Interpretation:
The yield that can be measured and not calculated has to be chosen from the given options.
Concept Introduction:
In a
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,
Want to see the full answer?
Check out a sample textbook solutionChapter 6 Solutions
General, Organic, and Biological Chemistry
- Question 1 Homework Complete the mass data table given below. B I X, x' n Undo C Start Over O Row Column Table Title Mass data table Column 1 Column 2 Column 3 Data set name Trial 1 Trial 2 Mass of empty crucible and cover 25.165 g 24.931 g Mass of cover 10.731 g 10.278 g Mass of magnesium ribbon 0.350 g 0.375 g Mass of magnesium ribbon, crucible, 14.784 g 15.028 g Mass of magnesium ribbon, crucible, 25.745 g 25.522 g mass of product 0.580 g 0.591 g mass of oxygen 0.230 g 0.216 g Answered A Resubmit Question 2 Homework Calculate the Empirical formula for Trial 1 by completing the table given below. B I X, x' 2- n Undo C Start Over Column Row Table Title Calculate the Empirical formula for Trial 1 Column 1 Column 2 Column 3 Column 4 Column 5 Trial 1 grams Molar mass moles molar ratio Mgarrow_forwardQUESTION 3 After balancing the following chemical equation, what are the coefficient FeCl2 + NazPO4 - Fe3(РОд)2 + NaCl O A. 3,2,1,6 ОВ. 3,1,1,3 O C. 3,1,1,6 O D. 6,2,2,6 O E. 3,2,1,3 QUESTION 4arrow_forward10. Ca(OH), + H,SO, - CaSO, + H,O How many moles of H,O are produced from 75.0 g of H,SO,? Balancing the equation: Name: Given Molar mass of Mole ratio Answerarrow_forward
- Gaseous butane (CH,(CH reacts with gaseous oxygen gas (0,) to produce gaseous carbon dioxide (CO,) and gaseous water (H,0). What is the theoretical yield of carbon dioxide formed from the reaction of 1.7 g of butane and 4.7 g of oxygen gas? g Round your answer to 2 significant figures. Explanation Check 2021 McGraw HilLLLC AILRights Reserved Terms of UUse Privacy Center Accessibility étv MacBook Air DII DO 10 esc FB F9 F10 F7 F3 @ %23 $ & 7 8 LOarrow_forwardThe balanced reaction of calcium carbonate and hydrochloric acid is as follows: CACO3 (s) + 2 HC1(aq) → CaCl2 (aq) + H2O (1)+ CO2 (g) Reaction equation of calcium carbonate and hydrochloric acid producing calcium chloride, water and carbon dioxide as products Record your moles and percent error calculations for calcium carbonate Trial 1 Trial 2 Trial 3 Value of CaCO3 reported 500 on the bottle (mg) Mass of antacid tablet used (g) 1.22 1.21 1.22 Moles of HCl from part I. .015000 .015000 .015000 Unrounded Moles of NaOH from part II. .0038610 .0039000 .0037080 Unrounded Moles of HCl neutralized by NaOH .011139 Unrounded Moles of HCl neutralized by NaOH Rounded Moles of HCl neutralized by CaCОз Unrounded Moles of HCl neutralized by CaCOз Rounded Moles of CaCO3 Unrounded Moles of CaCO3 Rounded Mass of CaCO3 in tablet (mg) Unrounded Mass of CaCO3 in tablet (mg) Rounded Percent error (%, use rounded values) Unrounded Percent error (%) Rounded Percent effectiveness of tablet (%) Unrounded…arrow_forwardAccording 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_forward
- find Percent yieldarrow_forwardThe 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_forwardFind h2o in mole Find magnesium chlorate in molearrow_forward
- Question 2 of 16 How many moles of H2SO. are required to completely react with 7.20 mol of AlI according to the balanced chemical reaction: Al(s) + H2SO (aq)A:(SO4)s(aq) + 3 H2(g) STARTING AMOUNT ANSWER RESET ADD FACTOR *( ) 1 26.98 98.08 21.6 342.14 3 7.20 10.8 2.02 6.022 x 1023 2.40 3.60 O Type here to searcharrow_forwardQuestion 36 Nitrogen and hydrogen react to form ammonia according to the reaction shown. 3 H2 (g) + N2 =2 NH, What is the percent yield if 18.75 g nitrogen and 10.60 g hydrogen react to form 5.24 g of ammonia? Type answer: CHECKarrow_forwardProblem 7.64 - Enhanced - with Feedback 25 of 33 I Review | Constants | Periodic Table You may want to reference (Pages 245 - 246) Section 7.8 while completing this problem. Part A Calcium cyanamide reacts with water to form calcium carbonate and ammonia via the following reaction: How many grams of water are needed to react with 78.0 g CACN,? CACN2(s) + 3H20(1) → CACO3 (s) + 2NH3(g) ΑΣφ mass H20 = g Submit Previous Answers Request Answer X Incorrect; Try Again Part B How many grams of NH3 are produced from 5.19 g CACN2? ? mass NH3 = g Submit Request Answerarrow_forward
- Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub Co