Answered: How many grams of X (MW = 91.45…

How many grams of X (MW = 91.45 g/mol)(in g) will be deposited on a cathode in 1.15 h by a current of 4.0 A? X6+ + 6e- → X(s) Report your answer with the correct number of significant figures.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter17: Electrochemistry And Its Applications

Section: Chapter Questions

Problem 74QRT

See similar textbooks

Related questions

Q: How long must constant current of 50.0 A be passed through an electrolytic cell containing aqueous…

A: According to the first law of Faraday, the mass of a metal deposited on the anode during…

Q: If 10 amp of current is passed through a solution of CaCl2 for 10 minutes in an electrolytic cell,…

Q: How much time in minutes would it take to deposit 1.74 grams of X (MW = 133.98 g/mol) on a cathode…

Q: Calculate the mass in grams of Zn deposited at the cathode in 42.5 minutes when 1.87A of current is…

Q: 3. A technician is plating a faucet with 1.26 g of Cr from an electrolytic bath containing aqueous…

Q: (a) In the electrolysis of aqueous NaCl, how many liters of Cl2(g) (at STP) are generated by a…

A: i = 81.2 A t = 59.2 min

Q: se a current of 770. mA flows through a copper wire for 10.0 minutes. Calculate how many moles of…

Q: A metal object is to be gold-plated by an electrolytic procedure using an aqueous AuCla solution.…

A: Given : Time = 3.0 min = 3.0 X 60 = 180 s (Since 1 min…

Q: What mass of gold can be plated onto an object in 9.18 minutes at 4.91 A of current ? Au^3^+…

Q: How long must a current of 5 amperes (A) be maintained to electroplate 60 g of calcium from the…

Q: A battery can provide a current of 2.20 A at 1.00 V for 8.00 hr. How much energy (in kJ) is…

A: Given information,Battery provides a current 2.20 A at 1.00 V for 8.00 hr.Calculate the power,

Q: A lead storage battery delivers a current of 6 A for one hour and 22 minutes at a voltage of 12 V.…

A: The electrical energy which is generated in the lead storage battery will be equivalent to the…

Q: 10

Q: A common car battery consists of six identical cells each of which carries out the reaction:…

Q: Copper is plated onto the cathode of an electrolytic cell containing CuCl2(aq). How long does it…

Q: ii) How many amperes of current needs to be passed through molten Sodium chloride (NaCl) to produce…

A: NOTE: Since there are no question in part (i), I'm solving the next 3 sub-parts.

Q: a) In the electrolysis of aqueous NaNO2, how many liters of O2(g) (at STP) are generated by a…

A: Given data: Current = 67.8 A = 67.8 C/sec Time = 86.4 min = 86.4 x 60 sec Formula used: q = I x t

Q: ii) How many amperes of current needs to be passed through molten Sodium chloride (NaCl) to produce…

A: Use the first law of Faraday.

Q: Suppose 220. mmol of electrons must be transported from one side of an electrochemical cell to…

A: Given mmol of electrons = 220 Time = 214 s We have to calculate current

Q: A solution of NaCl is neutral, with an expected PH of 7. If electrolysis was carried out on 500 mL…

Q: Electrolysis of an aqueous solution of sodium chloride produces chlorine, Cl2 (9). The reaction that…

Q: Calculate the amount of time it would take to collect 0.750L of hydrogen gas at the cathode of an…

A: Answer = 309 minutes

Q: (Q98) Electrolysis is being used to plate chromium onto a large plastic surface. If a total of 3.77…

A: Given, mass of Chromium (Cr) = 3.77 g Current (I) = ? Time (t) = ? min Note: molar mass of Cr = 52.0…

Q: Zinc metal is deposited onto a cathode surface by passing a current of 1.87 amps through a solution…

Q: What mass of aluminum metal can be produced per hour in the electrolysis of a molten aluminum salt…

A: According to the first law of Faraday, the mass of a metal deposited on the anode during…

Q: Consider an electrolytic cell with a steady voltage of 4.2 V which produces Al(s) (atomic mass =…

A: Given reaction: 2Al2O3 (l) +3C (s) -----> 4Al (s) + 3CO2 (g) Let us break this reaction in terms…

Q: A digital watch battery draws 0.10 milliamperes of current, which is provided by a mercury battery…

A: When a current gets passed in any electrolytic solution, it causes the deposition of chemical at the…

Q: Enter your answer in the provided box. The MnO, used in alkaline batteries can be produced by an…

A: Please find the answer attached here as handwritten note.

Q: If a current is flowing from a battery that's used to electroplate an object with silver, how do I…

A: Given:1.45 A.hr = 1.45 amp current per hour.

