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Using the Gibbs energy change, Delta G^(...

Using the Gibbs energy change, `Delta G^(@)=+ 63.3 kJ`, for the following reaction,
`Ag_(2)CO_(3)hArr2Ag^(+)(aq)+CO_(3)^(2-)`
the `K_(sp)` of `Ag_(2)CO_(3)(s)` in water at `25^(@)C` is
`(R=8.314 JK^(-1)mol^(-1))`

A

`3.2xx10^(-26)`

B

`8.0xx10^(-12)`

C

`2.9xx10^(-3)`

D

`7.9xx10^(-2)`

Text Solution

Verified by Experts

The correct Answer is:
B
`DeltaG^@` is related to `K_sp` by the equation. `DeltaG^@=-2.303"RT log "K_sp`
Given, `Deltag^@=+63.3kJ`
`=63.3xx10^3J`
Thus, substance `DletaG^@=63.3xx10^3J`.
`R=8.314JK^(-1)mol^(-1)` and `T=298K[25+273K]` from the above equation we get, `63.3xx10^3=--2.303xx8.314xx298logK_sp`
`therefore" "log K_sp=-11.09`
`rArrK_sp ="anti log "(-11.09)`
`K_sp=8.0xx10^(-12)`
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