Cu+ + e- ------> Cu
1 mole Cu+ require 96487 C charge
0.800 moles Cu+ require 0.800 x 96487 / 1 = 77189.6 C charge
Charge in C = 77189.6 C
1 mole Cu+ = 6.023 x 1023 electrons
0.800 moles Cu+ = 0.800 x 6.023 x 1023 / 1 = 4.82 x 1023 electrons
number of electrons = 4.82 x 1023 e-
You perform an electrochemical reaction in which 0.800 moles of Cu* are reduced to solid Cu....
2. In this lab, you will use a Zn-Cu electrochemical cell similar to the one shown in Figure 12.1. The overall chemical reaction occurring in this cell is: Zn(s) + Cu2+(ag) → Zn2+(aq) + Cu(s) a. In this reaction, how many electrons are being transferred from one substance to the other? Explain how you can determine this from the reaction shown above. b. Which metal is gaining electrons and which metal is losing electrons? c. Explain the function of a...
50 mL of a 0.050 M solution of Cu2+ was reduced to solid copper. How many coulombs had passed when the Cu2+ was completely reduced to Cu(s)? Use 2 significant figures. Please show all work, thank you!
If 1.123 g strip of Cu is used for the reaction? How many moles of Cu were reacted (Remember to use correct significant figures and show your work) After the reaction, the strip now weighs 1.345 g. How much mass was gained This gain in weight is attributed to that mass of what element? Using the information from above, how many moles of sulfur were reacted? (Remember to use correct significant figures and show your work) What is the difference...
In the following balanced reaction equation, identify which element is being reduced, which element is being oxidised and how many electrons are being transferred in the reaction. 3CH3CH2OH + 2Cr2O7 2− + 16H+ ⇌ 3CH3COOH + 4Cr3+ + 11 H2O (A) Cr reduced, C oxidised, 4 e− transferred (B) C reduced, H oxidised, 3 e− transferred (C) Cr reduced, H oxidised, 4 e− transferred (D) Cr reduced, C oxidised, 12 e− transferred (E) C reduced, Cr oxidised, 16 e− transferred
1. Balance the equation (smallest number of coefficients) for the reaction between iron (II) and permanganate ion. Remember that the equation must balance as to both mass and charge. 2. How many moles of electrons are transferred in the balanced equation? 3. Which species is oxidized? Which species is reduced? 5. What is the indicator for this reaction? Explain.
The cell potential of a redox reaction occurring in an
electrochemical cell under any set of temperature and concentration
conditions can be determined from the standard cell potential of
the cell using the Nernst equation where E is the cell
potential of the cell, E° is the standard cell potential
of the cell, R is the gas constant, T is the
temperature in kelvin, n is the moles of electrons
transferred in the reaction, and Q is the reaction
quotient....
How many coulombs (C) of charge are required to cause reduction of 0.25 mole of Cu2+ to Cu? Hint: 1 mol of electrons = 96500C/mol In the reaction of Cu2+ to Cu,2 moles of electrons are gained 2.4x104C 0.50 € 0.25 14.8× 104C 1.2 x 10°C
a) Find the total amount of charge transferred in Coulombs from a current of 0.338 A in 485 seconds. b) Then, determine how many electrons this amount of charge represents. c) Based on the number of electrons that passes through the wire, determine the number of Copper atoms that moved from the Copper metal to the Zinc. Cu(s) --> Cu2+ (aq) + 2e-. d) Using this information find Avogadro's number. I found the initial mass of the copper to be...
help with 13, 14, 15, 16
the cal l for the product of the y recovering the product by evaporating to comedy mass on we There betw Fal mass of in metal Mass of the evaporating dish watch glass and in chordeer heng simet Mass of zinc chionde formed You know ma sticker for units Show your calculations for the above w e belle 6. Mass of zinc reacted: om Proces 136.28 ondisi tion 0.8545g 7. Mass of zine chlorides....
A-D
A. How many miles of Cu2+ is present in the solution?
B. How many miles of electrons are needed to plate all the
Cu2+?
C. Calculate the coulombs of charge, q required to plate all
Cu2+?
D. How many hours will it take to plate out all the
Cu2+?
B. Electrodeposition A solution of 200.0 mL of a o015 M cu r solution was electrolyzed using a current, i, of 0.200 amp? The half reaction is shown below: 2...