Question

BG20.2 Determination of the Ideal Gas Law Constant Page 9 of 12 PRELAB QUESTIONS (Show all calculations.) I. Write a balanced chemical equation for the reaction of magnesium with hydrochloric acid. 2. A class ran this lab as described above. One student cut a piece of magnesium ribbon and found that it weighed 0.0347 g. The magnesium reacted with the 4.0 mL of concentrated hydrochloric acid. The concentration of concentrated hydrochloric acid is 12 mol/liter. Which reactant is the limiting reactant, the magnesium or the hydrochloric acid? a. b. How many moles of hydrogen gas will this piece of magnesium produce when reacted with 4 mLof 12 M hydrochloric acid? c. How many mL of hydrogen gas at STP would you expect to be produced by the reaction in b.? d. What gases were present in the eudiometer tube above the water after the reaction was complete' The barometric pressure was measured as 752 mm of Hg and the column of water in the eudiome tube was 34 mm tall. What was the pressure of the gas mixture in mm of Hg? e. f. The temperature of the solution in the 800 mL beaker was 24°C. What was the pressure hydrogen gas in the eudiometer tube in mm of Hg?

Answer 1

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1 Reaction of magnesium with Acid : hydrochloric ( Mg + 2HCL ngal2 + H2 d) (a) moles of mg - Given may = 0.0347 = 0.00144 moles. more o f Molar man 24 moles of HCl = Molarity & Volume = 12 * 4 = 0.048 mole V 1000 1000 Molar Ratio: ing: nu 1:2 0.00144: 0.00288 (HU) ùs in exces, limitory meagent = ng. (3) I mole of my produces 1 mole of H2. 0.00144 more of ing will produce 0.00144 mole of H2. = 0.00144 mole. (c) At STP PV = nRT 1XV= 0.00144 X 0.0821 x 298 V= 0.0352mL