Interpretation:
From the given amount of reactants, the maximum amount of product that can be obtained by a
Concept Introduction:
In a chemical reaction, when the reactants gives product, the amount of product formed from the given amount of reactant can be said in terms of yield.
Theoretical yield of a chemical reaction is the maximum amount of the product that can be obtained from the given amount of reactants provided there is no loss or inefficiencies occur. The actual yield of the chemical reaction is the experimental yield that is obtained. Actual yield of the product is always lesser than the theoretical yield. For this, there are two reasons. They are,
- In mechanical process, some of the product is lost. Mechanical process involves the transfer of materials from a container to another container.
- Unwanted side reactions occur in the actual chemical reaction due to impurities present. These are not considered in theoretical yield.
Actual yield is the amount of product that is got from a chemical reaction. The actual yield has to be measured and not calculated.
Percent yield is the term that is used to tell about the product loss. It is the ratio of the actual amount of product that is obtained in a chemical reaction to the theoretical yield multiplied by 100 to give percent. Mathematical equation for percent yield is given as,
Trending nowThis is a popular solution!
Chapter 6 Solutions
Bundle: General, Organic, And Biological Chemistry, Loose-leaf Version, 7th + Lms Integrated For Owlv2 With Mindtap Reader, 4 Terms (24 Months) ... Chemistry (powered By Owlv2), 4 Terms (2
- The illustration to the left represents a mixture of nitrogen ( blue ) and hydrogen ( light blue ) molecules. 8. If the molecules in the above illustration react to form NH3 according to the equation N2 + 3 H2 →2 NH3, the limiting reagent is the number of NH3 molecules formed is and the number of molecules in excess is Submit Answer Try Another Version 2 item attempts remainingarrow_forwardWhat is the percent yield when 32.18 g of octasulfur reacts with excess fluorine gas to produce 41.52 g hexaflouride. How much of the fluorine gas is consumed? S8 + F2 ---> SF6 Answer: Percent yield of SF6____________ Consumed F2________arrow_forwardAccording to the following reaction, how many moles of iron(II) oxide will be formed upon the complete reaction of 0.315 moles iron with excess oxygen gas? iron (s) + oxygen (g) →iron(II) oxide (s) moles iron(II) oxide Submit Answer Try Another Version 3 item attempts remainingarrow_forward
- According to the following reaction, how many moles of carbon dioxide will be formed upon the complete reaction of 0.359 moles carbon monoxide with excess oxygen gas? carbon monoxide (g) + oxygen (g) >carbon dioxide (g) moles carbon dioxide Submit Answer Try Another Version 3 item attempts remainingarrow_forwardDue: All changes s 3. How many moles of NaF are produced in the reaction between sodium bromide and calcium fluoride when 550 grams of sodium bromide are used? 2 NaBr+ CaF2 2 NaF+ CaBr2 O 5g NaF O 5.35 mol NaF O 10.7 mol NaF O 0.53 mol NaF 3 00:58:55 PREVIOUS 3 of 12 NEXT 4. 7arrow_forwardAccording to the following reaction, how many moles of copper(II) nitrate will be formed upon the complete reaction of 21.5 grams of silver nitrate with excess copper? silver nitrate (aq) + copper (s) >copper(II) nitrate (aq)+ silver (s) moles copper(II) nitrate Submit Answer Try Another Version 1 item attempt remainingarrow_forward
- 2.6 g sodium with 5 g chlorine gas recovers 5.8 g sodium chlorine whats percent yieldarrow_forwardExtra Exercise 3. In a baker , Sulfide is mixed with of aluminium Chloride, we obtain a mixture sodium chloride solution and aluminium Sulfide Solution. 1 Write the equation of the rxn 2 Calculate the initial' number of moles f reactants. 3. Are the reactants in stoichio metric mixture; if not determine the limiting reactant. 4. Calculate the mass of the oblained products and the mass of the exces reactant. Given: M (Na): 23 g.mol"; M(S). MLAI) = 279.mol ; M(Cl)=35.5g.mo. a solution containing 9.36 9 Sodium a solution contening 5,34g 1- %3Darrow_forwardProblems Mole.Mole and Mole.Mass.docx (22.7 KB) Directions: Answer each of the following questions using the equation provided. Be sure to balance each equation before solving any problems. Show all work for full credit. 1 point each for balancing each equation 1 point per question Problem Set 1: Cu + O, Cuo 1. If 101 grams of copper is used, how many moles of copper (II) oxide will be formed? 2. If 5.25 moles of copper are used, how many moles of oxygen must also be used? 3. If 78.2 grams of oxygen react with copper, how many moles of copper (II) oxide will be produced? Problem Set 2: С.Н. + O, CO, + H.O 4. How many moles of butane, C.H, are needed to react with 5.5 moles of oxygen? How many grams of carbon dioxide will be produced if 3.5 moles of O, react? 5. Prohlem Set 3: 54°F Sunny DELL F11 F12 F10 F9arrow_forward
- Stoichiometry Worksheet 6- Rev 12 Exercise C - Stoichiometry 1 ar For this problem, identify the limiting reagent and calculate the grams of Al2O3 obtained in the reaction of 200.0 grams of aluminum with 150.0 grams oxygen. If 85.50 grams of Al203 is actually produced, what is the % yield. The equations are not balanced. Al + O2- Al2O3 What is the limiting reagent? How many grams Al2O3 will be produced? If 85.5 grams of Al2O3 is produced, what is the % yield.arrow_forwardQuestion 69 Nice Consider the following equation 2 Mg (s) + O2 (g) → 2MgO (s) The number of moles of oxygen gas needed to react with 4.0 moles of Mg is ______ Group of answer choices 4.0 mole. 3.0 mole. 2.0 mole. 1.0 mole.arrow_forwardThe problem How many grams of O2 are needed to produce 2.00 moles of H2O via the chemical reaction 2H2 + O2 2H2O? is characterized as a a. moles of A to grams of A problem b. grams of A to moles of B problem c. moles of A to grams of B problem d. no correct responsearrow_forward
- General, Organic, and Biological ChemistryChemistryISBN:9781285853918Author:H. Stephen StokerPublisher:Cengage Learning