Q: 4. In a process called flash electroplating, a current of 2.5 x 10'A passes through an electrolytic…

Q: In an electrolytic cell, silver is deposited at the cathode when a current of 2.75 A is passed for…

Q: 4. What current is required to deposit on the cathode 5.00 g gold/h from a solution containing a…

A: Current = Charge/Time Q = I/t 1F =96500 C/mol Mass of 1 mole =Molar mass

Q: A lead storage battery delivers a current of 6 A for one hour and 22 minutes at a voltage of 12 V.…

A: The discharging reaction if lead storage battery is given as:Pb (s) + PbO2 (s) + 2SO42- (aq) + 4H+→…

Q: (a) In the electrolysis of aqueous Na2O2, how many liters of H2(g) (at STP) are generated by a…

A: The reaction taking place is given as, => Na2O2 (aq) + H2O (l) ↔ H2 (g) + O2 (g) + NaOH (aq)…

Q: How many amperes of current needs to be passed through molten Sodium chloride (NaCl) to produce 2.1…

A: We have given that during the electrolysis of molten Sodium chloride 2.1 g of Sodium is produced at…

Q: Electrolysis of an aqueous solution of sodium chloride produces chlorine, . The reaction that occurs…

A: Give that: the reaction of anode is: 2Cl- (aq) →Cl2 (g) + 2e- Mass of Cl2 produced, w =182 g, time…

Q: An object is electroplated with rhodium for 28.2 minutes at current of 1.4 A. Rh3+ + 3 e Rh Molar…

A: According to Faraday's law of electrolysis, the amount of solid deposited is given by m =…

Q: What current is used to liberate 213 grams of chlorine, Cl 2 from a solution NaCl if it take 2…

A: Faraday's 1st law of electrolysis is one of the most important law which explains that the quantity…

Q: During electrorefining of Cu from CUSO4, how much time (in hours) is needed to produce 250 g Cu on…

A: When a charge Q passes through a circuit the current through that circuit can be calculated by the…

Q: Electroplating is a way to coat a complex metal object with a very thin (and hence inexpensive)…

A: Electroplating is a process of coating layer of metal over another metal by the process of…

Q: Weighing a copper atom in an electrolysis experiment. A standard experiment involves passing a…

A: Electrolysis is the process through which electrical energy is converted into the chemical energy…

Q: If an electrolysis plant operates its electrolytic cells at a total current of 150. A, how long, (in…

A: According to Faraday's First Law of Electrolysis, The amount of product deposited is directly…

Q: 19. (a) Write a balanced equation for the reaction that occurs in a car battery when the ignition…

Q: How long would it take to deposit 7.54 g of copper (molar mass 63.55 g/mol) at the cathode of an…

A: current = 15.9 A (given) Molar mass of copper = 63.55 g/mol (given) Cu is having n factor of 2…

Q: A battery can provide a current of 3.80 A at 3.60 V for 8.00 hr. How much energy (in kJ) is…

A: Given that a current of 3.80 A was provided by battery at 3.60 V. The power can be calculated as…

Q: (a) In the electrolysis of aqueous Naz2C204, how many liters of H2(9) (at STP) are generated by a…

A: The balanced chemical reaction can be written as follows: Na2C2O4 (aq) + 2H2O (l) → 2CO2 (g) + H2…

Q: ow many grams of X (MW = 44.20 g/mol)(in g) will be deposited on a cathode in 1.91 h by a current of…

Q: A digital watch battery draws 0.10 milliamperes of current, which is provided by a mercury battery…

A: m=Mass of Hg=1.10g Equivalent wt of Hg =200.59/2 =100.295 Current = 0.10 mA or 0.10x10-3 F=96500C…

Q: How many grams of copper are deposited on the cathode of an electrolytic cell if an electric current…

A: Faraday's law of electrolysisAsW= Ite/FF= 965900 Ct=20 x 60 sece for copper if taken in copper…

Q: A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 3Cu*…

Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

How many grams of X (MW = 91.45 g/mol)(in g) will be deposited on a cathode in 1.15 h by a current of 4.0 A?

X⁶⁺ + 6e^- → X_(s)

_{Report your answer with the correct number of significant figures.}

Expert Solution

Step 1

Step by step

Solved in 2 steps with 2 images

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

An aqueous solution of an unknown salt of gold is electrolyzed by a current of 2.75 amps for 3.39 hours. The electroplating is carried out with an efficiency of 93.0%, resulting in a deposit of 21.221 g of gold. a How many faradays are required to deposit the gold? b What is the charge on the gold ions (based on your calculations)?
It took 150. s for a current of 1.25 A to plate out 0.109 g of a metal from a solution containing its cations. Show that it is not possible for the cations to have a charge of 1+.
A lead storage battery delivers a current of 6.00 A for one hour and 22 minutes at a voltage of 12.0 V. (a) How many grams of lead are converted to PbSO4? (b) How much electrical energy is produced in kilowatt hours?
Consider the electrolysis of water in the presence of very dilute H2SO4. What species is produced at the anode? Atthe cathode? What are the relative amounts of the speciesproduced at the two electrodes?
An electrolysis experiment is performed to determine the value of the Faraday constant (number of coulombs per mole of electrons). In this experiment, 28.8 g of gold is plated out from a AuCN solution by running an electrolytic cell for two hours with a current of 2.00 A. What is the experimental value obtained for the Faraday Constant?
You have 1.0 M solutions of Al(NO3)3 and AgNO3 along with Al and Ag electrodes to construct a voltaic cell. The salt bridge contains a saturated solution of KCl. Complete the picture associated with this problem by a writing the symbols of the elements and ions in the appropriate areas (both solutions and electrodes). b identifying the anode and cathode. c indicating the direction of electron flow through the external circuit. d indicating the cell potential (assume standard conditions, with no current flowing). e writing the appropriate half-reaction under each of the containers. f indicating the direction of ion flow in the salt bridge. g identifying the species undergoing oxidation and reduction. h writing the balanced overall reaction for the cell.