Calculate the standard cell potentials of galvanic cell in which the following reactions take place: (i) 2Cr(s) + 3Cd²⁺(aq) -> 2Cr³⁺(aq) + 3Cd (ii) Fe²⁺(aq) + Ag⁺(aq) -> Fe³⁺(aq) + Ag(s) Calculate the ΔᵣG and equilibrium constant of the reactions.
Answers
Galvanic cell of reaction: Cr(s) | Cr3+|| Cd2+ | Cd ( s): The formula of standerd cell potential is:
E0CELL = E0Right -E0left: E0Cell – E9Cd-R0Cr:E0cell = -0.40 –(-0.074)=+0.43 v:In balance reaction, 6 electrons are transferring.
So, n=6:Faraday constant ,F= 96500 C mol-1E0CELL=+0.34 v:
Use the formula :Ϫ rGϴ=nFE cell plugging the values we get:=-6x96500 C mol-1x0.34 V=-196860 CV mol-1: Again using second formula.
Ϫ rGϴ=-2.303RT log kc log kc =34.54taking antilog both sides: kc =3.192x1034
Ionic solids are hard and brittle. Answer: ... That is why both metals and ionic compounds are good conductors of electricity and have high melting points. The basis of difference is the absence of mobility of ions in the ionic crystals while the same is present in the valence electrons in case of metallic crystals.
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