Yield Step 1 :4.9668 g of Na2S03 was dissolved in 30ml distilled water by heating.Step 2 : Then 6.0895g of CuCl,. H,0 was dissolved in 20ml distilled water by stirring with a glassrod. The colour observed here was a deep blue/greenStep 3 : The solution from step 1 was added to step 2 solution. Colour turned Light green.Step 4 : 20ml 0.001M H2SO4 was then added to the solution in Step 3Step 5 : The solution was then funnelled using a buchner funnel, then washed three times withH,SO4 and washed three times with ethanol.The end product was solid white crystals, which weighed 2.4972 grams.What is the yield of the end product? Show all calculations

The objective of this question is to calculate the thereotical yield. The theoretical yield of a…

Step 1 :4.9668 g of Na₂SO3 was dissolved in 30ml distilled water by heating. Step 2: Then 6.0895g of CuCl2. H₂O was dissolved in 20ml distilled water by stirring with a glass rod. The colour observed here was a deep blue/green Step 3: The solution from step 1 was added to step 2 solution. Colour turned Light green. Step 4: 20ml 0.001M H₂SO4 was then added to the solution in Step 3 Step 5: The solution was then funnelled using a buchner funnel, then washed three times with H₂SO4 and washed three times with ethanol. The end product was solid white crystals, which weighed 2.4972 grams.

Step 1 :4.9668 g of Na₂SO3 was dissolved in 30ml distilled water by heating. Step 2: Then 6.0895g of CuCl2. H₂O was dissolved in 20ml distilled water by stirring with a glass rod. The colour observed here was a deep blue/green Step 3: The solution from step 1 was added to step 2 solution. Colour turned Light green. Step 4: 20ml 0.001M H₂SO4 was then added to the solution in Step 3 Step 5: The solution was then funnelled using a buchner funnel, then washed three times with H₂SO4 and washed three times with ethanol. The end product was solid white crystals, which weighed 2.4972 grams.

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

I know im missing other info but including just my mass of my product what else do i need to solve for percent yeild . please show work how to solve it an any other fake numbers so i can learn
Resources Lx Give Up? N но What is the chemical formula for the limiting reactant in the reaction shown? chemical formula: Write the balanced chemical equation for the reaction, using lowest whole-number coefficients chemical equation:
If 525.0 g of glucose yields 113.8 mL of ethanol, what is the percent yield for the reaction? %
If 20.0 grams of Potassium hydroxide reacts with 15.0 grams of Ammonium sulfate in a double replacement reaction. The products are Ammonia, NH3, Water, and Potassium sulfate(a) Determine the Limiting Reactant and then calculate the: (b) moles of Potassium sulfate produced(c)grams of Ammonia, NH3 produced
Why is it important to identify the limiting reactant? [Select all that apply] -The limiting reactant will be entirely used up in the reaction as it forms products. -The theoretical yield is the maximum amount of product that can be produced when all of the limiting reacting is converted into product. -In order to correctly calculate the percent yield, you need to know the actual yield and the theoretical yield, which depends on the limiting reactant. -If you don't determine the correct limiting reactant, it is possible to end up with percent yields that are too high or too low. -It doesn't matter which reactant is the limiting reactant, as long as I carefully follow the instructions in the lab procedure. or -The limiting reactant will always be the first reactant listed in a chemical reaction.
First, If 100.0 g of iron (III) oxide reacts with 40.00 g of aluminum to form aluminum oxide and iron, how many grams of aluminum oxide is made, and how much reactant remains? Next, How do you recognize a limiting reaction problem?
Which of the following conversioon proesses DOES NOT depend on the molar mass of a substance?
Calculate percent yield. Show your work pleasee 1. Theoretical 78.43 g Actual: 66.4 g
Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: a) Write the balanced reaction? b) What mass in grams of aluminum oxide that can be produced from 2.5 g of aluminum and 2.5 g of oxygen? c) Which one is limiting regeant? d) Which one is the excees reagent? e) How many moles of excess reagent were left over? f) What mass was experimentally measured if the percent yield was 75%?
Consider the unbalanced reaction NiS2(s) + O₂(g) --> NiO(s) + SO₂(g) When 11.2 g of NiS₂ react with 5.43 g of O₂, 4.86 g of NiO are obtained. The theoretical yield of NiO is (number and unit) A A/ 신 هم the limiting reactant is (name or symbol) and the percent yield is (number) %. (Remember to use correct sig figs)
If the theoretical yield substance is 13.65g and 11.33 g were recovered in an experiment what is the percent yield
the theoretical yield of water