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.
ScanSolve AI Answer
Step 1: Calculate the moles of zinc (Zn). The molar mass of zinc (Zn) is 65.4 g/mol. Moles of Zn = Mass of ZnMolar mass of Zn Moles of Zn = 1.96 g65.4 g/mol Moles of Zn ≈ 0.02997 mol Step 2: Calculate the moles of hydrochloric acid (HCl). The volume of HCl is 100 cm^3, which is 0.100 L. The concentration is 0.2 M. Moles of HCl = Concentration × Volume (in L) Moles of HCl = 0.2 mol/L × 0.100 L Moles of HCl = 0.020 mol Step 3: Determine the limiting reagent using the stoichiometric ratio. The balanced chemical equation is: Zn(s) + 2HCl(aq) → ZnCl_2(aq) + H_2(g) From the equation, 1 mole of Zn reacts with 2 moles of HCl. Let's determine how much HCl is needed to react with the available Zn: Moles of HCl needed = Moles of Zn × 2 mol HCl1 mol Zn Moles of HCl needed = 0.02997 mol Zn × 2 Moles of HCl needed ≈ 0.05994 mol HCl We have 0.020 mol of HCl, which is less than the 0.05994 mol needed. Therefore, HCl is the limiting reagent, and Zn is in excess. Alternatively, let's determine how much Zn is needed to react with the available HCl: Moles of Zn needed = Moles of HCl × 1 mol Zn2 mol HCl Moles of Zn needed = 0.020 mol HCl × (1)/(2) Moles of Zn needed = 0.010 mol Zn We have 0.02997 mol of Zn, which is more than the 0.010 mol needed. Therefore, Zn is in excess. The reagent that was in excess is Zinc. That's 2 down. 3 left today — send the next one.