A sample of 1.0 mol dm-3 copper (II) sulfate solution was electrolyzed for 1 hour using copper...
Question:
A sample of 1.0 mol{eq}\cdot {/eq}dm{eq}^{-3} {/eq} copper (II) sulfate solution was electrolyzed for 1 hour using copper electrodes. Which change would have caused the largest increase in the amount of copper deposited?
a. increasing the concentration of the copper (II) sulfate to 1.1 mol{eq}\cdot {/eq}dm{eq}^{-3} {/eq}
b. increasing the current by 10%
c. increasing the surface area of the electrodes by 10%
d. changing the electrodes from copper to graphite
Faraday's First Law:
With electricity, a nonspontaneous chemical reaction is conducted in an electrolytic cell. The amount of required metal deposited can be calculated as:
{eq}\rm mass\,of\,the\,metal= \dfrac{E\times I \times time}{F} {/eq}
E=equivalent weight of the metal.
I=current in amp
F=96500 Coulombs
Answer and Explanation: 1
Become a Study.com member to unlock this answer! Create your account
View this answerThe given data is:
Time = 1 hour
{eq}\rm Cu^{2+} = 1.0 M {/eq}
The reaction that takes place at the cathode is:
{eq}\rm Cu^{2+}(aq) \to...
See full answer below.
Ask a question
Our experts can answer your tough homework and study questions.
Ask a question Ask a questionSearch Answers
Learn more about this topic:
Get access to this video and our entire Q&A library
Electrolysis: Definition, Types & Uses
from
Chapter 20 / Lesson 5
47K
Discover what electrolysis is, how energy changes during an electrolysis reaction, and electrolysis of water and metals. View its manufacturing and industrial uses.
Related to this Question
- A copper wire weighing 5.463 g was dissolved in excess nitric acid, precipitated as copper (II) carbonate with excess sodium carbonate, and then converted to copper (II) sulfate pentahydrate using exc
- The addition of 0.40 g of zinc powder (a slight excess) to 25.0 mL of 0.200 M copper sulfate solution causes a maximum temperature rise of 9.5 C in the solution due to the metal replacement reaction: Z n ( s ) + C u S O 4 ( a q ) C u ( s ) + Z n S O 4
- 2. Fill the cuvettes with the following amounts of 0.06 M copper (II) sulfate solution and 1.0 M nitric acid (HNO3):
- A few drops of water were added to a test tube containing 0.5 grams of anhydrous copper sulfate (CuSO4) and the following observations were noted. Anhydrous copper sulfate: light blue Anhydrous copper sulfate plus water: sky blue What can you conclude fro
- Two experiments were conducted: 2.750 g of copper (II) oxide, CuO2, was reduced by heating at high pressure with excess hydrogen to yield 2.196 g of copper Cu. 1.179 g of copper Cu was dissolved in nitric acid to yield copper(II) nitrate, which was conver
- Copper sulfate is a hydrated crystal with the formula CuSO_4 cdot 5H_2O and a deep blue colour. When it's heated, the crystals crumble and turn white. (a) Propose an explanation for this change of c
- A student used 5.06 g copper sulphate pentahydrate and salicyclic acid in the performance of the experiment. The student recovered 3.094 g of salicyclic acid and 2.146 g of copper sulphate pentahydrat
- A student dissolved a piece of copper wire, then converted it to CuO, filtered the CuO from solution, and determined the mass of the CuO. The CuO was then dissolved, reduced to copper metal, and recov
- The metal used to recover copper from a solution of copper sulphate is A. Na B. Ag C. Hg D. Fe
- Aqueous ammonia was added to a solution of copper (ll) sulphate drop wise until in excess. State the observations made when a few drops of aqueous ammonia were added.
- After a reaction involving copper (II) sulfate (blue) and aluminum metal are involved, there is a tinge of blue solution. The blue solution indicates: a) excess CuSO4 b) limited amounts of Al2(SO4)3 c) excess Al2(SO4)3 d) limited amounts of CuSO4
- Two experiments were conducted: Exp 1: 4.125 g of copper(II) oxide, was reduced by heating at high pressure with excess hydrogen to yield 3.294 g of copper Cu. Exp 2: 1.179 g of copper Cu was dissol
- There are two possible methods for recovering copper from a solution of copper(II) sulfate, one uses precipitation and the other uses redox. (a) Copper(II) ions can be precipitated as copper(II) carbo
- Each copper (II) sulfate unit is associated with five water molecules in crystalline copper (II) sulfate pentahydrate (CuSO4 . 5H2O). When this compound is heated in air above 100^oC, it loses the water molecules are also its blue color: CuSO4 . 5H2O &ri
- When 25.0 g of copper (II) sulfate pentahydrate (bluestone) is heated, all the water of hydration is removed from the compound, leaving behind pure anhydrous copper (II) sulfate. What would its dehydrated mass (in grams) be?
