What mass of copper in gram would be deposited by a current of 1.00ampere passing for 965 seconds through copper(II) tertraoxosulphate (VI) solution? [Cu 63.5; If = 96500c]
0.32
0.64
3.18
6.35
9.65
Explanation
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The answer should be
Q=It
Q=965×1=965
If
96500=63.5
965=x
Cross multiply
x={965×63.5}/96500
x=0.635~0.64
The answer should be
Q=It
Q=965×1=965
If
96500=63.5
965=x
Cross multiply
x={965×63.5}/96500
x=0.635~0.64
96,500C is required to discharge 1 mol of a univalent element e.g H+, Li+, Na+ e.t.c
2(96500C) is required to discharge 1 mol of a divalent element e.g Cu²+, O²+
NOTE : Copper can either be monovalent or divalent. (Inorganic copper is divalent copper, or copper-2, while we now know that organic copper, or copper in foods, is primarily monovalent copper, or copper-1)
Therefore, in this case, we make use of Copper (2)
Therefore,
2×96,500C = 1 mol of Cu (63.5)
To find the mol of Cu, we must find the quantity of charge (C) required for it.
Therefore, Q=IT
= 965 × 1
Therefore, since 2×96,500C = 63.5
965C = X
= 193,000X = 61,277.5
X= 61,277.5/193,000
X= 0.32
