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2. A 0.158-g sample of unknown metal, X, reacted with hydrochloric acid according the following (balanced) reaction: 2 X (s) + 6 HCl(aq) → 2 XCl3 (aq) + 3 H₂ (g) The volume of hydrogen gas collected over water was 216 mL at 22 °C and a barometer reading of 764 mm Hg (VP of water at 22 °C is 20. mm Hg). SHOW ALL WORK. Find moles of (dry) hydrogen gas collected using PV=nRT, where R is 0.08206 L atm/mol K: Moles of hydrogen present 136 Determine moles of "X" that would have been present initially to produce those moles of hydrogen using the mole ratio in the balanced equation above: Moles of metal present Determine the molar mass of "X" knowing that molar mass is grams per mole.

2. A 0.158-g sample of unknown metal, X, reacted with hydrochloric acid according the following (balanced) reaction: 2 X (s) + 6 HCl(aq) → 2 XCl3 (aq) + 3 H₂ (g) The volume of hydrogen gas collected over water was 216 mL at 22 °C and a barometer reading of 764 mm Hg (VP of water at 22 °C is 20. mm Hg). SHOW ALL WORK. Find moles of (dry) hydrogen gas collected using PV=nRT, where R is 0.08206 L atm/mol K: Moles of hydrogen present 136 Determine moles of "X" that would have been present initially to produce those moles of hydrogen using the mole ratio in the balanced equation above: Moles of metal present Determine the molar mass of "X" knowing that molar mass is grams per mole.

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter5: Gases
Section: Chapter Questions
Problem 5.98PAE
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2. A 0.158-g sample of unknown metal, X, reacted with hydrochloric acid according the following (balanced) reaction: 2 X (s) + 6HCl(aq) → 2 XCl3 (aq) + 3 H₂ (g) The volume of hydrogen gas collected over water was 216 mL at 22 °C and a barometer reading of 764 mm Hg (VP of water at 22 °C is 20. mm Hg). SHOW ALL WORK. Find moles of (dry) hydrogen gas collected using PV=nRT, where R is 0.08206 L atm/mol K: Moles of hydrogen present Determine moles of "X" that would have been present initially to produce those moles of hydrogen using the mole ratio in the balanced equation above: Moles of metal present Determine the molar mass of "X" knowing that molar mass is grams per mole. 136 Atomic Mass of metal Identity of Unknown Metal
Transcribed Image Text:2. A 0.158-g sample of unknown metal, X, reacted with hydrochloric acid according the following (balanced) reaction: 2 X (s) + 6HCl(aq) → 2 XCl3 (aq) + 3 H₂ (g) The volume of hydrogen gas collected over water was 216 mL at 22 °C and a barometer reading of 764 mm Hg (VP of water at 22 °C is 20. mm Hg). SHOW ALL WORK. Find moles of (dry) hydrogen gas collected using PV=nRT, where R is 0.08206 L atm/mol K: Moles of hydrogen present Determine moles of "X" that would have been present initially to produce those moles of hydrogen using the mole ratio in the balanced equation above: Moles of metal present Determine the molar mass of "X" knowing that molar mass is grams per mole. 136 Atomic Mass of metal Identity of Unknown Metal
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