 16 CO2+ 18 H2O H degree rxn = -11018For a particular isomer of C8H18,C8H18, the combustion reaction produces 5099.5 kJ5099.5 kJ of heat per mole of C8H18(g)C8H18(g) consumed, under standard conditions. C8H18(g)+25/2 O2(g)⟶8CO2(g)+9H2O(g) ΔHrxn°=−5099.5 kJ/mol What is the standard enthalpy of formation of this isomer of C8H18(g)?Using the following equation for the combustion of postane, calculate the heat associated with the formation of 100.0 g of phosphorous dioxide. The molar mass of postane is 263.6 g/mole. The molar mass of phosphorous dioxide is 62.9 g/mole. 2 P8H18 + 25 O2 → 16 PO2 + 18 H2O ΔH°rxn = -12018 kJ
- For a particular isomer of C8H18, the combustion reaction produces 5113.3kJ of heat per mile of C8H18(g) consumed, under standard conditions. C8H18(g)+25/2O2(g) 8CO2(g)+9H2O(g) ∆H°rxn=-5113.3kJ/mol What is standard enthalpy of formation of this C8H18(g)? ∆Hf°= kJ/molMethanol, ethanol, and n-propanol are three common alcohols. When 1.00 g of each of these alcohols is burned in air, heat is liberated as follows: (a) methanol (CH3 OH), −22.6 kJ; (b) ethanol (C2 H5 OH), −29.7 kJ; (c) n-propanol (C3 H7 OH), −33.4 kJ. Calculate the heats of combustion of these alcohols in kJ/mol.Methanol undergoes combustion according to the equation. Find the amount of heat given off from the combustion of 64 g CH3OH (methanol). (MM = 32 g/mol) (∆H=-1452.8 kJ) 2 CH3OH(l) + 3 O2(g) -> 2 CO2(g) + 4 H2O(l) a. 726.4 kJ b. -1452.8 kJ c. -2179.2 kJ c. -2905.6 kJ
- The principal component of LPG is butane, C4H10 (g). If combustion of 1 mole of butane produces 126 kJ of heat, how much heat can be generated by complete combustion of 11.0-kg gas tank?A. -23 900 kJ B. 126 kJ C. -126 kJ D. 23 900kJMethanol undergoes combustion according to the equation. Find the amount of heat given off from the combustion of 64 g CH3OH (methanol). (MM = 32 g/mol) (∆H=-1452.8 kJ) 2 CH3OH(l) + 3 02(g) -> 2 C02(g) + 4 H2O(l) A. - 726.4 kJ B. -1452.8 kJ C. -2179.2 kJ D. -2905.6 kJ1. Determine the mass of CO2 produced by burning enough of octane to produce 1.00×10^2kJ of heat. C8H18(l)+25/2O2(g)→8CO2(g)+9H2O(g) ΔH∘rxn=−5074.1kJmol− Express your answer using three significant figures. 2.Which fuel contributes least to the increase in atmospheric CO2 per kJ of heat produced? propane methane octane