### Title: Silver Recovery via Reduction ReactionIn this example, silver metal is recovered during the reduction of silver nitrate:\[ \text{Cu}(s) + 2 \text{AgNO}_3(aq) \rightarrow 2 \text{Ag}(s) + \text{Cu(NO}_3)_2(aq) \]**Problem Statement:**During an experiment, 125 grams of copper (Cu) were placed into a solution containing 275 grams of silver nitrate (AgNO₃). As a result, 135 grams of silver (Ag) were recovered. The task is to determine the percent yield of the silver (Ag) obtained.**Details:**- **Cu (Copper):** 125 grams- **AgNO₃ (silver nitrate):** 275 grams- **Recovered Ag (Silver):** 135 grams**Objective:**Calculate the percent yield of silver (Ag) obtained from the reaction.**Percent Yield Calculation:**Percent yield is calculated as follows:\[ \text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100 \]For this reaction:- Find the theoretical yield of silver (Ag) using stoichiometry.- Use the given actual yield (135 grams) to compute the percent yield.

Answered: Image /qna-images/answer/23318637-34d9-4f37-8b94-3da304028d45.jpg

Silver metal is recovered during the reduction of silver nitrate: Cu(s) + 2 AgNO3(aq) → 2 Ag(s) + Cu(NO3)2(aq) During an experiment, 125 g of tion containing 275 g AgNO,.u were placed into a solu- 135 g Ag were recovered. What is the percent yield of Ag obtained?

Silver metal is recovered during the reduction of silver nitrate: Cu(s) + 2 AgNO3(aq) → 2 Ag(s) + Cu(NO3)2(aq) During an experiment, 125 g of tion containing 275 g AgNO,.u were placed into a solu- 135 g Ag were recovered. What is the percent yield of Ag obtained?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: Silicon, which occurs in nature as SiO2, is the material from which most computer chips are made. If…

A: When two reactive compounds are mixed, then they react according to the stoichiometry of the…

Q: Ca,(PO.) + SiO, +C→ CaSiO, + CO + P

A: The given chemical equation is--- Ca3(PO4)2 + SiO2 + C ------> CaSiO3 + CO + P To balance this…

Q: How many grams of silver nitrate must react to give 1.00 gg of AgAg?…

Q: 5. A student reacts 6.00 g of ammonium sulfide with 6.00 g of zinc (II) acetate. Upon completion of…

A: Limiting reactant :- A reactant which is present in lesser number of molrs than required as per…

Q: Reactant and Theoretical Yield; Read Section 4.4. You can click on the Review link to access the…

Q: A reaction mixture containing 101.7 g titanium(IV) oxide (TiO2; molar mass = 79.88 g/mol), 155.3 g…

Q: 2. Balanced Chemical Equation Reaction Type: At completion of reactions: Grams of nitrogen Grams of…

A: A question based on concentration terms that is to be accomplished.

Q: he percent yield of numerical value or

Q: When 250.0 mL of .2500 M Li2CO3 (aq) were mixed with 350.00 mL of .1500M AlBr3 (aq), 2.500 grams of…

A: Molarity of Li2CO3 = 0.2500 M Volume of Li2CO3 = 250 mL = 0.250 L Molarity of AlBr3 = 0.1500 M…

Q: For the following reaction, 0.431 moles of benzene (C6 H6) are mixed with 0.381 moles of oxygen gas.…

Q: 10.8 mL of 0.25 M HCl(aq) reacts with an excess of Mg(OH)2(aq), what mass of magnesium chloride…

Q: 1.003 g of soduim chloride was recovered in the reaction of Hydrochloric acid + Sodium carbonate →…

A: The reaction of hydrochloric acid with sodium carbonate forms sodium chloride, carbon dioxide and…

Q: Sodium metal reacts with water in the following single-displacement reaction: 2Na(s) + 2H2O(l) →…

A: Here we have to determine the limiting reactant and mass of H2 gas produced when 2.0 g of Na is…

Q: For the following reaction, 57.4 grams of potassium hydroxide are allowed to react with 38.3 grams…

A: The objective of this question is to determine the maximum amount of potassium phosphate that can be…

Q: A student carefully measures 1.069 g of an unknown brown copper chloride and dissolves it into…

A: Let the empirical formula of the copper chloride be CuClx. Copper chloride reacts with Zinc to form…

Q: A mixture of 9.275 g of iron (II) oxide and 8.435 g of aluminum metal is placed in a crucible and…

A: To solve this problem we will use the given chemical equation .

