Given
`E_(Ag^(+)//Ag)^(@)=0.80V`, `E_(Mg^(2+)//Mg)^(@)=-2.37V`,
`E_(Cu^(2+)//Cu)^(@)=0.79 E_(Hg^(2+)//Hg)^(@)=1.71V`
Which of the following statements is/are correct?

Options

A. `AgNO_(3)` can be stored in copper vessel
B. `CU(NO_(3))_(2)` can be stored in copper vessel magnesium vessel
C. `CUCl_(2)` can be stored in silver vessel
D. `Hg_(2)Cl_(2)` can be stored in copper vessel

Answer

A

Explanation

Check `E_(cell)^(@)`. If `E_(cell)^(@) > o` then the reaction is spontaneous.
(A) `E_(cell)^(@) = 0.8 - 0.34 = 0.46V (2Ag^(+) Cu rightarrow 2Ag + CU^(2))`
(B)`E_(cell)^(@) = 0.34 -(-2.37) = 2.81V (CU^(2+) + Mg rightarrow Cu+ Mg rightarrow CU+ Mg^2+)`
(C) `E_(cell))^(@) = 0.34 - 0.8 =- 0.46V (CU^(2+) 2Ag rightarrow Cu + Cu+ 2A^(+))`
(D) `E_(cell)^(@) = 0.79 - 0.34 = 0.45 V (Hg^(2+)) + Cu rightarrow (Cu^(2+) + Hg)`
In (A), (B) and(E) , `E_(cell)^(@)> 0` Which means that the respective solution in the respective vessel cannot be stored.