NEET 2020 Chemistry - Class 11 NEET-2020-Ch-660 Solution: Hydrolysis of sucrose is given by the following reaction.…

QNEET-2020-Ch-660: NEET 2020 Chemistry - Class 11 NEET-2020-Ch-660 Solution: Hydrolysis of sucrose is given by the following reaction.…

Hydrolysis of sucrose is given by the following reaction. Sucrose +

H_2O

\rightleftharpoons

Glucose + Fructose If the equilibrium constant (

K_c

) is

2 \times 10^{13}

at 800 K the value of

\Delta_r G^\circ

at the same temperature will be:

8.314\ \text{J mol}^{-1}\ \text{K}^{-1} \times 300\text{K} \times \ln(2 \times 10^{13})

8.314\ \text{J mol}^{-1}\ \text{K}^{-1} \times 300\text{K} \times \ln(3 \times 10^{13})

-8.314\ \text{J mol}^{-1}\ \text{K}^{-1} \times 300\text{K} \times \ln(4 \times 10^{13})

-8.314\ \text{J mol}^{-1}\ \text{K}^{-1} \times 300\text{K} \times \ln(2 \times 10^{13})

A 8.314 J $mo{l^{ - 1}}{K^{ - 1}} \times 300K \times In(2 \times {10^{13}})$ m o l _ 1 K _ 1 _ 300 K _ I n ( 2 _ 1 0 13 )
B 8.314 J $mo{l^{ - 1}}{K^{ - 1}} \times 300K \times In(3 \times {10^{13}})$ m o l _ 1 K _ 1 _ 300 K _ I n ( 3 _ 1 0 13 )
C $-$ _ 8.314 J $mo{l^{ - 1}}{K^{ - 1}} \times 300K \times In(4 \times {10^{13}})$ m o l _ 1 K _ 1 _ 300 K _ I n ( 4 _ 1 0 13 )
D -8.314 J $mo{l^{ - 1}}{K^{ - 1}} \times 300K \times In(2 \times {10^{13}})$ m o l _ 1 K _ 1 _ 300 K _ I n ( 2 _ 1 0 13 )

Step-by-Step Verified Solution

_ G = _ G _ + RT ln Q At equilibrium _ G = 0, Q = K eq So, _ r G _ = _ RT in K eq _ r G _ = _ 8.314 J mol -1 K -1 _ 300K _ ln (2 _ 10 13 )