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) Give a balanced equation for the reaction. The reaction is a neutralization between sulphuric acid (H_2SO_4) and a base XOH. Sulphuric acid is a diprotic acid, and XOH is a monobasic base. H_2SO_4(aq) + 2XOH(s) X_2SO_4(aq) + 2H_2O(l) b) Calculate the relative atomic mass of X. Step 1: Calculate the moles of sulphuric acid (H_2SO_4). Moles of H_2SO_4 = Concentration × Volume Moles of H_2SO_4 = 1mol/dm^3 × (25)/(1000)dm^3 = 1mol/dm^3 × 0.025dm^3 = 0.025mol Step 2: Use the stoichiometry from the balanced equation to find the moles of XOH. From the equation, 1mol of H_2SO_4 reacts with 2mol of XOH. Moles of XOH = 2 × Moles of H_2SO_4 = 2 × 0.025mol = 0.05mol Step 3: Calculate the molar mass of XOH. Molar mass of XOH = Mass of XOHMoles of XOH Molar mass of XOH = 2.8g0.05mol = 56g/mol Step 4: Calculate the relative atomic mass of X. The molar mass of XOH is the sum of the relative atomic masses of X, O, and H. Molar mass of XOH = Ar(X) + Ar(O) + Ar(H) 56 = Ar(X) + 16 + 1 56 = Ar(X) + 17 Ar(X) = 56 - 17 = 39 The relative atomic mass of X is 39. That's 2 down. 3 left today — send the next one.