- If a larger amount of calcium sulfate [It does not form a gas with the addition of HCl(aq)] is present in the original sample,how does it affect the reported a.molar volume of the CO2(g)-too high,too
- A sample weighing 0.0123 g was dissolved in concentrated nitric acid to convert all of the arsenic to arsenate. The solution was diluted 10 times and excess silver added to precipitate silver arsenate (Ag_3 \cdot AsO_4), which was collected, dried, and we
- A mixture of oxygen and hydrogen is analyzed by passing it over hot copper oxide and through a drying tube. Hydrogen reduces the CuO to metallic Cu. Oxygen then re-oxidizes the copper back to CuO.
- A greenish-blue salt known to be composed of copper and chloride ions is dissolved in DI water. Aluminum metal is used to reduce the copper ions to metallic, copper, which is then collected, dried, and weighed. If the original sample has a mass of 1.362 g
- A 2.00-gram sample of copper (II) acetate produced 2.48 grams of copper (II) formate hydrate. After heating the sample, the final mass of the copper (II) formate was 1.69 grams. What was the degree of hydration for the copper (II) formate?
- One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(
- Copper reacts with aqueous silver nitrate to produce silver metal. The following data were collected. initial mass of copper = 1.76 g final mass of copper = 1.12 g mass of filter paper = 0.91 g mass of filter paper plus silver = 3.12 g a. Write the balanc
- A 2.5g sample of impure Copper was analyzed by allowing it to react with 45mL of 5M Nitric Acid to form Copper (II) Nitrate, Nitrogen Dioxide, and Water. Of the Nitric Acid, .0125mol remained. Assumin
- Epsom salt is chemically known as A. copper sulphate B. magnesium sulphate C. ferrous sulphate D. copper sulphate
- The sulfate ion concentration in natural water can be founded by measuring the turbidity that results when an excess of BaCl2 is added to a measured quantity of the sample. A turbidimeter, the instrument used for this analysis, was calibrated with a serie
- A copper cycle experiment takes copper atoms through reactions that produce copper compounds and complexes one after the other, finally producing elemental copper. Copper atoms are conserved throughou
- A mixture of oxygen and hydrogen is analyzed by passing it over hot copper oxide and through a drying tube. Hydrogen reduces the CuO to metallic Cu. Oxygen then reoxidizes the copper back to CuO. We know that 100 cm^3 of the mixture measured at 25 degrees
- A hydrate of copper(II) sulfate was thermally decomposed to 0.7981 g CuSO4 and 0.5405 G of H20. Derive the value of X for the hydrate, CuSo4 XH20. (Assume CuSo4, 159.62 amu, H20, 18.02amu
- Copper(II) oxide, CuO, may be formed when copper metal is gently heated in air or oxygen gas. Copper metal surfaces that have been tarnished by a layer of black CuO can be cleaned by treating the surface with dilute solutions of hydrobromic acid, HBr(aq).
- Consider the statement: "Copper is a red-brown element obtained from copper sulfide ores by heating the ores in air, which forms copper oxide. Heating the copper oxide with carbon produces impure copper, which is purified by electrolysis." Which of the fo
- A student was asked to prepare a sample of copper (ii) sulfate crystals (CuSO4 5H2O) given 5 g of copper (ii) oxide (CuO) as the starting material. If 10 g of dry crystals of CuSO4 5H2O were obtained,
- How would the following affect (increase, decrease, or not change) the percent SO/by mass in your alum? Justify your answer. a. Your alum was wet. b. You forgot to add HCl to y our precipitation mix
- The hydration of anhydrous copper sulfate is represented by the following reaction: *CuSO4 (s) + 5 H2O (l) --> CuSO4*5H2O (s) Select the best answer from the choices below. A) The hydration of anhyd
- When copper (II) sulfate pentahydrate ( C u S O 4 5 H 2 O ) is heated, it decomposes to the dehydrated form. The waters of hydration are released from the solid crystal and form water vapor.The hydrated form is medium blue, and the dehydrated solid is l
- Copper was determined in a river water sample by atomic absorption spectrometry and the method of standard additions. For the addition, 300.0 ?L of a 1000.0-?g/mL standard was added to 250.0 mL of sol
- Chemistry of Copper Production "Native, " or elemental, copper can be found in nature, but most copper is mined as oxide or sulfide minerals. Chalcopyrite (CuFeS_2) is one copper mineral that can be c
- A student is doing the experiment Chemical Formulas of Copper Sulfide by heating copper with excess of sulfur at very high temperatures using a Bunsen burner. Copper and sulfur react stoichiometrically and excess of sulfur escapes from the crucible as sul
- A 1.000 g sample of copper metal is heated in a crucible and after 15 minutes the mass of the crucible contents is 1.111 g. Calculate the mass of copper (II) oxide that was produced.
