1 Old MathJax webviewAn unknown metal was reacted with HCl(ag). It was determined that this reaction evolved hydrogen gas (H2(g)) and left themetal in solution in the 2+ oxidation state. The unknown metal was then subjected to the same test as magnesium in the"Molar Mass of Magnesium" lab. After some adjustments to get the volume of gas collected in the right range, the followingdata and results were obtained:Mass of unknown metal used = 0.1315 gP(atmospheric) = 753.2 mmHgTemperature of gas = 22.8 °CVolume of gas collected = 61.2 mLDifference in height of solution levels in the buret and beaker = 146.2 mmVapour pressure of H2O at gas temperature = 20.749 mmHgConstants:(R = 62,3637 LmmHg/mol-KK = °C + 273.15dsolution = 1.00 g/mL; dHg = 13.6 g/mL)Given the data above, answer the following questions. Your answers should be given to the correct number of significantfigures at each step, but keep the unrounded numbers for use in further calculations. (For a value like 34.2173 (4 SFs), enter34.22, but use 34.2173 in further calculations.)When you are reviewing your answer, you may be able to get some hints for your next attempt by hovering your mouse overthe answer box.(a) What is the hydrostatic pressure in mmHg?34.54x mmHg(b) What is the total pressure of all gases in the buret?56.67* mmHg(c) What is the partial pressure of the H2 gas in the buret?25.78* mmHg(d) What is the number of moles of H2 gas in the buret?78.76x mol(e) What is the number of moles of metal used in the experiment?69.87x mol(f) What is the calculated molar mass of the metal according to this data?23.76x g/molprovide the correct solutionI tried solving the question and got theseanswers incorrect. could anyone please providethe correct answers for these questions

An unknown metal was reacted with HCl(ag). It was determined that this reaction evolved hydrogen gas (H2(g)) and left the metal in solution in the 2+ oxidation state. The unknown metal was then subjected to the same test as magnesium in the "Molar Mass of Magnesium" lab. After some adjustments to get the volume of gas collected in the right range, the following data and results were obtained: Mass of unknown metal used = 0.1315 g P(atmospheric) = 753.2 mmHg Temperature of gas = 22.8 °C Volume of gas collected = 61.2 mL %3D Difference in height of solution levels in the buret and beaker 146.2 mm Vapour pressure of H2O at gas temperature = 20.749 mmHg Constants: (R = 62.3637 L-mmHg/mol-K %3D K = °C + 273.15 dsolution = 1.00 g/mL; dHg = 13.6 g/mL)

An unknown metal was reacted with HCl(ag). It was determined that this reaction evolved hydrogen gas (H2(g)) and left the metal in solution in the 2+ oxidation state. The unknown metal was then subjected to the same test as magnesium in the "Molar Mass of Magnesium" lab. After some adjustments to get the volume of gas collected in the right range, the following data and results were obtained: Mass of unknown metal used = 0.1315 g P(atmospheric) = 753.2 mmHg Temperature of gas = 22.8 °C Volume of gas collected = 61.2 mL %3D Difference in height of solution levels in the buret and beaker 146.2 mm Vapour pressure of H2O at gas temperature = 20.749 mmHg Constants: (R = 62.3637 L-mmHg/mol-K %3D K = °C + 273.15 dsolution = 1.00 g/mL; dHg = 13.6 g/mL)

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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Question

Old MathJax webview
An unknown metal was reacted with HCl(ag). It was determined that this reaction evolved hydrogen gas (H2(g)) and left the
metal in solution in the 2+ oxidation state. The unknown metal was then subjected to the same test as magnesium in the
"Molar Mass of Magnesium" lab. After some adjustments to get the volume of gas collected in the right range, the following
data and results were obtained:
Mass of unknown metal used = 0.1315 g
P(atmospheric) = 753.2 mmHg
Temperature of gas = 22.8 °C
Volume of gas collected = 61.2 mL
Difference in height of solution levels in the buret and beaker = 146.2 mm
Vapour pressure of H2O at gas temperature = 20.749 mmHg
Constants:
(R = 62,3637 LmmHg/mol-K
K = °C + 273.15
dsolution = 1.00 g/mL; dHg = 13.6 g/mL)
Given the data above, answer the following questions. Your answers should be given to the correct number of significant
figures at each step, but keep the unrounded numbers for use in further calculations. (For a value like 34.2173 (4 SFs), enter
34.22, but use 34.2173 in further calculations.)
When you are reviewing your answer, you may be able to get some hints for your next attempt by hovering your mouse over
the answer box.
(a) What is the hydrostatic pressure in mmHg?
34.54
x mmHg
(b) What is the total pressure of all gases in the buret?
56.67
* mmHg
(c) What is the partial pressure of the H2 gas in the buret?
25.78
* mmHg
(d) What is the number of moles of H2 gas in the buret?
78.76
x mol
(e) What is the number of moles of metal used in the experiment?
69.87
x mol
(f) What is the calculated molar mass of the metal according to this data?
23.76
x g/mol
provide the correct solution
I tried solving the question and got these
answers incorrect. could anyone please provide
the correct answers for these questions

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