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 w.carbonate used for runs 1 and 2, calculate ..e theoretical yield of solid productsactual yieldPercent yield =x 100\theoretical yield|Reaction ANaHCO3(s)NaOH(s) +CO2(g)Run 1: Initial grams of NaHCO3NaCOTheoretical yield (grams) of NaOH:Percent yield (Run 1) = DATARecord all masses to the maximum number ofRun 1Run 2sig figs200°C400°C1.Mass of beaker81.6 6127,9862.Mass of beaker + NaHCO395.4573.Initial mass of NaHCO3니. 니704.292.4. Mass of beaker plus products afterheating.8438030,7425. Mass of product (actual yield)

Run 1Mass of products = 84.380 - 81.661 = 2.719 gRun 2Mass of products = 32.267 - 30.742 = 1.525 g…

Answered: Percent yield = the Reaction A…

Science

Chemistry

Percent yield = the Reaction A NaHCO3(s) -> _NaOH(s) + CO2(g) Run 1: Initial grams of NaHCO3 %3D

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...

See similar textbooks

Similar questions

Percent yield. 4Fe + 3O2 ---> 2Fe2 O3 Starting with 320g of oxygen gas you produce 75g of Iron(iii) oxide. What is the percent yield?
#25y of a 23% by mass magnesium chloride (MW= 95.21 g/mole) solution is reacted with 125.0 mL da125M solution of silver nitrate (MW= 169.87g/mole) determine the mass of silver chloride (MW = 143.32 p/mole) produced
Balance the following reaction. Enter a number in each blank. You must answer numerically, eg "1" not "one". FeBr3 + H2SO4 > Fe2(SO4)3 + HBr
Assuming you started with 3.23 g of sodium bicarbonate and your actual yield of solid product is 1.20g, which reaction is more likely to be the correct one?
1. KMnO,/NaOH/H₂O (x) 2. H₂O* IV OH
In a particular experiment 0.0039 moles of AgNO3 is added to 0.001875 NH4Cl and 0.156g of AgCl are recovered. What is the percent yield? AgNO3(aq) + NH4Cl(aq) --> AgCl(s) + NH4NO3(aq)
An unknown hydrated compound (AC·XH2O) contains 35.9% H2O. The molar mass of the anhydrous compound (AC) is 159.61 g/mol. Find the water of crystallization in this unknown hydrate. Part B is to find the number of moles of anhydrous compound (AC).
What is the mass percent of ethanol (CH3CH₂OH) if 0.0750 moles of ethanol is added to 0.350 kg of water?
what are the products?
2AI(s) +6HCl(aq)----->2AIcl3 (aq) + 3H2 (g) If a sample of 4.0 mole of AI is added to a solution containing 5.0 moles of HCl, How many moles of AICl3 are formed?
Given that 4 NH3 + 5 O2 → 4 NO + 6 H2O,when 4.50 mol of H2O are formed, the amountof NO formed isA) 3.00 mol B) 6.75 molC) 1.50 mol D) 4.50 mol
How many moles of NO, would be required to produce 2.75 moles of HNO, in the presence of excess water in the following chemical reaction? 3 NO,(g) + H,O (1) → 2 HNO,(g) + NO(g) MacBook Pro sc 80 888 #3 %2$ & 1 2 3 4 7 8. Q W E T Y A S D F G H J X C V B N M