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Consider the reaction Pb O (s) + CO (g) ...

Consider the reaction `Pb O (s) + CO (g) + CO_(2) (g)`,
`Delta_(r)H^(@) = - 65.69 kJ mol^(-1)`. If `Delta_(f) H^(@)` for `CO_(2)` and `CO (g)` are `393.5 kJ mol^(-1)` and `- 110.5 k J mol^(-1)`, respectively, calculate `Delta_(f) H^(@)` for yellow `PbO (s)`

A

`+ 217.3 k J mol^(-1)`

B

`- 317.2 k J mol^(-1)`

C

`+ 317.2 k J mol^(-1)`

D

`- 217.3 k J mol^(-1)`

Text Solution

Verified by Experts

The correct Answer is:
D
According to the mathematical form of Hess's law. We have
`Delta_(r) H^(@) = sum_(i) a_(i) Delta_(f) H^(@)` (products) `- sum_(i) b_(i) Delta_(f) H^(@)` (reactants)
`Delta_(r) H^(@) = [Delta_(r) H^(@) (Pb,s) + Delta_(f) H^(@) (CO_(2), g)]`
`-[Delta_(f) H^(@) (PbO,s) + Delta_(f) H^(@) (CO,g)]`
`implies - 35.69 kJ mol^(-1) = [0 + (-393.5 kJ mol^(-1))]`
`- [(Delta_(f) H^(@) (PbO,s) + (- 110.5 kJ mol^(-1)]`
Rearranging ot solve for `Delta_(f) H^(@) (PbO, s)`, we have
`Delta_(f) H^(@) (PbO,s) = (65.69 - 393.5 + 110.5) kJ mol^(-1)`
` = 217.3 kJ mol^(-1)`
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