5. The mass of metal deposited by the electrolysis of an aqueoussolution of metal ions increases in inverse proportion to whichproperty?1. Electrolysis timeII. Metal ion chargeIII. Electrolysis currentO II onlyO III onlyO I and IIO I, II, and III 7. Addition of manganese chloride to a saturated solution of silver (1)chloride causes a/anin mass of precipitate due toincrease, shifting the equilibría towards formation of productsdecrease, shifting the equilibría towards formation of productsincrease, shifting the equilíbria towards formation of reactantsdecrease, shifting the equilibría towards formation of reactants

The mass deposited at electrodes is determined by Faraday's law. And mass deposited is directly…

Answered: n of metal ions increases ty?…

Science

Chemistry

n of metal ions increases ty? Electrolysis time Metal ion charge Electrolysis current mly anly d II and III

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: Part A What mass of Ni+ is produced in solution by passing a current of 67.0 A for a period of 14.0…

Q: O The utandard reduction potential qor sn 24 and Ay 3t are -0.14 and † 1.50 V reupectively. Ca…

A: Given: ESn2+|Sno=-0.14 VEAu3+|Auo=+1.50 V

Q: How these electrons move in forming and breaking bonds, and if a reaction proceeds via a radical or…

A: The formation of a bond takes place by either sharing of electrons or by complete transfer of…

Q: An aqueous solution of nickel acetate is electrolyzed for 3 hours with a 1.9 ampere current. What…

Q: 26.) The standard reduction potential of A is 2.5 V and that of B is -0.63 V thus A reduced by B.…

A: In this question we have to tell that the given statement is True or False.

Q: None

A: First, you need to find the molar mass of manganese. The molar mass of manganese (Mn) is…

Q: How long will it take to plate out each of the following with a current of 200.0 Ampere? a. 1.0 kg…

A: The given current, I = 200.0 Ampere. Known, I = Qt Here, I = The current in Ampere. t = The…

Q: Which of the following is true for an electrolytic cell? a. G > 0 ; E 0 c. G 0 ; E > 0

A: An electrolytic cell is an electrochemical cell that uses electrical energy to run a non-spontaneous…

Q: Consider the following reaction: COCI2 (2) = CO + Cl2 (g) Keg = 8.33 x 10-4 (8) The reaction vessel…

Q: cator=assighment-lake [Review Topics] [References] CHEMWORK An electrolytic cell is set up to plate…

A: Introduction: As we know that the Michael Faraday described the quantitative aspects of Electrolysis…

Q: time re

Q: How many Seconds are reQuircd to deposst o.2859 Or Cadmium metal from a Solutior that Contams cazt…

A: By Faradays law of electrolysis; W/E = It/F where, W = mass of substance deposited E = equivalent…

Q: What amount of Cu (in grams) is deposited at the cathode when a current of 6 A is maintained for 15…

Q: 29

A: We have given that How much time (in hours) is required to produce 2.20 kg of Zn(s) from a solution…

Q: A current of 3.86 A is passed through a Pb(NO,), solution for 1.60 h. How much lead is plated out of…

A: Faraday law of electrolysis states that the amount of substance deposited at the electrode is…

Q: help please answer in text form with proper workings and explanation for each and every part and…

A: Step 1: Step 2: Step 3: Step 4:

Q: How many grams of chromium metal will be deposited from a solution that contains Cr* ions if a…

A: Given :- Current = 0.957A Time = 47.9 minutes

Q: - many grams of lead metal will be deposited from a solution that contains Pb2+ ions if grams ubmit…

A: The questions based on Faraday's first law of electrolysis. it states that mass of an element…

Q: A current of 3.36 A is passed through a Sn(NO,), solution. How long, in hours, would this current…

A: 1F of charge can precipitate 1 eqv weight of the particular atom .

Q: How many grams of zinc metal will be deposited from a solution that contains Zn2* ions if a current…

A: Given,

Q: A current of 3.75 A is passed through a Sn(NO,), solution. How long, in hours, would this current…

A: Required time calculation for Electrolysis:

Q: Complete and balance the following half-reaction in basic solution. Be sure to include the proper…

A: We know in a balanced chemical equation there is conservation of mass , number of atoms and charges…

Q: Values if needed for this question. How many grams of mercury metal will be deposited from a…

A: Approximately 1.90 grams of Hg deposited

Q: calculate the degree of dissociation of MCl2 salt in 0.065M solution, if the electrode potential of…

A: Concentration of MgCl2 = 0.065M Electrode potential of metal (Ecell) = -0.8V Standard electrode…

Q: A tub of water containing Cu²⁺(aq) is subjected to a current of 0.3 amperes for 30 minutes. How many…

A: Faraday's law of electrolysis states that the mass of metal produced or deposited at electrode is…

Q: Balance the half-reaction in basic solution. Use e as the symbol for an electron. half-reaction: SO

