DATARecord all masses to the maximum number ofRun 1Run 2sig figs200°C400°C1.Mass of beaker81.06127.9862.Mass of beaker + NaHCO385.45732.2673.Initial mass of NaHCO34.4764.292Mass of beaker plus products afterheating.4.84.3 8030.7425.Mass of product (actual yield)There are three theoretically possible chemical reactions that could occur during the thermal decomposition of bakingsoda.1)sodium bicarbonate (s) → sodium hydroxide (s) + carbon dioxide (g)2)sodium bicarbonate (s) → sodium oxide (s) + carbon dioxide (g) + water (g)3)sodium bicarbonate (s)→ sodium carbonate (s) + carbon dioxide (g) + water (g) 2)from each of the possible decomposition reactions, then calculate the percent yield by dividing your actual yield by thetheoretical yield you calculate for each reaction.Using the mass of sodium bicarbonate used for runs 1 and 2, calculate the theoretical yield of solid productsactual yieldPercent yield =x 100ltheoretical yield|Reaction ANaHCO3(s)->NaOH(s)_CO2(g)iteitRun 2: Initial grams of NaHCO3Theoretical yield (grams) of NaOH:Percent yield (Run 2) =

Answered: Image /qna-images/answer/ca495280-074f-4ac0-9a98-2179ce11ced6.jpg

2) from each of the possible decomposition reactions, then calculate the percent yield by dividing your actual yield by the theoretical yield you calculate for each reaction. Using the mass of sodium bicarbonate used for runs 1 and 2, calculate the theoretical yield of solid products actual yield Percent yield = Itheoretical yield 100 Reaction A NaHCO3(s) -> NaOH(s) Co2() Run 2: Initial grams of NaHCO3 %3D Theoretical yield (grams) of NaOH: Percent yield (Run 2) =

2) from each of the possible decomposition reactions, then calculate the percent yield by dividing your actual yield by the theoretical yield you calculate for each reaction. Using the mass of sodium bicarbonate used for runs 1 and 2, calculate the theoretical yield of solid products actual yield Percent yield = Itheoretical yield 100 Reaction A NaHCO3(s) -> NaOH(s) Co2() Run 2: Initial grams of NaHCO3 %3D Theoretical yield (grams) of NaOH: Percent yield (Run 2) =

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter8: Thermochemistry

Section: Chapter Questions

Problem 33QAP: A lead ore, galena, consisting mainly of lead(II) sulfide, is the principal source of lead. To...

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In the 1880s, Frederick Trouton noted that the enthalpy of vaporization of 1 mol pure liquid is approximately 88 times the boiling point, Tb, of the liquid on the Kelvin scale. This relationship is called Troutons rule and is represented by the thermochemical equation liquid gas H = 88 Tb, joules Combined with an empirical formula from chemical analysis, Troutons rule can be used to find the molecular formula of a compound, as illustrated here. A compound that contains only carbon and hydrogen is 85.6% C and 14.4% H. Its enthalpy of vaporization is 389 J/g, and it boils at a temperature of 322 K. (a) What is the empirical formula of this compound? (b) Use Troutons rule to calculate the approximate enthalpy or vaporization or one mole of the compound. Combine the enthalpy of vaporization per mole with that same quantity per gram to obtain an approximate molar mass of the compound. (c) Use the results of parts (a) and (b) to find the molecular formula of this compound. Remember that the molecular mass must be exactly a whole-number multiple of the empirical formula mass, so considerable rounding may be needed.
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