Hi, I'm really having trouble with this set of questions. Please help!
If a current of 733.7 mA is passed through an electrochemical cell for 26.60 minutes, what charge, in coulombs, is passed through the cell?
Charge passed through the cell = _________ coulombs
Suppose that the electrochemical cell consists of two copper electrodes immersed in a copper(II) sulfate solution. At which electrode, anode or cathode, does reduction occur?
The reduction occurs at the __________
Do you expect that this electrode will increase or decrease in mass as the electrolysis proceeds?
The mass of the electrode will ___________
Calculate the change in the mass of copper at the anode or cathode if the charge calculated above is passed through the cell described. Enter your answer as a positive quantity in mg.
Mass change at the electrode = _________ mg
If a current of 733.7 mA is passed through an electrochemical cell for 26.60 minutes, what charge, in coulombs, is passed through the cell?
Charge passed through the cell = _________ coulombs
Suppose that the electrochemical cell consists of two copper electrodes immersed in a copper(II) sulfate solution. At which electrode, anode or cathode, does reduction occur?
The reduction occurs at the __________
Do you expect that this electrode will increase or decrease in mass as the electrolysis proceeds?
The mass of the electrode will ___________
Calculate the change in the mass of copper at the anode or cathode if the charge calculated above is passed through the cell described. Enter your answer as a positive quantity in mg.
Mass change at the electrode = _________ mg
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a. 7337.7mA(1A/1000mA)(26.60min)(60sec/min)… in a. Multiply by molarmass of copper
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okay
ill go through all the steps i took to figure the answer
first one:
Q=IT
I= current in amps
T= time in seconds
Q= what you want (coulombs)charge
so Q= (733.7x100)+(26.60x60)=answer
DIY cuz then only you will learn it
second one is cathode
Remember it as RED CAT (reduction at cathode)
third one is increase
the copper is deposited on the cathode
the fourth one is a bit long but ill brief you as i have to go
first calculate the number of faradays
the number of faradays=number of moles electrons passsed
use the eqn for the reaction find the RAM of copper and then find the number of moles of copper made and find the final answer by using the formulae
moles=mass/molar mass
ill go through all the steps i took to figure the answer
first one:
Q=IT
I= current in amps
T= time in seconds
Q= what you want (coulombs)charge
so Q= (733.7x100)+(26.60x60)=answer
DIY cuz then only you will learn it
second one is cathode
Remember it as RED CAT (reduction at cathode)
third one is increase
the copper is deposited on the cathode
the fourth one is a bit long but ill brief you as i have to go
first calculate the number of faradays
the number of faradays=number of moles electrons passsed
use the eqn for the reaction find the RAM of copper and then find the number of moles of copper made and find the final answer by using the formulae
moles=mass/molar mass