Interpretation:
The percent yield for the given
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,
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Chapter 6 Solutions
General, Organic, and Biological Chemistry
- Consider the reaction below. If you start with 5.00 moles of C (propane) and 5.00 moles of O₂, how many moles of carbon dioxide can be produced? O C3H8(g) + 5 O₂(g) → 3 CO₂(g) + 4H₂O(g) 20.0 3.00 5.00 15.0 Submit Answer Try Another Version 1 item attempt remaining hp B TE C Previous Y Nextarrow_forwardFor the following reaction, 0.553 moles of potassium hydroxide are mixed with 0.555 moles of phosphoric acid. potassium hydroxide (aq) + phosphoric acid (aq) → potassium phosphate (aq) + water(!) What is the formula for the limiting reagent? Limiting reagent: What is the maximum amount of potassium phosphate that can be produced? Amount moles Submit Answer Try Another Version 10 item attempts remainingarrow_forwardHow many moles of CO2 will be produced from 2.00 moles C2H6O and 5.00 moles O2? C2H6O + 3 O2 → 2 CO2 + 3 H2O Options for answer: 1.67 moles 3.33 moles 4.00 moles 2.00 molesarrow_forward
- When the following molecular equation is balanced using the smallest possible integer coefficients, the values of these coefficients are: Jammonia (g) + oxygen (g) nitrogen monoxide (g) +| water (g) Submit Answer Try Another Version 1 item attempt remainingarrow_forwardSuppose 10.0 g of Compound A are consumed in a rection with excess 10.0 g of Compound B that produces only one product, Compound C. Calculate the theoretical yield of C. Round your answer to the nearest 0.1 g. Suppose 12.6 g of C are actually isolated at the end of the reaction. What is the percent yield of Compound C? Round your answer to the nearest whole percent. Explanation Check 0 0% 0 x10 0.0 X 3 00 S 4 zuza mcGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accearrow_forwardExtra Practice : Predict the products with their states of matter, indicate the type of reaction, and balance the equation for the following chemical reaction: A solution of lead (II) nitrate is mixed with a solution of sodium iodide. nited States) E Accessibility: Good to go D. Focus 目 Page 3 of 4 1200 words English w %23arrow_forward
- Objective Knowledge Check Question 6 Balance the chemical equation below using the smallest possible whole number stoichiometric coefficients. CH,CH, (g) + 0,(g) – co,(g) + H,0(g) I Don't Know Submit O2021 McGraw Hilarrow_forward18 E 20 C Submit Answer $ When H₂S(g) reacts with O₂(g) to form H₂O(g) and SO₂(g), 124 kcal of energy are evolved for each mole of H₂S(g) that reacts. 4 Write a balanced equation for the reaction with an energy term in kcal as part of the equation. Use the SMALLEST INTEGER coefficients possible and put the energy term in an appropriate box. If a box is not needed, leave it blank. 999 F4 R F V + % 5 tivity.do?locator assignment-take T G Retry Entire Group 7 more group attempts remaining tv 6 B [Review Topics] [References] Use the References to access important values if needed for this question. + MacBook Air F6 Y H TAO & 7 17 N F7 U J * - 8 30 FB M ( 9 DI K H Unline teaching and le Xx 0 V F9 I + ) 0 L command PLO F10 P A. > Y 1 option + 4 Email Instructor F11 { [ ? + Previous B + = 11 I A Next> Q2 Tue Save and Exit delete * O return shift Sarrow_forwardPRACTICE EXERCISE : Problem Solving N2 + 3H2 --> 2NH3 How many grams of H2 are needed to react with 4.5 moles of N2? Step 1. Identify the problem. Step 2. Identify the conversion factor based from the balanced chemical equation. Step 3. Find out the number of moles using the Dimensional Analysis. Step 4. Change the moles using the molar mass.arrow_forward
- Exercise: Assume that 10g of K-PtCl, and 10g of NHare allowed to react, how many grams of the excess reactant are consumed, and how many grams remain? R KPtCla + 2NH3 Pt(NH)Cl+ 2KCIarrow_forwardWhich of the following is the correct conversion factor setup for the problem How many grams of H2O can be produced from 3.2 moles of O2 and an excess of H2S via chemical reaction 2H2S + 3O2 2H2O + 2SO2? a. 3.2molesO2(32.00gO21moleO2)(18.02gH2O32.00gO2) b. 3.2molesO2(2molesH2O3MolesO2)(18.02gH2O1moleH2O) c. 3.2molesO2(32.00gO21moleO2)(2molesH2O3MolesO2) d. no correct responsearrow_forward5.0 moles of CO and 7.5 moles of H2 react to form CH3OH. What is the theoretical yield of the reaction (mass of product in grams that will form)? CO(g) + 2H2 (g) à CH3OH (l) Responsesarrow_forward
- General, Organic, and Biological ChemistryChemistryISBN:9781285853918Author:H. Stephen StokerPublisher:Cengage Learning