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- Hi! Are tou sure it's not [H2O] / [CO] [H2] ?C6H12O6(s)→C3H6O3(s)+C2H5OH(l)+CO2(g) Calculate ΔH∘rxnEstimate the heat released when ethene(CH2=CH2) reacts with HBr to giveCH3CH2Br. Bond enthalpies areC-H : 412 kJ/mol; C-C : 348 kJ/mol;C=C : 612 kJ/mol; C-Br : 276 kJ/mol;Br-Br : 193 kJ/mol; H-Br : 366 kJ/mol. Choose the correct answer:1. 1036 kJ/mol2. 58 kJ/mol3. 424 kJ/mol4. 200 kJ/mol5. 470 kJ/mol
- table of thermodynamic properties: - C2H4(g) Hf = 52.4 Gf = 68.4 S = 219.3 - H2O(l) Hf = -285.8 Gf = -237.1 S = 70.0 - C2H5OH(l) Hf = -277.6 Gf = -174.8 S = 160.7Given the following for the oxidation of 1-decanol. CH3(CH2)8CH2OH(l) + O2(g) → CO2(g) + H2O(l) a) Calculate the work done when 1 mole is oxidized at 1 atm pressure.a) H2O b) CH4 c) H3O+ d) NH3 e) C2H4
- Draw an expanded structural formula of pent-1-en-3-yne/ CH3-CC-CH=CH2 and then label each carbon. Indicate the longest and shortest C-H bond and predict the C—C single bond that has the highest BDE(bond dissociation energy).Estimate the heat released when 1-butene(CH3CH2CHCH2) reacts with bromine to give CH3CH2CHBrCH2Br. Bond enthalpies are CH : 412 kJ/mol; CC : 348 kJ/mol;CC : 612 kJ/mol; CBr : 276 kJ/mol;BrBr : 193 kJ/mol. 1.317 kJ/mol 2.507 kJ/mol 3.95 kJ/mol 4.288 kJ/mol 5.181 kJ/molAnswer the following questions about the conversion of the sucrose (C 12H 22O 11) in sugarcane to ethanol (C 2H 6O) and CO 2 according to the following unbalanced equation. In this way sugarcane is used as a renewable source of ethanol, which is used as a fuel additive in gasoline. C12H22O11(s) + H2O(l)---------->C2H6O(l) + CO2(g) sucrose ethanol a. What is the molar mass of sucrose? b. Balance the given equation. c. How many moles of ethanol are formed from 2 mol of sucrose? d. How many moles of water are needed to react with 10 mol of sucrose? e. How many grams of ethanol are formed from 0.550 mol of sucrose? f. How many grams of ethanol are formed from 34.2 g of sucrose? g. What is the theoretical yield of ethanol in grams from 17.1 g of sucrose? h. If 1.25 g of ethanol are formed in the reaction in part (g), what is the percent yield of ethanol?
- Do ethanol (C2H5OH) C and DCalculate the energy change of the following reaction: 2NO + O2→ 2NO2 ΔH: NO = 90.0 kJ/mol NO2= 34.0 kJ/mol O2= 0.0 kJ/mol a -180 kJ b -112 kJ c 35.0 kJ d -248 kJExplain why the boiling point of CH3CONH2 (221 °C) is signicantly higher than the boiling point of CH3CO2H (118 °C).