Question

For the reaction...
$ΔG > 0$

But, the reaction is REVERSIBLE ONE!

Then, what is the correct option??​

Answer 1

Answer:

non feasible

for feasibility∆g<0

E>0

Answer 2

Question :

∆H, ∆S & T of a reaction are 40.63kJ/mol and 108.8J/k/mol and 373.4 K respectively. Predict the feasibility of the reaction

$\Large\bold{\underline{\underline{Answer:-}}}$

$\Large\bold{\boxed{\boxed{c) Remains\:at\:equilibrium}}}$

$\rule{200}{4}$

$\bf\small\bold{\underline{\underline{Step-By-Step\:Explanation:-}}}$

We know that

∆G = ∆H - T∆S

$\tt{\Rightarrow\triangle \:G = 40.63 - \frac{108.8\times \:373.4} {1000} }$

$\tt{\Rightarrow\triangle \:G = 40.63 - 40.63}$

$\tt{\Rightarrow\triangle \:G = 0 }$

Hence the reaction will remains at equilibrium