Time required for Flowing of Charge given Mass and Time Solution

STEP 0: Pre-Calculation Summary
Formula Used
Total Time Taken = Mass of Ions/(Electrochemical Equivalent of Element*Electric Current)
ttot = mion/(Z*ip)
This formula uses 4 Variables
Variables Used
Total Time Taken - (Measured in Second) - Total Time Taken is the total time taken by the body to cover that space.
Mass of Ions - (Measured in Kilogram) - The Mass of Ions is the weight of ions reacted or formed during the electrolysis.
Electrochemical Equivalent of Element - (Measured in Kilogram Per Coulomb) - The electrochemical equivalent of element is the mass of that element (in grams) transported by 1 coulomb of electric charge.
Electric Current - (Measured in Ampere) - Electric Current is the time rate of flow of charge through a cross sectional area.
STEP 1: Convert Input(s) to Base Unit
Mass of Ions: 5.6 Gram --> 0.0056 Kilogram (Check conversion here)
Electrochemical Equivalent of Element: 22 Gram Per Coulomb --> 0.022 Kilogram Per Coulomb (Check conversion here)
Electric Current: 2.2 Ampere --> 2.2 Ampere No Conversion Required
STEP 2: Evaluate Formula
Substituting Input Values in Formula
ttot = mion/(Z*ip) --> 0.0056/(0.022*2.2)
Evaluating ... ...
ttot = 0.115702479338843
STEP 3: Convert Result to Output's Unit
0.115702479338843 Second --> No Conversion Required
FINAL ANSWER
0.115702479338843 0.115702 Second <-- Total Time Taken
(Calculation completed in 00.004 seconds)

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K J Somaiya College of science (K J Somaiya), Mumbai
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25 Electrolytes & Ions Calculators

Valencies of Positive and Negative Ions of Concentration Cell with Transference
Go Valencies of Positive and Negative Ions = ((Transport Number of Anion*Total number of Ions*[R]*Temperature)/(EMF of Cell*Number of Positive and Negative Ions*[Faraday]))*ln(Cathodic Ionic Activity/Anodic Ionic Activity)
Total Number of Ions of Concentration Cell with Transference given Valencies
Go Total number of Ions = ((EMF of Cell*Number of Positive and Negative Ions*Valencies of Positive and Negative Ions*[Faraday])/(Transport Number of Anion*Temperature*[R]))/ln(Cathodic Ionic Activity/Anodic Ionic Activity)
Number of Positive and Negative Ions of Concentration Cell with Transference
Go Number of Positive and Negative Ions = ((Transport Number of Anion*Total number of Ions*[R]*Temperature)/(EMF of Cell*Valencies of Positive and Negative Ions*[Faraday]))*ln(Cathodic Ionic Activity/Anodic Ionic Activity)
Fugacity of Cathodic Electrolyte of Concentration Cell without Transference
Go Cathodic Fugacity = (exp((EMF of Cell*[Faraday])/(2*[R]*Temperature)))*((Anodic Concentration*Anodic Fugacity)/(Cathodic Concentration))
Fugacity of Anodic Electrolyte of Concentration Cell without Transference
Go Anodic Fugacity = ((Cathodic Concentration*Cathodic Fugacity)/Anodic Concentration)/(exp((EMF of Cell*[Faraday])/(2*[R]*Temperature)))
pOH of Salt of Strong Base and Weak Acid
Go Negative Log of Hydroxyl Concentration = 14-(Negative Log of Acid Ionization Constant+Negative Log of Ionic Product of Water+log10(Concentration of Salt))/2
pOH of Salt of Weak Base and Strong Base
Go Negative Log of Hydroxyl Concentration = 14-(Negative Log of Ionic Product of Water-Negative Log of Base Ionization Constant-log10(Concentration of Salt))/2
pH of Salt of Weak Acid and Strong Base
Go Negative Log of Hydronium Concentration = (Negative Log of Ionic Product of Water+Negative Log of Acid Ionization Constant+log10(Concentration of Salt))/2
pH of Salt of Weak Base and Strong Base
Go Negative Log of Hydronium Concentration = (Negative Log of Ionic Product of Water-Negative Log of Base Ionization Constant-log10(Concentration of Salt))/2
pOH of Salt of Weak Acid and Weak Base
Go Negative Log of Hydroxyl Concentration = 14-(Negative Log of Ionic Product of Water+Negative Log of Acid Ionization Constant-Negative Log of Base Ionization Constant)/2
pH of Salt of Weak Acid and Weak base
Go Negative Log of Hydronium Concentration = (Negative Log of Ionic Product of Water+Negative Log of Acid Ionization Constant-Negative Log of Base Ionization Constant)/2
pH Value of Ionic Product of Water
Go Negative Log of H+ Conc. for Ionic Pdt. of H₂O = Negative Log of Acid Ionization Constant+Negative Log of Base Ionization Constant
Time required for Flowing of Charge given Mass and Time
Go Total Time Taken = Mass of Ions/(Electrochemical Equivalent of Element*Electric Current)
Cell Potential given Electrochemical Work
Go Cell Potential = (Work Done/(Moles of Electron Transferred*[Faraday]))
Concentration of Hydronium Ion using pOH
Go Hydronium Ion Concentration = 10^Negative Log of Hydroxyl Concentration*Ionic Product of Water
Ionic Product of Water
Go Ionic Product of Water = Constant of Ionization of Acids*Constant Of Ionization Of Bases
Fugacity of Electrolyte given Activities
Go Fugacity = (sqrt(Ionic Activity))/Actual Concentration
pOH using Concentration of Hydroxide ion
Go Negative Log of Hydroxyl Concentration = 14+log10(Hydronium Ion Concentration)
pH of Water using Concentration
Go Negative Log of Hydronium Concentration = -log10(Hydronium Ion Concentration)
Quantity of Charges given Mass of Substance
Go Charge = Mass of Ions/Electrochemical Equivalent of Element
Relation between pH and pOH
Go Negative Log of Hydronium Concentration = 14-Negative Log of Hydroxyl Concentration
pOH of Strong acid and Strong base
Go Negative Log of Hydroxyl Concentration = Negative Log of Ionic Product of Water/2
Ionic Mobility
Go Ionic Mobility = Speed of Ions/Potential Gradient
Ionic Activity given Molality of Solution
Go Ionic Activity = (Activity Coefficient*Molality)
Concentration of Hydronium ion using pH
Go Hydronium Ion Concentration = 10^(-Negative Log of Hydronium Concentration)

