Hydrolysis of sucrose is given by the following reaction. Sucrose + H _ 2 O Glucose +…
Chemistry · NEET · NTA Exams — Chemical Thermodynamics
Hydrolysis of sucrose is given by the following reaction.
Sucrose \(+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons\) Glucose + Fructose
If the equilibrium constant (KC) is \(2 \times 10^{13}\) at 300 K, the value of \(\Delta_{r} \sigma^{\ominus}\) at the same temperature will be:
- \(-8.314 \downharpoonleft \mathrm{~mol}^{-1} \mathrm{~K}^{-1} \times 300 \mathrm{~K} \times \ln \left(2 \times 10^{13}\right)\)
- \(8.314 \downharpoonleft \mathrm{~mol}^{-1} \mathrm{~K}^{-1} \times 300 \mathrm{~K} \times \ln \left(2 \times 10^{13}\right)\)
- \(8.314 \downharpoonleft \mathrm{~mol}^{-1} \mathrm{~K}^{-1} \times 300 \mathrm{~K} \times \ln \left(3 \times 10^{13}\right)\)
- \(-8.314 \downharpoonleft \mathrm{~mol}^{-1} \mathrm{~K}^{-1} \times 300 \mathrm{~K} \times \ln \left(4 \times 10^{13}\right)\)
Answer
(A) -8.314 ~mol ^ -1 ~K ^ -1 300 ~K (2 10^ 13 )
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