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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You're on a roll — Here are the answers to your questions: a) Write an equation for the combustion of methanol (CH_3OH). Step 1: Write the unbalanced equation for complete combustion, which produces carbon dioxide and water. CH_3OH(l) + O_2(g) → CO_2(g) + H_2O(l) Step 2: Balance the carbon atoms. (1 C on each side, already balanced). Step 3: Balance the hydrogen atoms. There are 4 H atoms on the left (3 from CH_3 and 1 from OH). So, place a coefficient of 2 in front of H_2O on the right. CH_3OH(l) + O_2(g) → CO_2(g) + 2H_2O(l) Step 4: Balance the oxygen atoms. There are 1 + 2x oxygen atoms on the left (1 from CH_3OH and 2x from O_2). There are 2 + (2 × 1) = 4 oxygen atoms on the right. 1 + 2x = 4 2x = 3 x = (3)/(2) Step 5: Substitute the coefficient for O_2 and multiply the entire equation by 2 to remove the fraction. 2CH_3OH(l) + 3O_2(g) → 2CO_2(g) + 4H_2O(l) The balanced equation is: 2CH_3OH(l) + 3O_2(g) → 2CO_2(g) + 4H_2O(l) b) Calculate: i) The number of moles of methanol used in this experiment. Step 1: Calculate the mass of methanol used. Mass of methanol used = Initial mass of lamp + methanol - Final mass of lamp + methanol Mass of methanol used = 22.98 g - 22.11 g = 0.87 g Step 2: Calculate the molar mass of methanol (CH_3OH). Molar mass of CH_3OH = (1 × C) + (4 × H) + (1 × O) Molar mass of CH_3OH = (1 × 12) + (4 × 1) + (1 × 16) = 12 + 4 + 16