Posted by hriday on Thursday, February 19, 2009 at 6:58pm.
amperes x seconds = coulombs
coulombs/96,485 = Faraday's
1 Faraday will deposit 1 equivalent weight of Zn^+2 or 1/2 mole Zn^+2.
I get 0.965 x 10 min x (60 sec/min) = ?? coulombs.
That divided by 96,485 = 0.006 Faraday's and that will deposit 0.003 mole Zn^+2.
How many moles Zn^+2 in 500 mL 0.2 M ZnSO4. M x L = 0.2 x 0.50 = 0.1 mol
0.003 is deposited. How much is left. What is the molarity of that solution?
Related Questions
chemistry - A current of 0.965 A is passed through 500 ml of 0.2 M solution of ...
chemistry - a current is passed through 500 mL of a solution of CaI2. the ...
chemistry - A STUDENT STUDYING THE FE+3- HSCN equilibrium put into a test tube ...
chemistry - Calculate the molarity of a solution prepared by diluting 200.0 mL ...
CHEMISTRY - A STUDENT STUDYING THE FE+3- HSCN equilibrium put into a test tube ...
11th grade ..CHEMISTRY - This is a Quantitative Redox titration. (KMnO4) = 1.8 G...
Chemistry - If 1.0 mL of 6.0M HCl is added to 499 mL of water to give exactly a ...
chemistry - 6.67 mL of 18.0 molar sulfuric acid solution was dissolved in enough...
Chem - How many grams of Ni would be electroplated if a constant current of 7.2 ...
science - 50 ml of ZnSO4 solution was transferred to a mercury cathode and ...
For Further Reading
