Answer:
Yes
Explanation:
Yes, you can test this by comparing grades you received when you studied and when you did not study
solution,carbonation,hydration,oxidation,and hydrolysis
The amount of aluminum deposited when a current of 10A is passed through a solution of aluminum salt for 1930s is 5.4 g.
An electrochemical cell converts chemical energy into electrical energy. Metals with higher negative electrode potential undergo oxidation and its ionization produces electron flow through the solution.
The weight of the metal that deposited by reduction is related to the mass of metal, current passed and time as follows:
w = z It
where z = E/96500 F
Equivalent mass of Al, E = 27 g
t = 1930 s
current I = 10 A.
Now, the weight of aluminum metal deposited is calculated as follows:
w = 1930 s × 10 A × 27/96500 = 5.4 g.
Therefore, the weight of Al deposited on the electrode is 5.4 g.
Find more on electrochemical cells:
#SPJ2
Answer:
AL*3+ + 3e- =AL.
(10A×1930)÷96500=0.2mole e-
0.2÷3×27=1.8g(AL)