Answer: Reaction A: pi + glucose ⇒ glucose-6-phosphate + H2O ΔG = 13.8 kJ/mol
Reaction B: pi + frutose-6-phosphate ⇒fructose-1,6-biphosphate + H2O ΔG = 16.3kJ/mol
Explanation: ΔG is the representation of the change in Gibbs Free Energy and relates enthalpy and entropy in a single value, which is:
ΔG = ΔH - TΔS
where:
ΔH is enthalpy
T is temperature
ΔS is entropy (measure of the )
It can also predict the direction of the reaction with the conditions of temperature and pressure being constant.
When the change is positive, the reaction is non-spontaneous, which means the reaction needs external energy to occur. If the change is negative, it is spontaneous, i.e., happens without external help.
Analyzing the reaction, we see that reaction A and B have a positive ΔG, while reaction C is negative, so the reaction that are unfavorable or nonspontaneous are <u>reactions A and B</u>.
Explanation:
In sugar solution 200 g has sugar 10 g
In sugar solution 100 g has sugar 10/200 × 100
= 5 %w/w