A: Balanced Reaction is given below

Q: Draw galvanic cells based on the net L for the follow equoions irg reochas. to -> fea)

A: The given cell reaction = Fe (s) + Sn2+(aq.) →Fe2+(aq.) + Sn (s)

Q: The electrolysis of molten AIClz for 4.25 hr with an electrical current of 25.0 A produces g of…

A: The amount of Aluminum produced can be calculated as follows

Q: what electrochemical reaction uses in AA alkaline battery

A: ANSWER IS DISCUSSED BELOW :

Q: A current of 4.46 A is passed through a Pb(NO,), solution for 1.30 h. How much lead is plated out of…

Q: A current of 4.26 A is passed through a Fe(NO,), solution. How long, in hours, would this current…

A: Applying Faraday law W= Zit

Q: What mass of Al

Q: Check Your Understanding Suppose that a machine part requires 400 mg of copper to pro- vide a…

A: Solution: Electroplating is a method of coating one metal onto the other with the help of an…

Q: Consider an electrochemical cell based on the following cell diagram ven that the standerd cell emf…

Q: A current of 5.47 A is passed through a Fe(NO,), solution for 1.70 h. How much iron is plated out of…

A: The question is based on the concept of electrolysis. it involves Faraday's first law which states…

Q: How many grams of iron metal will be deposited from a solution that contains Fe* ions if a current…

Q: An electrode Is prepared fromm liquid mercury in contct willh a salurated solution o mercury(1)…

A: The standard reduction potentials of half- cell reactions are, The most positive standard reduction…

Q: What current is required to plate 1.75 g of chromium from a chromium(II) nitrate solution in 4.70…

A: Mass of Chromium = 1.75 g Atomic Mass of Chromium = 52 g mol-1 Time, t = 4.70 hr = 4.70…

Q: Which statement about a voltaic cell is not correct? O The cell voltage measured with a voltmeter is…

A: Here we have to predict the incorrect statements from the following given statements for a Galvanic…

Q: Indicate which one of the metals should be the anode in all reactions. Choose one: O Al(s) O Ni(si O…

A: A question based on electrode potential. 5 options of metal are given from that the most appropriate…

Q: the electrolysis of molten alcl3 for 1.00 gr with an electronical current of 12.0 A produce _____ g…

Q: How many seconds are required to deposit 0.164 grams of magnesium metal from a solution that…

Q: A student does an experiment to determine the molar solubility of lead lodide. She constructs a…

A: Concentration of lead nitrate = 0.698 M Cell potential 8.23×10-2 V

Question

5. The mass of metal deposited by the electrolysis of an aqueous
solution of metal ions increases in inverse proportion to which
property?
1. Electrolysis time
II. Metal ion charge
III. Electrolysis current
O II only
O III only
O I and II
O I, II, and III

7. Addition of manganese chloride to a saturated solution of silver (1)
chloride causes a/an
in mass of precipitate due to
increase, shifting the equilibría towards formation of products
decrease, shifting the equilibría towards formation of products
increase, shifting the equilíbria towards formation of reactants
decrease, shifting the equilibría towards formation of reactants

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 by step

Solved in 2 steps

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

The standard reduction potential of A is 2.5 V and that of B is -0.63 V thus A reduced by B. TRUE OR FALSE
What current in ampere will be required to produce 2.369 x10-3 kg of cu from CuS04 solution in one hour? (Molar mass of Cu = 63.5g/mole) Tuno vour Answer bere
complete solution no need explanation Determine the molar mass (amu) of Metal (M) if it took 2.61 minutes for a current of 1.72 A to plate 0.0595 g of metal from a solution containing M2(SO4)3. (Round off the final answer to TWO decimal places. Do not include the unit.)
16. How many grams of Cu are plated out from a CUSO4 solution by a current of 10.0 amps flowing for 15.0 minutes? (1 amp=1C/second)
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential 2 H,O(1)+2e H,(9)+2ОН (аq) E red -0.83 V Cu"(aq)+e 2+ - Cu (aq) End=+0.153 V red Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.
What is the equation to determine cell voltages using standard reduction potential? 2. What are the steps to balance redox equations under acidic conditions?
E:19 The electrode potential of a metal is: a) The potential which exists at the interface between the metal and the electrolyte b) The potential between the anodic and cathodic areas of the metal c) The potential between two metals immersed completely in the same electrolyte d) The potential of a metal with respect to another metal, which is at a higher concentration
3.
See image below. To solve this, do we use Faraday's constant?
I need hand written solution only
Metal ENGGMATH GMATH ENGGCHEM GRVA FIT HW What metal is used as the cathode in the experiment? O FIT HW OGMATH O ENGGCHEM O ENGGMATH GRVA Average Voltage 0.21 0 0.56 0.98 0.76
How many minutes would it take to deposit all the Al from 225 ml of 0.10 M aluminum nitrate with a current of 220 amperes