Q: If 45.4 mL of 0.25 M HCl(aq) reacts with an excess of Mg(OH)2(aq), what mass of magnesium chloride…

Q: How many grams of Fe are produced when 62.00 g of Fe2O3 reacts with excess aluminum according to the…

A: Answer Grams of Fe Produced = 43.365 g Explanation According to the balanced equation, 1 mole of…

Q: A student analyzes a sample of rock that contains the element calcium (Ca). In the student's…

A: Given that,182.2 mg of the rock produces 120.7 mg of CaC2O4 on treatment of Na2C2O4 We have to find…

Q: Copper(II) carbonate was used by artists as a pigment due to its bright green-blue colour. It can be…

Q: Hydrobromic acid dissolves solid iron according to the followiaung reaction: Fe(s)+2HBr(aq)→…

A: The reaction of iron and hydrobromide is given by equation 1.So, from equation (1) one mole of iron…

Q: Consider the following balanced equation: 2 Li3PO4 (aq) + 3 Zn(NO3)2 (aq) → Zn3(PO4)2 (s) + 6 LiNO3…

A: Molar mass of zinc nitrate= 189.36 g/mol

Q: For the following reaction, 48.6 grams of potassium hydrogen sulfate are allowed to react with 24.6…

Q: Upon reaction of 1.27 g of copper sulfate with excess zinc metal, 0.239 g copper metal was obtained…

A: The relation to calculate the percentage yield is shown below. % yield=actual yield theoretical…

Q: Consider the following reaction Ca(s) + 2HCl(aq) --> CaCl2(aq) + H2(g) What mass of Ca is needed…

Q: A powder contains FeSO4·7H2O (molar mass = 278.01 g/mol) among other components. A 3.200-g sample of…

A: Answer:The question is based on the concept of gravimetric analysis and Stoichiometric Calculations.…

Q: According to the following reaction, how many grams of silver chloride will be formed upon the…

Q: Complete and balance the reaction equation in Figure 7. What is the molecular formula of the salt…

Q: Aluminum metal reacts with bromine according to the following unbalanced equation: Al (s) + Br₂ (1)→…

A: 4. Recall the given unbalanced equation, Al s + Br2 l → AlBr3 sWant to…

Q: In an experiment,12.4g of KCIO3 were carefully decomposed and 4.52 of O2 gas were collected. What…

A: The percent yield is useful for manufacturing of products and the expression for calculating the…

Q: In an experiment, 0.2490 g of sodium bicarbonate, NaHCO3(s) was allowed to react with excess…

A: In the given question we have to calculate the percent yield of NaCl in the following reaction,…

Q: A sample of ore containing manganese weighed 1.2354 grams. This sample was heated in a solution of…

A: A question based on mole concept. A set of data about the ore is given using that the percentage of…

Q: Hydrogen cyanide, a highly toxic compound, is made by the following reaction: 2 CH4(g) + 2 NH3(g) +…

Q: When an aqueous solution of 6.71 g of barium chloride was added to an aqueous solution of 7.77 g of…

A: The reaction between barium chloride and potassium chromate is shown below, The given grams are…

Q: Consider the mechanism of the reaction shown below. Give the structure of the next important organic…

A: The given reaction is the hydration of alcohol in presence of concentrated sulphuric acid to form…

Q: Determine the mass of sodium nitrate produced when 0.73 g of aqueous nickel(II) nitrate reacts with…

A: NOTE : There is a typing error in question. The solid will be of nickel (II) hydroxide and and…

Q: An aqueous solution containing 9.20 g of lead(II) nitrate is added to an aqueous solution containing…

A: Balancing of chemical reaction- It consists of reactant (starting material) and products…

Q: the References to access important values if needed for this question. For the following reaction,…

Q: Suppose a 250. mL flask is filled with 0.40 mol of CO, 1.6 mol of CO₂ and 0.20 mol of H₂. This…

A: The ICE table gives the initial concentration of compounds, change in concentration of compounds,…

Q: Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with…

Q: If 25.5 mL of a 0.123 M solution of iodide was added to 22.3 mL of a 0.209 M solution of iodate ions…

A: The reactants given are iodide i.e I- and Iodate i.e IO3- and the product forming is I3-. Hence the…

Q: For the following reaction, 0.308 grams of hydrogen gas are allowed to react with 42.9 grams of…

Q: A student is looking to react barium ions in solution (Ba²+ (aq)) with something that will make them…

A: The common precipitate with the Ba2+ ion is BaSO4. To get it, we can add H2SO4 to it. Therefore, she…

Q: The drawing below shows a mixture of molecules: carbon nitrogen oxygen key hydrogen sulfur chlorine…

A: Supposed the following chemical reaction take place in this mixture:2H2(g) + O2(g) ---->…

Q: 1. _NaOH + _Cu(NO3)2 → _Cu(0H)2 (s) + _NaNO3| nen 25.00g of NaOH reacts with 25.00g Cu(NO3)2, how…

A: Given chemical equation is :

Concept explainers

Stoichiometry

Stoichiometry is a chemical division that evaluates the quantitative content of the chemical process with the help of the reacting molecules or products taking part in the reaction. The term “stoicheion” in “Stoichiometry”, is an old Greek term for "element" whereas “metron” means "measure".