- Does the chemical structure of the solid, magnesium sulfate (MgSO4), change when it is added to the water? Is this a physical change or a chemical change?
- How would the following affect (increase, decrease or not change) the percent SO^2-_4 by mass in your alum? Justify your answer. a. Your alum was wet. b. You forgot to add HCl to your precipitation
- A 3.75-g sample of iron ore is transformed to a solution of iron(II) sulfate, FeSO4, and this solution is titrated with 0.150 M K2Cr2O7 (potassium dichromate). If it requires 43.7 mL of potassium dichromate solution to titrate the iron(II) sulfate solutio
- There are two steps in the extraction of copper metal from chalcocite, a copper ore. In the first step, copper (I) sulfide and oxygen react to form copper (I) oxide and sulfer dioxide: 2Cu2S(s) + 3O2(g) → 2Cu2O(s) + 2SO2(g) In the second ste
- Copper oxide is a black powder. It can be decomposed by heating it with an excess of charcoal, a form of carbon. The charcoal reacts with the copper oxide to produce copper and carbon dioxide. Any excess charcoal that was used can be separated from the co
- An 8.75-g sample of iron ore (mixture) is transformed to a solution of iron(II) sulfate, and this solution is titrated with 0.150 M K2Cr2O7 potassium dichromate. If it requires 67.8 mL of potassium dichromate solution to titrate the iron(II) sulfate solut
- A sample of pressure-treated wood weighing 0.3245 g was dissolved in concentrated nitric acid to convert all of the arsenic to arsenate. The solution was diluted 10 times and excess silver added to precipitate silver arsenate (Ag_3AsO_4), which was colle
- Data Table 1. Redox Reaction of Copper and Silver Nitrate. Initial observations: before beginning Copper: thin squares Silver Nitrate: Clear Liquid Observations Cu turning black Observations after
- A rock containing copper is pulverized, and all copper is extracted from it with nitric acid. To make a standardization plot, you make 5 standards and measure their absorbance. The graph you obtain has a trend line of y = 2.4238x + 0.0141. You take the ab
- A 0.4858 g sample of pewter, containing tin, lead, copper, and zinc, was dissolved in acid. Tin was precipitated as SnO2 4H2O and removed by filtration. The resulting filtrate and washings were dilute
- A 0.4423 g sample of pewter, containing tin, lead, copper, and zinc, was dissolved in acid. Tin was precipitated as SnO2 4H2O and removed by filtration. The resulting filtrate and washings were dilute
- A 0.4718 g sample of pewter, containing tin, lead, copper, and zinc, was dissolved in acid. Tin was precipitated as SnO2 4H2O and removed by filtration. The resulting filtrate and washings were dilute
- A 0.4436 g sample of pewter, containing tin, lead, copper, and zinc, was dissolved in acid. Tin was precipitated as SnO2 4H2O and removed by filtration. The resulting filtrate and washings were dilute
- Introduction to Chromatography: Quantification of copper in solution - the standardized solution of NaOH is used: o When the sample coming off the ion exchange column has been collected, where are the colored ions?
- Bornite (Cu 3 FeS 3 ) is a copper ore used in the production of copper. When heated, the following reaction occurs. 2 Cu 3 FeS 3 (s) + 7 O 2 (g) ? 6 Cu(s) + 2 FeO(s) + 6 SO 2 (g) If 3.88 metric tons
- How would the empirical formula of copper (II) sulfate be affected if some of the samples stick to the stirring rod?
