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A 0.130-g sample of an unknown metal (X) reacted with hydrochloric acid according to the following chemical equation: 2 X (s) + 6 HCI (ag) 2 XCI3 (ag) + 3 H2 (g) The volume of hydrogen gas collected over water was 92.0 mL at 20 °C and 763 mm Hg. Referring to Example Exercise 2, 1. Calculate partial pressure of H2 gas = 2. Calculate moles of H2 gas using Ideal gas law 3. Calculate moles of metal using balanced equation

A 0.130-g sample of an unknown metal (X) reacted with hydrochloric acid according to the following chemical equation: 2 X (s) + 6 HCI (ag) 2 XCI3 (ag) + 3 H2 (g) The volume of hydrogen gas collected over water was 92.0 mL at 20 °C and 763 mm Hg. Referring to Example Exercise 2, 1. Calculate partial pressure of H2 gas = 2. Calculate moles of H2 gas using Ideal gas law 3. Calculate moles of metal using balanced equation

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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A 0.130-g sample of an unknown metal (X) reacted with hydrochloric acid according to the following chemical equation: 2 X (s) + 6 HCI (ag) 2 XCI3 (ag) + 3 H2 (g) The volume of hydrogen gas collected over water was 92.0 mL at 20 °C and 763 mm Hg. Referring to Example Exercise 2, 1. Calculate partial pressure of H2 gas = 2. Calculate moles of H2 gas using Ideal gas law 3. Calculate moles of metal using balanced equation_ 4. Calculated atomic mass of the unknown metal (atomic mass = mass/mol) 5. Identiy the symbol of the metal from the periodic table
Transcribed Image Text:A 0.130-g sample of an unknown metal (X) reacted with hydrochloric acid according to the following chemical equation: 2 X (s) + 6 HCI (ag) 2 XCI3 (ag) + 3 H2 (g) The volume of hydrogen gas collected over water was 92.0 mL at 20 °C and 763 mm Hg. Referring to Example Exercise 2, 1. Calculate partial pressure of H2 gas = 2. Calculate moles of H2 gas using Ideal gas law 3. Calculate moles of metal using balanced equation_ 4. Calculated atomic mass of the unknown metal (atomic mass = mass/mol) 5. Identiy the symbol of the metal from the periodic table
B. DETERMINING THE ATOMIC (MOLAR) MASS OF AN UNKNOWN METAE After determining the molar volume of hydrogen gas, we will determine the atomne for of an unknown metal (M) using a similar experimental method. The general equation te the reaction is: M (s) + 2 HCI(aq) → MCI2(aq) + H2(g) Equation 8 We will repeat the experiment as before and determine the volume of hydrogen Bar produced. According to the balanced equation above, we can use the stoichiometne relationship of 1 mole H2 to 1 mole unknown metal (M) to determine the moles of uhe unknown. Next, we will use the mole equation to determine the molar mass of the unknown and use the Periodic Table to identify the unknown metal by comparing the results to given molar masses. Molar mass = Equation 9 mol Example 2 - Atomic Mass of an Unknown Metal (M): An unknown metal (M), was reacted with excess hydrochloric acid, yielding hydrogen gas. Determine the identity of the unknown metal, given the following experimental data (make sure the equation is balanced): M(s) + 2 HCI(aq) → MCI2(aq) + H2(B) Mass of unknown metal 0.111 g Volume of gas produced: 43.6 mL 0.0436 L Temperature: 23.1°C = 296.3 K Atmospheric Pressure: 761.4 mm Hg Vapor Pressure of Water @ 23.1°C 21.20 mm Hg 1) Determine corrected pressure of gas sample: 761.4 torr - 21.2 torr = 740.2 torr 2) Convert mm Hg to atm: 740.2 mm Hg x (1 atm/760 mm Hg) = 0.9755 atm 3) Determine # moles of H2, using the Ideal Gas Law (P*V = n*R*T) (0.9755 atm) (0.0436 L) = n (0.08206 L atm/mol K) (296.3 K) (0.0425 atm L) = n (24.31 L atm/mol) n = 0.00175 mol H2 