Chemistry, asked by salmaz7907, 1 year ago

For a given reaction, \Delta H = 35.5 kJ mol⁻¹ and DS = 83.6 JK⁻¹ mol⁻¹. The reaction is spontaneous at : (Assume that \Delta H and \Delta S do not vary with tempearature)
(a) T > 425 K
(b) All temperatures
(c) T > 298 K
(d) T < 425 K

Answers

Answered by anchalyadav32
29

Explanation:

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Answered by kobenhavn
13

Answer: (a) T > 425 K

Explanation:

According to Gibb's equation:

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

\Delta G = Gibbs free energy  

\Delta H = enthalpy change  = 35.5 kJ/mol = 35500 J/mol

\Delta S = entropy change  =  83.6 J/Kmol

T = temperature in Kelvin

\Delta G= +ve, reaction is non spontaneous

\Delta G= -ve, reaction is spontaneous

\Delta G= 0, reaction is in equilibrium

\Delta G=(+ve)-T(+ve)

\Delta G=(+ve)(-ve)=-ve  

when T\times \Delta S> \Delta H

Thus T\times 83.6J/Kmol&gt;35500J/mol

T&gt;425Kl

Thus reaction is spontaneous at temperatures greater than 425 Kelvin

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