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 pressure of water at 24oC = 22.4 torr (from the appendices given) k = 0.706 g K/ L torrUsing the formula given: Density = k (Patm-Pwater)TDensity = 0.706 g K L-1 torr-1 (729 - 22.4 )torr297.15 KDensity =1.68 g L-1 Reaction involved: Na2CO3 + 2HCl →2NaCl + CO2 + H2O Trial 1: Mass of Na2CO3 used = 1.084 g Molar mass of Na2CO3 = 106 g/mol ∴ Moles of Na2CO3 = 1.084106 = 0.01 mol Molarity of HCl = 6 M Volume of HCl used = 5 mL = 0.005 L ∴ Moles of HCl = Molarity x volumeMoles of HCl = 6 M x 0.005 L = 0.03 mol From the balanced equation, we can see that 1 mole of Na2CO3 reacts with 2 moles of HCl So, 0.01 mol of Na2CO3 will react with 0.02 moles of HCl hence, HCl is in excess. ∴Na2CO3 is the limiting reagent. 1 mole of Na2CO3 produces 1 mole of CO2 0.01 mole Na2CO3 produces 0.01 mole of CO2 So, mass of CO2 produced = 0.01 mol x 44 g mol-1 = 0.44 g Mass of CO2 produced in Trial I = 0.44 g Moles of HCl are constant in all the trials i.e. 0.03 mol ∴ Moles of Na2CO3 = 1.292106 = 0.012 mol Na2CO3 is the limiting reagent. Mass of CO2 produced = 0.012 mol x 44 g mol-1 = 0.528 g Mass of CO2 produced in Trial II = 0.528 g ∴ Moles of Na2CO3 = 1.420106 = 0.0134 mol Na2CO3 is the limiting reagent. Mass of CO2 produced = 0.0134 mol x 44 g mol-1 = 0.5896 g Mass of CO2 produced in Trial III = 0.5896 g ∴ Moles of Na2CO3 = 1.668106 = 0.0157 mol So, mass of CO2 produced = 0.0157 mol x 44 g mol-1 = 0.6908 g Mass of CO2 produced in Trial IV = 0.6908 g Density = 1.68 g L-1 = 1.68 x 10-3 g/mL Formulas used: Mass = density x volume percent yield = theoretical mass of CO2experimental mass of CO2 X 100 Trials Volume of CO2 produced (mL) Mass of CO2 (experimental) g Mass of CO2 (theoretical) g Percent yield I 74 0.1243 0.44 28.25 II 182 0.3057 0.528 57.89 III 225 0.378 0.5896 64.11 IV 310 0.5208 0.6908 75.39 Average % yield = 28.25 + 57.89 + 64.11 + 75.394 = 56.41 %

Science

Chemistry

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.

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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Concept explainers

Stoichiometry

Stoichiometry is a chemical division that evaluates the quantitative content of the chemical process with the help of the reacting molecules or products taking part in the reaction. The term “stoicheion” in “Stoichiometry”, is an old Greek term for "element" whereas “metron” means "measure".

Question

Data Table
Part I: Determination of % Yield
Trial
Mass of NazCO3 used
Volume of
Volume of CO2 produced
6.00 M HC1
74 ml
182ml
1.089
used
I
5.00 mL
1.292 g
II
5.00 mL
1.420 g
225ml
II
5.00 mL
1.668g
310 ml
IV
5.00 mL
24°C
Temperature of water:
729 torr
Atmospheric Pressure:
Part II: Determination of the Formula Weight of an Unknown Metal Carbonate
2.
Unknown #
Volume of
Volume of CO2 produced
Mass of Unknown
Carbonate used
Trial
6.00 M HCI
Used
180ml
188ml
1.00 g
5.00 mL
II
1.00 g
5.00 mL

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