What is the theoretical yield (in grams) of the product, Al2 O3 (101.962g/mol) when 15.0g of each reactant is allowed to react by the following equation? NOTE: This is a limiting reactant problem. 4Al(s) + 3O2(g) --> 2Al2O3(s)
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.
What is the theoretical yield (in grams) of the product, Al2 O3 (101.962g/mol) when 15.0g of...
1. What is the theoretical yield in grams of SiF4 (104.08 g/mol) if 37.1 g of SiO2 (60.08 g/mol) are allowed to react with 106.9 g of hydrogen fluoride? SiO2 + 4HF---> SiF4 + 2H2O 2. What is the theoretical yield in grams of Fe2O3 if 54.9 g of iron are allowed to react with 13.5 g of molecular oxygen? 4Fe + 3O2 ---> 2 Fe2O3
For each of the reactions, calculate the mass (in grams) of the product formed when 3.14 g of the underlined(bold) reactant completely reacts. Assume that there is more than enough of the other reactant. Ba(s)+Cl2(g)→BaCl2(s) CaO(s)+CO2(g)→CaCO3(s) 2Mg(s)+O2(g)→2MgO(s) 4Al(s)+3O2(g)→2Al2O3(s)
Chem 143 - Lab 46) CALCULATE THE THEORETICAL YIELD Grams of sodium carbonate used Moles of sodium carbonate used Grams of calcium chloride used Moles of calcium chloride used Moles of precipitate expected Theoretical yield of precipitate in grams Actual yield of precipitate in grams Percent yield 5.6 Show detailed work for percent yield. Page 4 of 4 Chem 143 - Lab Pre-lab Exercise Show the details of each calculation to get full credit 1. Magnesium oxide, a white powdery...
NAME 1) For the reaction shown, find the limiting reactant and the theoretical yield in moles of potassium chloride (CI) with the following initial quantities of reactants: 14.6 mol K, 7.8 mol Cla 2 K{s} + Cla(g) – 2 KCl(s) 2) For the reaction shown, find the limiting reactant and the theoretical yield of the product (LiF) in grams for the following initial quantities of reactants: 10.5g Li and 37.2g F2 2 Li(s) + F2(g) → 2 Lif(s) 3) Consider...
for the reaction shown, find the limiting reactant for each of the following initial amounts of reactants. 4Al(s)+3O2(g)->2Al2O3(s) -11.4 mol Al,9.5 mol O2 -1 mol Al,1 mol O2 -20 mol Al,16 mol O2 -4mol Al,2.6 mol O2
3. How many grams of Alum could form (theoretical yield) when 1.00 g Al (limiting reactant) is used according to the balanced chemical equation given below? 2Al(s) + 2KOH(aq) + 4H2SO4 + 22H2O(1) ► 2KAI(SO4)2:12H2O(s) + 3H2(g)
The theoretical yield of 1,2-epoxycyclohexane is _grams, when starting with 3.0 grams of trans-2- bromocyclohexanol. (Enter the number using 3 significant figures, i.e. 1.22) Given: 3.0 g of trans-2-bromocyclohexanol FW: 179.05 25 mL of 10% NaOH FW: 40 and density: 1.11 g/mL 1,2-expoxycyclohexane FW: 98.15 Hint: Identify the limiting reactant (NaOH or trans-2- bromocyclohexanol) by calculating the number of moles of each. For 1 mole of limiting reactant, 1 mole of product is formed. Use the # of moles and...
Aluminum oxidizes according to the following equation: 4 Al + 3 O2 -> 2 AL2 O3. If 0.048 mol of Al is placed into a container with 0.030 mol O2, what are the limiting and excess reactants? Based on the previous question, how many moles of excess reactant remain?
What is the theoretical yield (in grams) of phosphorus pentachloride when 3.85 g of phosphorus reacts with 25.8 g of chlorine according to the following reaction: P4 (s) + 10 Cl2 (g) → 4 PCl5 (l) Use the correct number of significant figures, fill in the number ONLY! lan 4 15 What is the mass of excess reactant (in grams) that remains after the limiting reagent produces the maximum amount of phosphorus pentachloride possible upon the reaction of 4.69 g...
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