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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Hey precious — ready when you are. Here are the solutions to your homework questions: 5. a) (i) The gas obtained is acetylene*, and its formula is C_2H_2. (ii) The balanced chemical equation is: CaC_2(s) + 2H_2O(l) → Ca(OH)_2(aq) + C_2H_2(g) (iii) Calculate the mass of slaked lime obtained from 2.5g of calcium carbide. Step 1: Calculate the molar mass of CaC_2 and Ca(OH)_2. Molar mass of CaC_2 = 40 + (2 × 12) = 64 g/mol. Molar mass of Ca(OH)_2 = 40 + (2 × 16) + (2 × 1) = 74 g/mol. Step 2: Calculate the moles of CaC_2 used. Moles of CaC_2 = 2.5 g64 g/mol = 0.0390625 mol Step 3: From the balanced equation, 1 mole of CaC_2 produces 1 mole of Ca(OH)_2. So, moles of Ca(OH)_2 produced = 0.0390625 mol. Step 4: Calculate the mass of Ca(OH)_2. Mass of Ca(OH)_2 = 0.0390625 mol × 74 g/mol = 2.890625 g The mass of slaked lime obtained is 2.89 g. b) (i) The number of Faradays used in this experiment. Step 1: Calculate the total charge passed. Q = I × t = 2 A × (15 × 60) s = 2 A × 900 s = 1800 C Step 2: Calculate the number of Faradays. (Using Faraday's constant F = 96485 C/mol) Number of Faradays = (Q)/(F) = 1800 C96485