What mass of copper is deposited when 6.5g of granulated zinc reacts with excess copper(II) tetraoxosulphate(VI) solution?
The equation for the reaction is: Zn(s) + \( CuSO_4(aq)→ ZnSO_4(aq)+ Cu(s)\)[CU= 64; Zn=65]
3.2 g
3.25 g
6.4 g
6.5 g
64.0 g
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According to Faraday'S second law of electrolysis
mole=k/charge
k=m×c
m1c1=m2c2
1=cu 2=Zn m of Zn=6.5÷65=0.1
m1=m2c2/c1
0.1×2/2
m1=0.1
since answers were given in gram
Cu=0.1×64=6.4
6.4 is the final answer
To the look of this question, it is faraday second law question. And to solve it you have to note this, If more than one element or compound are mentioned with the same quantity of electricity pls note it is second law, although first law is different. So if you have noted that, to solve it the formula is (there are many formulas but am just going to bring this one to solve the question) m(mass)×q(charge)/Mm(molar mass)=m(mass)×q(charge)/Mm(molar mass) pls note the first element called is the one to take the first formula which is (mass×charge/molar mass) and the first element called was copper and the charge for copper is (+2), Zn (+2). Pls read the procedure you will be able to solve it and you will understand it better. Although I can still use first law to solve it but it will be a little bit complicated.
What mass of copper deposited when 6.5g of granulated zinc react with excess copper (II) tetraoxosulphate (V) solution?
