Need help answering all with given data Experiment 5: Generating Hydrogen Gasm:7609Part B: Molar mass of unknown metalMass of unknown metal (X):Volume of H₂ gasTemperature of H₂ gasAtmospheric pressure (see barometer)Vapor pressure of waterPartial pressure of H₂ gas746.5mmHg- /6.5mmHg = 730 mmHgUsing PV=nRT and your data, calculate the moles of hydrogen gas produced in theexperiment:(0.96atm)(0.0194)V=19.0mLlatmmolk;)(292K)2:52 158P=746.5mmHgT: 292K273+19.0=292°TEPTO 0:Unknown #:201310.0g0.3019x0.000769x0.130719.019.0746.5 mmHg16.5 mmHg 0.0217730.0 mmHg 0.961mL°℃0.019292moles H₂:drenaje19.0m₂ xIL2 1000ML0.019L1000mLConvert moles of hydrogen gas to moles of the metal (X), using the balanced equation.X (s) + 2 HCl (aq) → XCl₂2 (aq) + H₂ (g)0.000/m1 maix= 0.0000 101%(XSPS)IMOLKCalculate the molar mass of the metal (g/mol) and identify the metal.3079x75gin61atmlatm: 760mmHgL0.00076molXmoles X:KR=0.0821 LCmMetal:0.00076Molar mass: 171.97

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Experiment 5: Generating Hydrogen Gas Part B: Molar mass of unknown metal Mass of unknown metal (X): Volume of H₂ gas Temperature of H₂ gas Atmospheric pressure (see barometer) Vapor pressure of water Partial pressure of H₂ gas 746.5mmHg-/6.5mmHg = 730 mmHg Using PV=nRT and your data, calculate the moles of hydrogen gas produced in the experiment: (0.96atm)(0.019L) V=19.0mL latm molk ;)(292K) 35-2 158 P=746.5mmHg T: 292K 273+19.0=292° Unknown #: TEPYO 0: 2017CA10.0 0.1307 19.0 19.0 g mL °℃ 0.019 292 746.5 mmHg 16.5 mmHg 0.0217 730.0 mmHg 0.961 moles H₂: atm latm: 760mmHg 07anaje 19.0m₂ x IL 2 1000ML 0.019L 1000mL Convert moles of hydrogen gas to moles of the metal (X), using the balanced equation. X (s) + 2 HCl (aq) → XCl₂2 (aq) + H₂ (g) 0.000/6₂1 marx = 0.0000 lot% (XSPS) IMOLK Calculate the molar mass of the metal (g/mol) and identify the metal. 0.3079x1759 ginal 0.000769x L 0.00076 mol X moles X: K R=0.0821 LC m Metal: 0.00076 Molar mass: 171.97

Experiment 5: Generating Hydrogen Gas Part B: Molar mass of unknown metal Mass of unknown metal (X): Volume of H₂ gas Temperature of H₂ gas Atmospheric pressure (see barometer) Vapor pressure of water Partial pressure of H₂ gas 746.5mmHg-/6.5mmHg = 730 mmHg Using PV=nRT and your data, calculate the moles of hydrogen gas produced in the experiment: (0.96atm)(0.019L) V=19.0mL latm molk ;)(292K) 35-2 158 P=746.5mmHg T: 292K 273+19.0=292° Unknown #: TEPYO 0: 2017CA10.0 0.1307 19.0 19.0 g mL °℃ 0.019 292 746.5 mmHg 16.5 mmHg 0.0217 730.0 mmHg 0.961 moles H₂: atm latm: 760mmHg 07anaje 19.0m₂ x IL 2 1000ML 0.019L 1000mL Convert moles of hydrogen gas to moles of the metal (X), using the balanced equation. X (s) + 2 HCl (aq) → XCl₂2 (aq) + H₂ (g) 0.000/6₂1 marx = 0.0000 lot% (XSPS) IMOLK Calculate the molar mass of the metal (g/mol) and identify the metal. 0.3079x1759 ginal 0.000769x L 0.00076 mol X moles X: K R=0.0821 LC m Metal: 0.00076 Molar mass: 171.97

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter10: Solids, Liquids, And Phase Transitions

Section: Chapter Questions

Problem 35P

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