4) From balanced equation: moles H2 = moles of the unknown metal 0.00175 mol M, 5) Determine atomic mass of M - using Equation 9, divide the mass of unknown metal by the stoichiometric equivalent moles of unknown metal: Atomic mass of unknown metal = (0.111 g) / (0.00175 mol) = 63.4 g/mol 6) Identify the unknown metal - consulting a periodic table of the elements, you would be safe in concluding that the unknown metal is most likely copper (Cu). Copper's molar mass is 63.546 g/mol. If your calculated answer is slightly off from a given molar mass on the periodic table, you can assume the answer is the metal closest to your calculated answer. ASSESSMENTS 1. Pre-Lab Assignment 2. Lab Data Sheet 3. Post-Lab Assignment EO CLIPS Before completing the assessments, watch the videos covering the background, procedure, & calculations for this lab. • https://www.youtube.com/watch?v=FXgDuBidYNO IPMENT & MATERIALS NEEDED • Gas collection tube (Eudiometer) • Robber stopper w/tubing Ruler to measure Mg ribbon • Electronic balance
Transcribed Image Text:B. DETERMINING THE ATOMIC (MOLAR) MASS OF AN UNKNOWN METAE After determining the molar volume of hydrogen gas, we will determine the atomne for of an unknown metal (M) using a similar experimental method. The general equation te the reaction is: M (s) + 2 HCI(aq) → MCI2(aq) + H2(g) Equation 8 We will repeat the experiment as before and determine the volume of hydrogen Bar produced. According to the balanced equation above, we can use the stoichiometne relationship of 1 mole H2 to 1 mole unknown metal (M) to determine the moles of uhe unknown. Next, we will use the mole equation to determine the molar mass of the unknown and use the Periodic Table to identify the unknown metal by comparing the results to given molar masses. Molar mass = Equation 9 mol Example 2 - Atomic Mass of an Unknown Metal (M): An unknown metal (M), was reacted with excess hydrochloric acid, yielding hydrogen gas. Determine the identity of the unknown metal, given the following experimental data (make sure the equation is balanced): M(s) + 2 HCI(aq) → MCI2(aq) + H2(B) Mass of unknown metal 0.111 g Volume of gas produced: 43.6 mL 0.0436 L Temperature: 23.1°C = 296.3 K Atmospheric Pressure: 761.4 mm Hg Vapor Pressure of Water @ 23.1°C 21.20 mm Hg 1) Determine corrected pressure of gas sample: 761.4 torr - 21.2 torr = 740.2 torr 2) Convert mm Hg to atm: 740.2 mm Hg x (1 atm/760 mm Hg) = 0.9755 atm 3) Determine # moles of H2, using the Ideal Gas Law (P*V = n*R*T) (0.9755 atm) (0.0436 L) = n (0.08206 L atm/mol K) (296.3 K) (0.0425 atm L) = n (24.31 L atm/mol) n = 0.00175 mol H2 4) From balanced equation: moles H2 = moles of the unknown metal 0.00175 mol M, 5) Determine atomic mass of M - using Equation 9, divide the mass of unknown metal by the stoichiometric equivalent moles of unknown metal: Atomic mass of unknown metal = (0.111 g) / (0.00175 mol) = 63.4 g/mol 6) Identify the unknown metal - consulting a periodic table of the elements, you would be safe in concluding that the unknown metal is most likely copper (Cu). Copper's molar mass is 63.546 g/mol. If your calculated answer is slightly off from a given molar mass on the periodic table, you can assume the answer is the metal closest to your calculated answer. ASSESSMENTS 1. Pre-Lab Assignment 2. Lab Data Sheet 3. Post-Lab Assignment EO CLIPS Before completing the assessments, watch the videos covering the background, procedure, & calculations for this lab. • https://www.youtube.com/watch?v=FXgDuBidYNO IPMENT & MATERIALS NEEDED • Gas collection tube (Eudiometer) • Robber stopper w/tubing Ruler to measure Mg ribbon • Electronic balance
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