Question

### Title: Silver Recovery via Reduction Reaction

In this example, silver metal is recovered during the reduction of silver nitrate:
\[ \text{Cu}(s) + 2 \text{AgNO}_3(aq) \rightarrow 2 \text{Ag}(s) + \text{Cu(NO}_3)_2(aq) \]

**Problem Statement:**
During an experiment, 125 grams of copper (Cu) were placed into a solution containing 275 grams of silver nitrate (AgNO₃). As a result, 135 grams of silver (Ag) were recovered. The task is to determine the percent yield of the silver (Ag) obtained.

**Details:**
- **Cu (Copper):** 125 grams
- **AgNO₃ (silver nitrate):** 275 grams
- **Recovered Ag (Silver):** 135 grams

**Objective:**
Calculate the percent yield of silver (Ag) obtained from the reaction.

**Percent Yield Calculation:**
Percent yield is calculated as follows:
\[ \text{Percent Yield} = \left( \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \right) \times 100 \]

For this reaction:
- Find the theoretical yield of silver (Ag) using stoichiometry.
- Use the given actual yield (135 grams) to compute the percent yield.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Step by step

Solved in 3 steps with 3 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

Write the balanced NET ionic equation for the reaction when aqueous Cs₃PO₄ and aqueous AgNO₃ are mixed in solution to form solid Ag₃PO₄ and aqueous CsNO₃.
A mixture consisting of only chromium(III) bromide (CrBr3) and aluminum bromide (AlBr3) weighs 1.1218 g. When the mixture is dissolved in water and an excess of silver nitrate is added, all the bromide ions associated with the original mixture are precipitated as insoluble silver bromide (AgBr). The mass of the silver bromide is found to be 2.2708 g. Calculate the mass percentages of chromium(III) bromide and aluminum bromide in the original mixture. Mass percent CrBr3 Mass percent AlBr3 = % %
When exactly 750.0 mL of a solution containing 0.5840 N of magnesium hydroxide was combined with 250.0 mL of a solution containing 0.08090 N sulfuric acid: Molar mass of Mg = 24.31, S = 32.06, H = 1.01, and O = 16 Write a balance equation. Which of these reactants is the limiting one? Which reactant is in excess? How much water molecule was formed in grams? What was the unreacted reagents’ molar concentration?
How many molecules of carbon monoxide (CO) are needed to react with excess iron (III) oxide (Fe₂O 2 3) to produce 11.6 g of iron (Fe)? Fe₂O₂ +3CO→2Fe + 3CO A 11.6 molecules CO FR [] U D 6.02 x 10 molecules of CO 1.88 x 10² molecules of CO 2.0 molecules CO
Identifying the limiting reactant in a drawing of a mixture
What is the percent of chloride ion in a sample if 1.1324 g of the sample produces 1.0881 g of AgCl when treated with excess Ag? Ag+ (aq) + Cl¯(aq) → AgCl(s) • Your answer should contain five significant figures.
Ammonia(NH3) can be produced by the reaction of hydrogen and nitrogen shown in the chemical equation below: N2+3H2→2NH3 If a student makes calculations and finds out that the theoretical yield of ammonia is 107.0g and the actual yield is 92.0g, what is the percent yield?
Sodium hypochlorite is the active ingredient in most household bleach products. One method of preparing this compound is as follows: Cl2(g) + 2N2OH(aq) → NaOCI (aq) + NaCl(aq) + H2O(1) In a certain experiment, 50.0 g chlorine was reacted with 50.0 g sodium hydroxide to yield 37.8 g sodium hypochlorite. (a) Calculate the theoretical yield (b) Calculate the percent yield.
Chlorine gas can be prepared in the laboratory by the reaction of hydrochloric acid with manganese(IV) oxide. 4 HCl(aq) + MnO₂ (s) - - MnCl₂(aq) + 2 H₂O(l) + Cl₂(g) A sample of 36.9 g MnO, is added to a solution containing 44.7 g HCI. What is the limiting reactant? MnO₂ HCI What is the theoretical yield of Cl₂? theoretical yield: If the yield of the reaction is 86.3%, what is the actual yield of chlorine? g CL₂
Iodine is prepared both in the laboratory and commercially by adding Cl, (g) to an aqueous solution containing sodium iodide. 2 Nal(aq) + Cl,(g) I,(s) + 2 NaCI(aq) How many grams of sodium iodide, Nal, must be used to produce 89.9 g of iodine, I,? mass: g Nal
Fe2O3 (s) + 3CO(g)→2Fe(s) + 3CO2(g) In a reaction mixture containing 181 g Fe2O3 and 65.4 g CO, CO is the limiting reactant. Part A Calculate the mass of the reactant in excess (which is Fe2O3) that remains after the reaction has gone to completion. Express the mass with the appropriate units. O μÅ Value Units ?
What is the amount of excess reactant left over at the end of the reaction. Use the first image as an example.