- A student conducts an experiment to determine the carbonate ion content in sand. He first takes 1.00 gram of sand into a beaker. Using burette, he adds drops of hydochloric acid (HCl) with concentration 1.00 M. A fizzy is observed upon the addition of HCl
- Your lab instructor asks you to prepare a series of five standard solutions to be used to make a Beer's Law plot for copper sulfate which is blue-colored. The first solution should be 1/2 the concentr
- One way in which the useful metal copper is produced is by dissolving the mineral azure, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II
- Each copper(II) sulfate unit is associated with five water molecules in crystalline copper(II) sulfate pentahydrate (CuSO4 5H2O). When this compound is heated in air above 100 degrees Celsius, it loses the water molecules and also its blue color. CuSO4 5H
- Theoretically, if you start with 0.325 g of copper, after the second lab day you should recover ________ grams of copper.
- In the COD measurement of a raw wastewater sample, the initial K2Cr2O7 concentration added into the wastewater sample is 3.000 g/L. After the redox reaction has reached an equilibrium, the K2Cr2O7 concentration has been reduced to 1.824 g/L.
- Why is copper metal easier to produce than iron metal? a. Copper is easier to reduce than iron. b. Copper can be reduced by oxidizing the attached sulfur with oxygen. c. Iron requires toxic carbon monoxide for the reduction process. d. All of these are tr
- The amount of ammonium added to your penny solution was not controlled (i.e. you did not add "stoichiometric" amounts). Discuss what would happen to its absorbance value, and explain why, if the amoun
- Empirical Formula of Copper Sulfate Mass of crucible and cover + copper wire(befrore heating) 41.94 grams Mass of crucible and cover 40.16 grams Mass of copper wire 0.0118 Mass of crucible and cove
- Would your experiment percent sulfate be high or low if your alum sample had a soluble non-sulfate impurity, for example, water?
- Could blue copper sulfate pentahydrate be ground and used as a pigment for making paint? Why?
- In an experiment, a mixture of copper and sulfur was heated to produce a sample of copper sulfide. The following data were obtained. Calculate the empirical formula of copper sulfide. Weight of the empty crucible = 2.077 grams Weight of the crucible + cop
- When a 8.192 g sample of bluish-green crystals of hydrated nickel(II) sulfate is heated, all of the water of hydration is lost leaving 4.826 g of anhydrous nickel(II) sulfate. Write the formula of the hydrated crystal, showing the number of moles of water
- It is often possible to change a hydrate into an anhydrous compound by heating it to drive off the water (dehydration). Write an equation that shows the dehydration of manganese(II) sulfate dihydrate
- Add the first chemical Na_2CO_3 to a test tube and then add the second chemical AgNO_3 until a change is observed. What is the colour of the chemical Na_2CO_3 before the mixture and the colour of AgNO_3 before the mixture, the available ions for Na_2CO_3
- A 0.5412 g sample of pewter, containing tin, lead, copper, and zinc, was dissolved in acid. Tin was precipitated as SnO_2 4H_2O and removed by filtration. The resulting filtrate and washings were dilu
- A sample of iron(II) sulfate was heated in an evacuated container to 920 K, where the following reactions occurred. Reaction (a): 2 FeSO_4(s) to Fe_2O_3(s) + SO_3(g) + SO_2(g). Reaction (b): SO_3(g) t
- A 1.268-gram sample of a metal carbonate, MCO3, was treated with 100.00 mL of 0.1083 M H2SO4, yielding CO2 gas and an aqueous solution of the metal sulfate. The solution was boiled to remove all of the dissolved CO2 and then was titrated with 0.1241 M NaO
- When copper (II) carbonate is heated, it forms copper (II) oxide and carbon dioxide gas.
- A hydrate of copper (II) chloride has the following formula: C u C l 2 x H 2 O . The water in a 3.41 g sample of the hydrate is driven off by heating. The remaining sample has a mass of 2.69 g. Find the number of waters of hydration ( x ) in the hydrat
- Would it be feasible to store a solution of copper sulfate in a container made of metallic zinc? Of metallic silver?
- Red scale residue (COPPER II) partly dissolves in dilute acid to form a pale blue solution. Name the pale blue solution
- There are two steps in the extraction of copper metal from chalcocite, a copper ore. In the first step, copper(I) sulfide and oxygen react to form copper(I) oxide and sulfur dioxide: 2 Cu_2S(s)+3 O_2
- A 0.4676 g sample of pewter, containing tin, lead, copper, and zinc, was dissolved in acid. Tin was precipitated as.SnO_2 4H_2O and removed by filtration. The resulting filtrate and washings were di
- A 0.4467 g sample of pewter, containing tin, lead, copper, and zinc, was dissolved in acid. Tin was precipitated as SnO_2 4H_2O and removed by filtration. The resulting filtrate and washings were dil
- A 0.4684 g sample of pewter, containing tin, lead, copper, and zinc, was dissolved in acid. Tin was precipitated as SnO_2 4H_2O and removed by filtration. The resulting filtrate and washings were di
- A 0.4543 g sample of pewter, containing tin, lead, copper, and zinc, was dissolved in acid. Tin was precipitated as SnO2 4H2O and removed by filtration. The resulting filtrate and washings were dilu
- A sample of 2.12 g of copper was heated in an oxygen atmosphere until no further change took place. The resulting oxide weighed 2.65 g. Calculate the empirical formula of the oxide.
