If the theoretical yield of a reaction is 29.1 g and the actual yield is 20.5...

If the theoretical yield of a reaction is 29.1 g and the actual yield is 20.5 g , what is the percent yield?

How many moles of H2 are formed by the complete reaction of 0.384 mol of Al?

Expert Solution

Ans. # % yield = (Actual yield / Theoretical yield) x 100

= (20.5 g/ 29.1 g) x 100

= 70.45 %

# [[[Note: The question does not specify the what reacts with Al to produce H₂. It’s assumed that it is reaction of metal with dilute acid (say, HCl)- one of the commonest possible reaction. Please let me know if the reaction is a different one. ]]]

Balanced reaction: 2 Al + 6 HCl -----------> 2 AlCl₃ + 3 H₂

Stoichiometry: 2 mol of Al produces 3 mol H₂.

So, moles of H₂ produced by 0.384 mol Al = (3 mol H₂ / 2 mol Al) x 0.384 mol Al

= 0.576 mol

queen_honey_blossom answered 2 years ago

Q1: If the theoretical yield of a reaction is 24.8 g and the actual yield is...

Q1: If the theoretical yield of a reaction is 24.8 g and the actual yield is 18.5 g, what is percent yield? Q2: When 11.5 gram of C are allowed to react with 114.5 g Cu2O, 87.4 g of Cu are obtained. Determine the limiting reactant, theoretical yield and percent yield. Q3:This reaction of 185 g of Fe2O3 with 95.3 g of CO produces 87.4 g of Fe. Determine limiting reactant, theoretical yield, and percent yield.

Define the following: limiting reagent, theoretical yield, actual yield, percent yield, enthalpy of reaction, exothermic reaction,...

Define the following: limiting reagent, theoretical yield, actual yield, percent yield, enthalpy of reaction, exothermic reaction, endothermic reaction.

a) What is the theoretical yield of ethyl chloride in the reaction of 19.9 g of...

a) What is the theoretical yield of ethyl chloride in the reaction of 19.9 g of ethylene with 50 g of hydrogen chloride? (For ethylene, MW=28.0amu; for hydrogen chloride, MW=36.5amu; for ethyl chloride, MW=64.5amu.) H2C=CH2+HCl→CH3CH2Cl b) What is the percent yield if 24.0 g of ethyl chloride is actually formed?

Calculate theoretical yield, actual yield and percent yield. Data: mass recovered: 12.1188 g. 2-methylcyclohexanol MM: 114.2...

Calculate theoretical yield, actual yield and percent yield. Data: mass recovered: 12.1188 g. 2-methylcyclohexanol MM: 114.2 g/mol D: 0.930 g/mL BP: 166 C 1-methylcyclohexene MM: 96.2 g/mol D:0.813 g/mL BP: 110 C

What is the theoretical yield of both products of the reaction between 17.56 g of carbon...

What is the theoretical yield of both products of the reaction between 17.56 g of carbon disulfide and an excess of oxygen? First write a balanced equation of this reaction that results in the formation of carbon dioxide and sulfur dioxide. What is the percent yield if this reaction produces 15.75 g of sulfur dioxide? Which is the limiting reagent if we only use 25.45 g of Oxygen?

Consider the following reaction: 2SO2(g)+O2(g)→2SO3(g) What is the theoretical yield of SO3? If 188.5 mL of...

Consider the following reaction: 2SO2(g)+O2(g)→2SO3(g) What is the theoretical yield of SO3? If 188.5 mL of SO3 is collected (measured at 327 K and 54.5 mmHg ), what is the percent yield for the reaction?

Consider the following reaction: 2SO2(g)+O2(g)→2SO3(g) Part B What is the theoretical yield of SO3? nSO3 =...

Consider the following reaction: 2SO2(g)+O2(g)→2SO3(g) Part B What is the theoretical yield of SO3? nSO3 = Part C If 175.8 mL of SO3 is collected (measured at 327 K and 48.7 mmHg ), what is the percent yield for the reaction? Express your answer using four significant figures.

what is theoretical yield and actual yield of this experiment. 1.104g of cysteine hydrochloride monohydrate added...

what is theoretical yield and actual yield of this experiment. 1.104g of cysteine hydrochloride monohydrate added with 2.5 ml of freshly made 10% aqueous sodium hydroxide solution and 10 ml of 3% aqueous hydrogen peroxide solution. product was 0.336g of Cystine

For the reaction Ti(s)+2F2(g)→TiF4(s) compute the theoretical yield of the product (in grams) for each of...

For the reaction Ti(s)+2F2(g)→TiF4(s) compute the theoretical yield of the product (in grams) for each of the following initial amounts of reactants. Part A 4.0 g Ti, 4.0 g F2 Part B 2.3 g Ti, 1.4 g F2 Part C 0.227 g Ti, 0.293 g F2

For the reaction Ti(s)+2F2(g)?TiF4(s) compute the theoretical yield of the product (in grams) for each of...

For the reaction Ti(s)+2F2(g)?TiF4(s) compute the theoretical yield of the product (in grams) for each of the following initial amounts of reactants. 2.4 g Ti, 1.6 g F2 0.233 g Ti, 0.288 g F2

Question