Report QuestionsThese questions are to be answered on notebook paper and included withthis lab handout as your experiment report. Be sure to show complete setups forall problem solving. Also, use units and follow all rules of significant figures inyour calculations.To determine the mass of carbon dioxide (CO2) produced in your trials, you willneed a density value for CO2. Gas densities vary somewhat with temperature andpressure so I will provide you with a formula that you can use to determine thisquantity at your experimental conditions.Density of CO2 = k (Patm- Pwater) / TWhere: k 0.706 g K/L torrPatmPwater%3Dthe atmospheric press in torrthe vapor pressure of water at your experimental temperature%3DT= the temperature of the water in KelvinFor your convenience, a brief table of water vapor pressures is included here. Amore complete table is found in the appendices at the end of your text.Temp (°C)18Pwater (torr)15.5Temp (°C)24Pwater (torr)22.41916.52523.82017.52625.22118.72726.72219.82828.32321.12930.0Determine the density of CO2 gas at your experimental conditions.For each of the trials I-IV in Part I of the experiment, determine which reactantwas limiting and determine the theoretical mass of CO2 which could have beenproduced in each of these trials.From the volumes of CO2 produced in trials I-IV of Part I, and your answer toquestion 1, find the mass of CO2 actually produced in each of these trials and find a% yield for each trial.Determine the average % yield for your 4 trials. Data TablePart I: Determination of % YieldTrialMass of NazCO3 usedVolume ofVolume of CO2 produced6.00 M HC174 ml182ml1.089usedI5.00 mL1.292 gII5.00 mL1.420 g225mlII5.00 mL1.668g310 mlIV5.00 mL24°CTemperature of water:729 torrAtmospheric Pressure:Part II: Determination of the Formula Weight of an Unknown Metal Carbonate2.Unknown #Volume ofVolume of CO2 producedMass of UnknownCarbonate usedTrial6.00 M HCIUsed180ml188ml1.00 g5.00 mLII1.00 g5.00 mL

Temperature of water = 24oC = 24 + 273.15 K = 297.15 K Atmospheric pressure, Patm= 729 torr Vapour…

For each of the trials I-IV in Part I of the experiment, determine which reactant was limiting and determine the theoretical mass of CO2 which could have been produced in each of these trials. From the volumes of CO2 produced in trials I-IV of Part I, and your answer to question 1, find the mass of CO2 actually produced in each of these trials and find a % yield for each trial. Determine the average % yield for your 4 trials.

For each of the trials I-IV in Part I of the experiment, determine which reactant was limiting and determine the theoretical mass of CO2 which could have been produced in each of these trials. From the volumes of CO2 produced in trials I-IV of Part I, and your answer to question 1, find the mass of CO2 actually produced in each of these trials and find a % yield for each trial. Determine the average % yield for your 4 trials.

