Question

Consider the following chemical reactions
(1) ASO4(aq) + B(s) - BSO₂(aq) + A(s)
(ii) BSO4(aq) + D(s) - DSO (aq) + B(s)
(iii) DSO4(aq) + C(s) - CSO4(aq) + D(s)
(iv) CSO4(aq) + A(s) - No reaction

A, B, C and D respectively can be​

Answer 1

Answer:

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Answer 2

Therefore the relation for A, B, C, and D will be A < B < C < D.

Given:

(i) ASO4(aq) + B(s) - BSO₂(aq) + A(s)

(ii) BSO4(aq) + D(s) - DSO (aq) + B(s)

(iii) DSO4(aq) + C(s) - CSO4(aq) + D(s)

(iv) CSO4(aq) + A(s) - No reaction

To Find:

To find a relation for A, B, C, and D

Solution:

These basic Redox reactions can be balanced in this way.

Equation i: ASO4(aq) + B(s) - BSO₂(aq) + A(s)

Since A is displaced by B from its salt solution, A is less reactive than B. ( A < B )

Equation ii: BSO4(aq) + D(s) - DSO (aq) + B(s)

Since B is displaced by C from its salt solution, B is less reactive than C. ( B < C )

Equation iii: DSO4(aq) + C(s) - CSO4(aq) + D(s)

Since C is displaced by D from its salt solution, C is less reactive than D. ( C < D )

Equation iv: CSO4(aq) + A(s) - No reaction

Since D is not displaced B from its salt solution, B is less reactive than D ( B < D ).

Therefore the relation for A, B, C, and D will be A < B < C < D.

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