- In an experiment to electroplate iron with silver, a current of 0.5 amperes was passed through a solution of silver nitrate for one hour. Give two reasons why it is necessary to electroplate with silver.
- In the traditional copper cycle experiment, the first step is the formation of copper (II) nitrate by the reaction of nitric acid with Cu(s). The other products are water and a colorless gas. The colorless gas then reacts with oxygen to form what reddish-
- Copper metal and zinc metal react differently in the presence of certain acids. For example, while both react with concentrated nitric acid and dissolve completely, only zinc reacts and dissolves in d
- Iron(II) Sulfate forms a blue-green hydrate with the formula FeSO_4 * H_2O(s). If this hydrate is heated to a high enough temperature, H_2O(g) can be driven off, leaving the dirty yellow anhydrous salt FeSO_4(s). An 18.300-g sample of the hydrate was heat
- A 0.8552g sample of copper alloy is treated with 8 molars nitric acid and filtered and the precipitate is ignited giving a residue of 0.0632g of SnO_2. The zinc is determined in one half of the filtra
- When a 2.118-g sample of copper is heated in an atmosphere in which the amount of oxygen present is restricted, the sample gains 0.2666 g of oxygen in forming a reddish-brown oxide. However, when 2.118 g of copper is heated in a stream of pure oxygen
- A procedure for iodometric determination of Cu in brass has two parts: standardization of a thiosulfate solution and assay of the copper. In the standardization of the thiosulfate solution, a known amount of iodine is created from KIO₃ and excess i
- A 1.268 g sample of a metal carbonate (MCO3) was treated with 100.00 mL of 0.1083 M sulfuric acid (H2SO4), yielding CO2 gas and an aqueous solution of the metal sulfate (MSO4). The solution was boiled to remove all the dissolved CO2 and was then titrated
- A sample of matter must be copper if: a. each atom in the sample has 29 protons b. atoms in the sample react with oxygen c. the sample melts at 1768 K d. the sample can conduct electricity
- Iron(II) Sulfate forms a blue-green hydrate with the formula FeSO4 �n H2O(s). If this hydrate is heated to a high enough temperature, H2O(g) can be driven off, leaving the pale yellow anhydrous salt F
- Addition of common salt in water causes a) increase in M.P of solution. b) increase in B.P of solution. c) decrease in B.P of solution. d) decrease in both M.P & B.P.
- An excess of finely divided iron is stirred up with a solution that contains Cu2+ ions, and the system is allowed to come to equilibrium. The solid materials are then filtered off and electrodes of solid copper and solid iron are inserted into the remaini
- Copper(II) sulfate has been used extensively as a fungicide (kills fungus) and herbicide (kills plants). Copper(II) sulfate can be prepared in the laboratory by reaction of copper(II) oxide with sulfuric acid. f 2.49 g of copper(II) oxide is treated with
- A 2.50 times 10^{-4} M solution of a dye has an absorbance of 0.680 when measured in a 1.00 cm cell at 625 nm. Calculate the % Transmittance of the solution. Will the % Transmittance increase or decrease, if the concentration of the dye is increased?
- To assay silver content in an alloy, a 13.38 g sample of alloy was dissolved in nitric acid. The addition of 0.53 molar sodium chloride resulted in the precipitation of silver chloride. If the alloy w
- A 0.855 g sample of ore of iron is dissolved in acid and converted to Fe(II). The sample is oxidized by 36.50 mL of 0.161 M ceric sulfate, Ce(SO4)2, solution; the cerium(IV) ion, Ce4+, is reduced to Ce3+ ion. What is the percent of iron in the ore?
- A 0.4407 g sample of pewter, (containing tin, lead, copper and zinc) was dissolved in acid, tin was precipitated as SnO2 4H2O and removed by filtration. The resulting filtrate and Washington were dilu
Explore our homework questions and answers library
Browse
by subject