Recycling Al experiment
Mass of Al : 0.49g
Mass of KAl(SO4)2 12H2O synthesized: 2.86g
1. Assuming you started with pure aluminium scrap, calculate the theoretical mass of the precipitate, alum. Include a balanced net ionic equation for the formation of the product from Al3+.
2. Calculate your percent yield.
3. If you had a large number amount of impurities in the scrap aluminium, what would be the impact in the percent yield calculation? explain.
4. In this experiment volume of 1.5M potassium hydroxide and 9M sulfuric acid were added, why was this information not precise?
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
Recycling Al experiment Mass of Al : 0.49g Mass of KAl(SO4)2 12H2O synthesized: 2.86g 1. Assuming...
Data Sheet: Experiment 9 Name Date Performed 75 pts 1. Mass of Al metal reacted. 0.51 09 2. Mass of alum product 6.80 3. Theoretical yield of alum 10 pts 4. Percent yield of alum, KAl(SO4)2 12H2O 10 pts 15 pts Calculations: Volume of water necessary to dissolve the 6.80 g alum crystals: mL. 9 pts 5. Write the net ionic equations for the reactions of the following compounds with KOI 21 pts . AINO.). (a) ові ове с
Prelab Questions: Name 1) What is the molar mass of KAl(SO4)2 12H20 ? (the 12 waters are part of the molecule) 2) Calculate the mass of alum that can be produced from 14.471g of Al 3) Calculate the mass of alum that can be formed from 0.724 moles of KOH 4) Calculate the mass of alum that can be formed from 1.10 mole of H2SO4 5) a) Based on the data above which reactant is the limiting reactant? b) What...
Chemical Conversion (Stoichiometry): Aluminum Scrap to Alum Data mass of aluminum - 0.54g mass of water + filter paper - 42.84g mass of alum product + watch class + filter paper - 43.70g Calculate the mass of your alum produce - this is the actual yield of you synthesis??? Calculate the molar mass of alum [KAl(SO4)2 * 12H2O] - round the result to the nearest 0.1 gram/mol??? Calculate the theoretical yield in grams for this reaction. Assume the aluminum is...
Chemical Conversion (Stoichiometry): Aluminum Scrap to Alum Data mass of aluminum - 0.54g mass of water + filter paper - 42.84g mass of alum product + watch class + filter paper - 43.70g Calculate the mass of your alum produce - this is the actual yield of you synthesis??? Calculate the molar mass of alum [KAl(SO4)2 * 12H2O] - round the result to the nearest 0.1 gram/mol??? Calculate the theoretical yield in grams for this reaction. Assume the aluminum is...
I synthesized Common Alum in my lab. KAl(SO4)212H2O(s) We then had to find the water content based on the initial mass of the Common Alum subtracted from the anhydrous mass after heating. I had 1g of the Common Alum and after heating it, I had 0.57g and I was able to find the percent of water content: 43%. 1g - 0.57 = 0.43g 0.43g / 1g = 0.43 x 100 = 43% Now I have to calculate the percentage error...
OD) A procedure for purifying solid product compounds. Question 8 (1 point) Alum is a compound used in a variety of applications including cosmetics, water purification, and as a food additive. It can be synthesized from aluminum metal, sulfuric acid, water, and potassium hydroxide, as seen in the following equation: 2 Al(s) + 2 KOH(aq) + 4H2SO4(aq) + 22 H20(1) - 2 KAl(SO4)2-12H2O(s) + 3 H2(g) Using the data below, determine the theoretical yield for this alum synthesis. Assume that...
Alum [KAl(SO4)2·xH2O] is used in food preparation, dye fixation, and water purification. To prepare alum, aluminum is reacted with potassium hydroxide and the product with sulfuric acid. Upon cooling, alum crystallizes from the solution. (a) A 0.4711−g sample of alum is heated to drive off the waters of hydration, and the resulting KAl(SO4)2 weighs 0.2564 g. Determine the value of x and the complete formula of alum. Value of x: Complete Formula: (b) When 0.7339 g of aluminum is used,...
CHEM 101 LAB 7 PRELAB QUESTIONS B C AND D Experiment 7 Preparation of Alum PURPOSE oF EXPERIMENT: Prepare KAI(So,)2 12H20, an aluminum alum, from aluminum metal. (Note: ExPERIMENT 8 describes the gravimetric analysis of the sulfate content in alum.) Alums have the general formula MM(So) 12HO, where M* is commonly Na". K', Tl., NH,., or Ag, and Mt''is A广, Fe". Cr". Ti". or Co. . Samples of these compounds have a variety of uses in our everyday lives. Sodium...
2Al(s)+2KOH(aq)+4H2SO4+22H2O(l)→2KAl(SO4)2⦁12H2O(s)+3H2(g) What is the limiting reactant, theoretical and percent yield of this equation? 1.03 grams of Al foil 35.10 grams of KOH 15 grams of Sulfuric acid 20 grams of water the mass of the product is 24.88 grams
percent error #3 Calculations for Part 2 Ou in KAl(SO4)2 1. Experimental value for percent sulfate in alum BA 0.15793504) H20 12 ( 18.0a)= 216.24 KAYS0y), 12H20 MM (504)₂ = 64.327 128.00 2 = 192.32 glmor 2. Theoretical value for percent sulfate in alum are monologa dobar odbud 3. Percent error Results and Data Analysis Table 1: Determination of the Water of Hydration in Alum Crystals Mass of crucible + cover + alum 43.10509 - water Mass of crucible +...