Hydrolysis of sucrose is given by the following reaction. Sucrose + H20 leftharpoons Glucose + Fructose If the equilibrium constant (Kc) is 2 × 1013 at 300K, the value of Δr G ominus at the same temperature will be :

Question

Hydrolysis of sucrose is given by the following reaction. Sucrose + H20 leftharpoons Glucose + Fructose If the equilibrium constant (Kc) is 2 × 1013 at 300K, the value of Δr G ominus at the same temperature will be : (A) -8.314 Jmol-1K-1 × 300 K × ln (2×1013) (B) 8.314 mol-1K-1 × 300 K × ln (2 × 1013) (C) 8.314 J mol-1 300 K × ln(3 × 1013) (D) -8.314 J mol-1 K-1 × 300 K × In(4 × 1013)

Tardigrade Admin · Accepted Answer

Δ G° = -RT ln KC Δ G° = -8.314 × 300 ln ( 2 × 1013)

Q. Hydrolysis of sucrose is given by the following reaction. $S u crose + H_{2} 0 ⇌ Gl u cose + F r u c t ose$
If the equilibrium constant $(K_{c})$ is $2 \times 1 0^{13}$ at 300K, the value of $Δ_{r}$ $G^{⊖}$ at the same temperature will be :

$- 8.314 J m o l^{- 1} K^{- 1} \times 300 K \times l n (2 \times 1 0^{13})$

$8.314 m o l^{- 1} K^{- 1} \times 300 K \times l n (2 \times 1 0^{13})$

$8.314 J m o l^{- 1} 300 K \times l n (3 \times 1 0^{13})$

$- 8.314 J m o l^{- 1} K^{- 1} \times 300 K \times I n (4 \times 1 0^{13})$

$Δ G^{\circ} = - RT l n K_{C}$
$Δ G^{\circ} = - 8.314 \times 300 l n (2 \times 1 0^{13})$

Q. Hydrolysis of sucrose is given by the following reaction. Sucrose+H2​0⇌Glucose+Fructose If the equilibrium constant (Kc​) is 2×1013 at 300K, the value of Δr​ G⊖ at the same temperature will be :

−8.314Jmol−1K−1×300K×ln(2×1013)

8.314mol−1K−1×300K×ln(2×1013)

8.314Jmol−1300K×ln(3×1013)

−8.314Jmol−1K−1×300K×In(4×1013)