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.
Question
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.
Solution
The text you provided is in English, so I will continue to respond in English.
(a) O2(g) is reduced in the reaction. This is because the oxidation number of Oxygen changes from 0 in O2 to -2 in CO2 and H2O, indicating that it has gained electrons, which is the definition of reduction.
(b) To determine the number of moles of CO2(g) produced, we can use the ideal gas law equation, PV = nRT. Rearranging for n, we get n = PV/RT. Substituting the given values, we get n = (1.03 atm * 18.0 L) / (0.0821 Latm/molK * 294.85 K) = 0.766 moles of CO2.
(c) The balanced chemical equation for the combustion of ethanol is C2H5OH + 3O2 -> 2CO2 + 3H2O. From this, we can see that 1 mole of ethanol produces 2 moles of CO2. Therefore, 0.766 moles of CO2 corresponds to 0.383 moles of ethanol. Using the molar mass of ethanol (46.07 g/mol), this is equivalent to 17.66 g of ethanol. Given the density of ethanol is 0.79 g/mL, this corresponds to 22.3 mL of ethanol.
(d) The heat released by the combustion reaction cannot be determined without additional information such as the heat of combustion of ethanol.
(e) The final temperature of the air in the room after the combustion cannot be determined without knowing the amount of heat released by the combustion reaction.
(f) The intermolecular force most responsible for the difference in boiling point between ethanol and dimethyl ether is hydrogen bonding. Ethanol can form hydrogen bonds due to the presence of the -OH group, while dimethyl ether cannot. Hydrogen bonds are stronger than the dipole-dipole interactions and dispersion forces that dimethyl ether can form, leading to a higher boiling point for ethanol.
(g) To maximize the amount of C2H5OH(g) produced, the chemist could increase the pressure or decrease the temperature. According to Le Chatelier's principle, increasing the pressure will shift the equilibrium to the side with fewer moles of gas, which is the product side in this case. Decreasing the temperature will shift the equilibrium to the side that absorbs heat, which is also the product side since the reaction is exothermic.
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