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The reaction,

$MgO(s)+ C(s)\rightarrow Mg(s)+CO(g)$ , for which $\Delta _{r}H^{o}= + 491.1$ kJ mol^-1 and $\Delta _{r}S^{o}= 198.0 \: JK^{-1}$ mol^-1 , is not feasible at 298 K. Temperature above which reaction will be feasible is :
Option 1)
2380.5 K
Option 2)
2480.3 K
Option 3)
2040.5 K
Option 4)
1890.0 K

Answers (1)

best_answer

ΔG{reaction} -

$\Delta G _{reaction }= \sum \Delta G_{product}- \sum \Delta G_{reactant}$

- wherein

$\sum \Delta G_{product}=$ Sum of $\Delta G$ of all product

$\sum \Delta G_{reactant}=$ Sum of $\Delta G$ of all reactant

Gibb's free energy (Δ G) -

$\Delta G= \Delta H-T \Delta S$

- wherein

$\Delta G=$ Gibb's free energy

$\Delta H=$ enthalpy of reaction

$\Delta S=$ entropy

$T=$ temperature

Spontanous process -

$\Delta G=\Delta H-T\Delta S$

- wherein

For spontanouse process $\Delta G$ must be negative.

$\Delta H-T\Delta S<O$

$T>\frac{\Delta H}{\Delta S}$

$T>\frac{491.1\times 1000}{198}$

$T>2480.3 K$

Option 1)

2380.5 K

Option 2)
2480.3 K
Option 3)

2040.5 K

Option 4)

1890.0 K

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