Time required for Flowing of Charge given Mass and Time Formula

Total Time Taken = Mass of Ions/(Electrochemical Equivalent of Element*Electric Current)
ttot = mion/(Z*ip)

What is faraday's first law of electrolysis?

Faraday's first electrolysis Law states that the quantity of reaction taking place in terms of the mass of ions formed or discharged from an electrolyte is proportional to the amount of electric current passed. Since electric current (ampere) is the number of coulombs (Q) flowing in one second.

How to Calculate Time required for Flowing of Charge given Mass and Time?

Time required for Flowing of Charge given Mass and Time calculator uses Total Time Taken = Mass of Ions/(Electrochemical Equivalent of Element*Electric Current) to calculate the Total Time Taken, The Time required for Flowing of Charge given Mass and Time formula is defined as the ratio of the mass of ions formed or reacted to the product of electrochemical equivalent of element and electric current during electrolysis. Total Time Taken is denoted by ttot symbol.

How to calculate Time required for Flowing of Charge given Mass and Time using this online calculator? To use this online calculator for Time required for Flowing of Charge given Mass and Time, enter Mass of Ions (mion), Electrochemical Equivalent of Element (Z) & Electric Current (ip) and hit the calculate button. Here is how the Time required for Flowing of Charge given Mass and Time calculation can be explained with given input values -> 0.115702 = 0.0056/(0.022*2.2).

FAQ

What is Time required for Flowing of Charge given Mass and Time?
The Time required for Flowing of Charge given Mass and Time formula is defined as the ratio of the mass of ions formed or reacted to the product of electrochemical equivalent of element and electric current during electrolysis and is represented as ttot = mion/(Z*ip) or Total Time Taken = Mass of Ions/(Electrochemical Equivalent of Element*Electric Current). The Mass of Ions is the weight of ions reacted or formed during the electrolysis, The electrochemical equivalent of element is the mass of that element (in grams) transported by 1 coulomb of electric charge & Electric Current is the time rate of flow of charge through a cross sectional area.
How to calculate Time required for Flowing of Charge given Mass and Time?
The Time required for Flowing of Charge given Mass and Time formula is defined as the ratio of the mass of ions formed or reacted to the product of electrochemical equivalent of element and electric current during electrolysis is calculated using Total Time Taken = Mass of Ions/(Electrochemical Equivalent of Element*Electric Current). To calculate Time required for Flowing of Charge given Mass and Time, you need Mass of Ions (mion), Electrochemical Equivalent of Element (Z) & Electric Current (ip). With our tool, you need to enter the respective value for Mass of Ions, Electrochemical Equivalent of Element & Electric Current and hit the calculate button. You can also select the units (if any) for Input(s) and the Output as well.
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