This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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a) (i) Butan-1-ol CH_3CH_2CH_2CH_2OH (ii) Hexanoic acid CH_3CH_2CH_2CH_2CH_2COOH b) (i) The conditions necessary for fermentation of glucose to take place are: • Yeast (as a source of enzymes like zymase) • Absence of oxygen (anaerobic conditions) • Temperature between 25^ and 40^ (optimum around 37^) (ii) One reagent that can be used to carry out process S (reduction of ethanoic acid to ethanol) is lithium aluminium hydride (LiAlH_4). (iii) • Gas P is ethene (CH_2=CH_2). This is formed by the dehydration of ethanol using concentrated sulfuric acid. • Gas T is methane (CH_4). This is formed by the decarboxylation of sodium ethanoate using dry sodium hydroxide (soda lime). (iv) Sodium hydroxide is kept dry during the reaction by mixing it with calcium oxide (CaO) to form soda lime. Calcium oxide is a drying agent and also helps prevent the sodium hydroxide from melting. c) Step 1: Calculate the molar mass of ethanol (C_2H_5OH). Molar mass of C_2H_5OH = (2 × 12.01) + (6 × 1.008) + (1 × 15.999) = 24.02 + 6.048 + 15.999 = 46.067 g/mol. Using approximate atomic masses (C=12, H=1, O=16): Molar mass of C_2H_5OH = (2 × 12) + (6 × 1) + (1 × 16) = 24 + 6 + 16 = 46 g/mol. Step 2: Calculate the number of moles of ethanol in 1 litre. Given that 1 litre of ethanol has a mass of 780 g. Moles of ethanol = MassMolar mass = 780 g46 g/mol ≈ 16.9565 mol Step 3: Calculate the total heat energy released. Given that 1 mole of ethanol releases 1370 kJ of heat energy. Heat energy released = Moles of ethanol × Heat released per mole Heat energy released = 16.9565 mol × 1370 kJ/mol Heat energy released ≈ 23230.355 kJ Rounding to three significant figures: Heat energy released ≈ 23200 kJ Send me the next one 📸