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

Section: Chapter Questions

Problem 10CR

See similar textbooks

Similar questions

A commercial mercury vapor analyzer can detect in air, concentrations of gaseous Hg atoms (which are poisonous) as low as 2106 mg/L of air. At this concentration, what is the partial pressure of gaseous mercury if the atmospheric pressure is 733 tort at 26 C?
Silver ions can be found in some of the city water piped into homes. The average concentration of silver ions in city water is 0.028 ppm. (a) How many milligrams of silver ions would you ingest daily if you drank eight glasses (eight oz/glass) of city water daily? (b) How many liters of city water are required to recover 1.00 g of silver chemically?
Solutions of hydrogen in palladium may be formed by exposing Pd metal to H2 gas. The concentration of hydrogen in the palladium depends on the pressure of H2 gas applied, but in a more complex fashion than can be described by Henry's law. Under certain conditions, 0.94 g of hydrogen gas is dissolved in 215 g of palladium metal (solution density = 10.8 g cm3). (a) Determine the molarity of this solution. (b) Determine the molality of this solution. (c) Determine the percent by mass of hydrogen atoms in this solution.
The mercury content of a stream was believed to be above the minimum considered safe —1 part per billion (ppb) by weight. An analysis indicated that the concentration was 0.68 parts per billion. What quantity of mercury in grams was present in 15.0 L of the water, the density of which is 0.998 g/ml? ( 1ppbHg=1ngHg1gwater)
Question. Determination of percent water (%H₂O) in hydrated FeSO4nH₂O is demonstrated in General Chemistry Laboratory (I), Chem. 105. The following table contains the results collected from the students groups. 1 2 3 4 5 6 (a) Calculate the average number of water molecules (b) %H₂O in each sample. 3.38 3.47 3.35 3.40 3.44 3.41 1.4 1.35 1.35 1.44 1.49 1.39 Mass of water (g) Moles of water Moles FeSO4 11= Moles H₂O Mole FeSO Average n % water in hydrated salt (wt/wt) Hint: Atomic mass: Fe = 56 g/mol; O = 16 g/mol; H = 1.0 g/mol; S = 32 g/mol.
Calculate te mass proont of NaS04 inasdution containing of Naz sO4 in vwate, where in He water has a volme 20g 3.
and Employees CH STATE GE 90 ENDULERSE IS FOREVER "ON-Tame Name Jodi Rayal Molarity = wt. x1000 3. Calculate the massof Potassium hydrogen phthalate (KHP) to prepare a 250.0 mL solution of 0.1000 M KHP solution. Mol ut. x Voluse the 2500×1000 204.22250 mass Initial Buret Reading Final Buret Reading Vol NaOH Added Moles of NaOH Moles of HCI Volume of unknown HCI solution Concentration of HCI Average concentration of HCI of KHP = 5.11g 4. Complete the table below for the following neutralization reaction of an unknown concentration of hydrochloric acid with 0.100 M sodium hydroxide: Mu spate solution Trial 1 0 11.15 го data and calculate the concentration 15 Trial 2 11.15 22.15 Trial 3 22.15 33.25 abyh 067 LANDINUKASHU TROWTHCENTISSATE ARAD Ma That par މއކނި REMURNAR MISAMARALISERDRY Tile
command option MOD Science 7 nt lonsns to smulov yd dne ai sw.E 179Gw 16 evbim 2ib bovloeelb lonshje lo aisii de A TASK TASK 1: Concentration of solutions that involves liguid solute and solvent uses with an equation: ni lodo Volume of % volume = Volume of biowaao1S phnswens yd wolsd 2nsmstsia srli edslgmoɔ:ar Noodeton yivlos 9onsiba Tuay rio 21swens 10oy ihV TASK 2: Directions: Choose the letter of the best answer. of a colution?
Expeniment and name Chemical formula Cobalt (11) nitzate Co(NOs)2 Buldatance Aane and dhemical farmula mm, q/mo! 182.95g lmol Fruihal volume , L Iniial concentrahion measure d, mal/L Number of mole's and massof mass Of solute 500ML 0.876 mollL 0 -438 mol Colw0z to Concentration after eventahom affer evapo 1.461 mal L Can you please explatn to calculate how the 180.19) cduo wsas arrived at ? Thanks ass
70 alll ll ? ..::0E is اجابة قصيرة A solution of Al2 (S04) 3 at a concentration of 0.3 N , What is the volume needed to prepare a solution at a concentration of 0.04 M in a volume of 150 ml of distilled water إجابتك كتب إجابتك. . is
The indicator of Moher regent is. O KCro4. O KMN04.
Most commercial samples of K MnO contain some manganese dioxide that must be femoved prie Submit Request Answer Part B Why is the K MnO4 not stored in a rubber-stoppered bottle? Rubber doesn't make a good seal with the plastic bottles in which permanganate is usually stored. Rubber can oxidize the permanganate solution. O Rubber is made of inorganic matter and will reduce the permanganate solution. Rubber is made of organic matter and will reduce the permanganate solution. Submit Request Answer Provide Feedback P Pearson Copyright © 2020 Pearson Education Inc. All rights reserved. I Termns of Use I 40 DELL