For the combustion reaction of ethanolCH3CH2OH(l)  +  3 O2(g)  →  2 CO2(g)  +  3 H2O(l)     ΔH  =  - 1368 kJ / mol CH3CH2OHchoose the correct energy profile:

For combustion of ethanol C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(l), the amount of heat produced as measured in bomb calormeter, is 1364.47 kJ/mol at 25°C. Assuming all gases are behaving ideally, the enthalpy of combustion ΔCH, for ethanol will be : (R = 8.314 kJ/mol)

Which expression gives the mass, in g, of ethanol required to produce 683.5 kJ of heat upon complete combustion?(Mr for ethanol = 46.0, ΔHθc=−1367 kJmol−1Δ𝐻𝑐𝜃=−1367 kJmol−1)A.     683.51367×46.0683.51367×46.0B.     1367683.5×46.01367683.5×46.0C.     683.5×46.01367683.5×46.01367D.     1367×46.0683.51367×46.0683.5

Ethanol, C2H5OH, will combust in air according to the equation above.(a) Is O2(𝑔) oxidized in the reaction, or is it reduced? Justify your answer in terms of oxidation numbers.BoldItalicUnderlineSuperscriptSubscriptUndoRedoΩBullet listNumbered listImage (12 image limit)Edit imageView imageDelete imageO2 is reduced since it gains electrons, changing its oxidation number from 0 in O2 to -2 19 / 10000 Word LimitQuestion 2(b) When a sample of C2H5OH was combusted, the volume of CO2(𝑔) produced was 18.0L when measured at 21.7°C and 1.03atm. Determine the number of moles of CO2(𝑔) that was produced.BoldItalicUnderlineSuperscriptSubscriptUndoRedoΩBullet listNumbered listImage (12 image limit)Edit imageView imageDelete imageUsing the equation n = PV/RT, I got the answer 0.766 moles 11 / 10000 Word LimitQuestion 3(c) Determine the volume of C2H5OH(𝑙), in mL, that was combusted to produce the volume of CO2(𝑔) collected in part (b). (The density of C2H5OH(𝑙) is 0.79g/mL.)BoldItalicUnderlineSuperscriptSubscriptUndoRedoΩBullet listNumbered listImage (12 image limit)Edit imageView imageDelete image.766 moles x 1/2 x 46g/1 mol x 1g /0.79 mL = 22.3 12 / 10000 Word LimitQuestion 4(d) Determine the amount of heat, in kJ, that is released by the combustion reaction.BoldItalicUnderlineSuperscriptSubscriptUndoRedoΩBullet listNumbered listImage (12 image limit)Edit imageView imageDelete image 0 / 10000 Word LimitQuestion 5The combustion reaction occurred in a closed room containing 5.56×104g of air originally at 21.7°C. Assume that all of the heat produced by the reaction was absorbed by the air (specific heat = 1.005 J/(g°C)) in the room.(e) Determine the final temperature of the air in the room after the combustion.BoldItalicUnderlineSuperscriptSubscriptUndoRedoΩBullet listNumbered listImage (12 image limit)Edit imageView imageDelete image 0 / 10000 Word LimitQuestion 6(f) The boiling points of ethanol and dimethyl ether are provided in the following table. Identify the intermolecular force that is most responsible for the difference in boiling point. In terms of this force, explain why the boiling point of ethanol is higher than that of dimethyl ether.Compound Structural Formula Boiling Point (°C)Ethanol 78Dimethyl ether −24BoldItalicUnderlineSuperscriptSubscriptUndoRedoΩBullet listNumbered listImage (12 image limit)Edit imageView imageDelete image 0 / 10000 Word LimitQuestion 7One method of producing ethanol is by the reaction of ethene and water, as represented below.C2H4(𝑔)+H2O(𝑔)⇄C2H5OH(𝑔)Δ𝐻°=−45kJ/mol𝑟𝑥𝑛(g) A chemist wants to run the reaction and maximize the amount of C2H5OH(𝑔) produced. Identify two ways the chemist could change the reaction conditions (other than adding or removing any chemical species) to favor the formation of more product. Justify your answer.

0.3 g of ethane undergoes combustion at 27°C in a bomb calorimeter. The temperature of calorimeter system (including the water) is found to rise by 0.5°C. The heat evolved during combustion of ethane at constant pressure is ________kJ mol–1.(Nearest integer)[Given : The heat capacity of the calorimeter system is 20 kJ K–1, R = 8.3 JK–1 mol–1.Assume ideal gas behaviour. Atomic mass of C and H are 12 and 1 g mol–1 respectively]

Acetone (3CH3COCH3) undergoes combustion in the presence of oxygen to produce carbon dioxide and water: 2C3H6O+9O2→6CO2+6H2OIf you have 8 moles of acetone, calculate the moles of oxygen needed for complete combustion