sucrose change of H is -2226.1kj/mol
fructose change of H is -1265.6KJ/mol
calculate the enthalpy change for the hydrolysis reaction of sucrose.
sucrose + H2O(l)-> C6H12O6(s)+Fructose
Is it just the products-reactants?? I'm confused.
Yes, that's what it is. Don't forget to include the liquid H2O in the reactants.
I'm not really sure what liquid H20 kj/mol is?
To calculate the enthalpy change for the hydrolysis reaction of sucrose, you should consider the difference in enthalpy between the products and reactants.
The balanced chemical equation for the hydrolysis reaction of sucrose is:
sucrose + H2O(l) → C6H12O6(s) + fructose
From the information given, we can see that the change in enthalpy for the hydrolysis of sucrose is ΔH = -2226.1 kJ/mol. This means that 2226.1 kJ of energy is released during the reaction.
To calculate the enthalpy change for the reaction, you need to consider the enthalpies of the products and subtract the enthalpies of the reactants. Since the reaction involves the formation of fructose, we also need to consider the change in enthalpy for fructose.
The enthalpy change for the hydrolysis of sucrose can be calculated as follows:
ΔH = ΔH_products - ΔH_reactants
ΔH = (ΔH_f for C6H12O6) + (ΔH_f for fructose) - (ΔH_f for sucrose) - (ΔH_f for H2O)
Given that ΔH_f for C6H12O6 (s) is 0 kJ/mol and ΔH_f for fructose is -1265.6 kJ/mol, the equation becomes:
ΔH = (0) + (-1265.6 kJ/mol) - (ΔH_f for sucrose) - (ΔH_f for H2O)
By substituting the known values, we have:
ΔH = -1265.6 kJ/mol - ΔH_f for sucrose - (ΔH_f for H2O)
Please note that the enthalpies of formation for sucrose and H2O are required to calculate the enthalpy change accurately.
To calculate the enthalpy change for a reaction, you need to consider the difference in enthalpy between the products and the reactants. This can be determined using Hess's Law, which states that the enthalpy change for a reaction can be calculated by considering the enthalpy changes of other reactions that can be combined to give the overall reaction.
Let's break down the reaction into two steps:
1. Sucrose (C12H22O11) hydrolysis:
Sucrose + H2O(l) → Glucose (C6H12O6) + Fructose
Here, glucose is one of the products, and fructose is the other product.
2. Glucose isomerization:
Glucose ↔ Fructose
In this step, glucose converts to fructose, and vice versa.
To calculate the enthalpy change for the hydrolysis reaction of sucrose, we need to sum up the enthalpy changes for the two steps mentioned above.
Step 1: Sucrose hydrolysis
The enthalpy change for this reaction can be determined by considering the enthalpy changes of the products (glucose and fructose) and reactants (sucrose and water).
Enthalpy change for sucrose hydrolysis = (Enthalpy of glucose + Enthalpy of fructose) - (Enthalpy of sucrose + Enthalpy of water)
Given:
Enthalpy of glucose = 0 kJ/mol
Enthalpy of fructose = -1265.6 kJ/mol
Enthalpy of sucrose = 0 kJ/mol (Not provided, assuming the enthalpy of sucrose is 0)
Enthalpy of water = 0 kJ/mol (Not provided, assuming the enthalpy of water is 0)
Enthalpy change for sucrose hydrolysis = (0 kJ/mol + (-1265.6 kJ/mol)) - (0 kJ/mol + 0 kJ/mol) = -1265.6 kJ/mol
Therefore, the enthalpy change for the hydrolysis reaction of sucrose is -1265.6 kJ/mol.