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

Given: Mass of unknown metal used = 0.1315 g P(atmospheric) = 753.2 mmHg Temperature of gas = 22.8…

Answered: An unknown metal was reacted with…

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter3: Statistical Tests With Excel

Section: Chapter Questions

Problem 5P

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Chemistry Hand written please. Please list four properties that describe a gas. Please give at least five gas laws mathematically in the gas chapter. What is the STP condition? What is the molar volume? Please give at least two specific examples for strong electrolytes, weak electrolytes and nonelectrolytes. Please give the detailed steps and final answer for the following question: A gas sample containing 12 g of CO2 has a volume of 14 L. What will the volume be if 12 g of He is added? __
In the preparation of 60 mL Magnesium citrate in the laboratory, you are required to:calculate for the volume of Carbon dioxide released from the hydrated double salt of Magnesium carbonate when reacted with Citric acid if 2.57 g of Magnesium carbonate is used. MW of Magnesium carbonate = 485.65 g/mol H3C6H5O7 = 192.12 g/mol Equations: (MgCO3)4 .Mg(OH)2 .5H2O + 5H3C6H5O7 → 5MgHC6H5O7 + 4CO2 + 11H2O3KHCO3 + H3C6H5O7 → K3C6H5O7 + 3CO2 + 3H2O Reacting ratio: 1mol (MgCO3)4 .Mg(OH)2 .5H2O = 4 mol CO2 1 mol of any gas at STP occupies a volume of 22.4 L or 22, 400 mL Choices: a 385.71 mL b 496.23 mL c 365.20 mL d 474.15 mL
BSA for concentration measurements is often prepared as a 10 mg/mL stock solution. Suppose you wish to prepare a series of 10 mL solutions of BSA at 1.0, 0.8, 0.6, 0.4, and 0.2 mg/mL. Using the dilution equation C1 × V1 = C2 × V2, you plan to do this by transferring a calculated volume (V1) of the 10 mg/mL (C1) into a clean test tube, then adding water in sufficient volume to produce 10 mL (V2) at the desired concentration (C2). Complete the table below, showing the volume of stock 10 mg/mL solution you need to add to each tube, and the volume of water you need to add to each. Also, convert the desired mg/mL concentration values to their equivalent in μM (micromolar; 10-6 M).
An unknown sample containing a mixture of NaCl and Na2CO3 was analyzed to determine the % composition of each compound. In the analysis for Na2CO3 (soda ash), the following data were obtained mass of unknown - 0.4436 g conc. of HCl used - 0.25 N initial volume - 0.5 mL final volume - 20.0 mL (MW soda ash) 106.12) 1.) What method was used to determine the concentration of HCl? 2.) What is the net volume of HCl used in the titration? 3.) What is % Na2CO3 in the given sample? NOTE: Round off your answer to a whole number (2 sig fig)
Report sheet analysis of KCIO3/KCI Unknown substance 1 Mass of empty 400mL beaker 164.93g, Mass of 30mL beaker+test tube 96.181g, Mass of 30mL beaker+test tube+unkown mixture 97.218g, Mass of unkown substance 1 1.037g, Mass of 400mL beaker and water 304.97g, Temperature of O2 20 celsius, Atmospheric pressure 750.1 torr. Mass of water ___, Volume of O2___, Vapor pressure of water ___torr, Partial pressure of O2 (Po2) ___torr, Partial pressure of O2 (Po2) ___atm, Moles of O2 (no2) ___, Moles of KCIO3 in unkown ___, Grams of KCIO3 in known ___, % by mass KCIO3 in unknown ___.
93.6g to ng and 93.6g to tons with the set up in the image possible show how to get the answer please
An unknown sample containing citric acid (C6H8O7) was analyzed using 0.2347N NaOH. The following data were obtained in one of the trials of the analysis: Mass of Unknown 0.4232 g Initial reading of NaOH 2.50 mL Final reading of NaOH 28.00 mL Write the balanced chemical equation involved. What is the net volume of NaOH reacted? What is the molar mass of citric acid? Calculate % citric acid in the sample.
A 19.51 ݃ sample of impure methylamine, which contains 72.58% (by mass) of CH3NH2 , isreacted with 30.81 ݃ of pure oxygen gas:4CHଷNHଶ(g) + 9Oଶ(g) ⟶ 4COଶ(g) + 10HଶO(ℓ) + 2Nଶ(g) In another experiment, this impure methylamine was used as follows: An unknown mass of the impure compound is dissolved in enough water to make 500.0 ݉ܮof solution. 20 ݉ܮ of this solution was transferred by pipette to a clean 250 mL volumetric flask andmade up to the mark. The molarity of the CH3NH2 in the final solution was determined to be 0.103 M.Determine the mass of CH3NH2 present in the original amount of impure compound used tomake this solution.
A reaction generates hydrogen gas, H2, as a product. The reactants are mixed and sealed in a 250-mL vessel. After 20.0 minutes, 3.91x10-2 mol H2 have been generated. Calculate the final concentration (in M) of H2 gas.
Chemistry A group of students was tasked with synthesizing dibenzalacetone (DBA) in the lab. They used acetone as limiting reagent, calculated their TY to be 8.0 g DBA, obtained 14.0 g crude product (wet) and their % Yield was 65%. What was the actual yield for their final product (recrystallized, dry DBA)? What was the minimum volume (ml) of ethanol they needed to recrystallize their wet crude? What was the amount of impurities (side products, moisture,...) contained in their wet crude?
Using the procedure above, please annswere the below question: a. In step 1 of the experiment, you sanded the magnesium strip before weighing (and reacting) to remove any magnesium oxide. If you skipped step 1 and left a MgO film on the strip, would the calculated molar volume of hydrogen gas collected be higher or lower than if the weighed mass were all magnesium metal? Explain which experimental data would be incorrect for the measured mass. b. The gas collected in the eudiometer was a mixture of hydrogen gas and water vapor. How is the calculated molar volume affected if the partial pressure of water vapor collected is not accounted for? Explain.
In the preparation of 60 mL Magnesium citrate in the laboratory, you are required to: calculate for the volume of Carbon dioxide released from the hydrated double salt of Magnesium carbonate when reacted with Citric acid if 2.57 g of Magnesium carbonate is used. MW of Magnesium carbonate = 485.65 g/mol H3C6H5O7 = 192.12 g/mol a 385.71 mL b 496.23 mL c 365.20 mL d 474.15 mL

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