Answer : The value of standard free energy is, -152.4 kJ/mol
Explanation :
The given balanced cell reaction is:
The half reaction will be:
Reaction at anode (oxidation) :
Reaction at cathode (reduction) :
First we have to calculate the standard electrode potential of the cell.
Relationship between standard Gibbs free energy and standard electrode potential follows:
where,
= standard free energy = ?
n = number of electrons transferred = 2
F = Faraday constant =
= standard electrode potential of the cell = 0.79 V
Now put all the given values in the above formula, we get:
Therefore, the value of standard free energy is, -152.4 kJ/mol
Answer : The enthalpy for the reaction is 49.1 kJ/mol
Explanation :
According to Hess’s law of constant heat summation, the heat absorbed or evolved in a given chemical equation is the same whether the process occurs in one step or several steps.
According to this law, the chemical equation can be treated as ordinary algebraic expression and can be added or subtracted to yield the required equation. That means the enthalpy change of the overall reaction is the sum of the enthalpy changes of the intermediate reactions.
The formation reaction of will be,
The intermediate balanced chemical reaction will be,
(1)
(2)
(3)
Now we will reverse the reaction 1 and divide by 2, multiply reaction 2 by 6 and reaction 3 by 3/2 then adding all the equations, we get :
(1)
(2)
(3)
The expression for enthalpy of formation of will be,
Therefore, the enthalpy for the reaction is 49.1 kJ/mol
Answer:
C) 2H2SO4(aq)+ 2Ba(OH)2(aq)---->2BaSO4(s)+4H2O(I)
Explanation:
The reaction proper:
2H₂SO₄ + 2Ba(OH)₂ → 2BaSO₄ + 4H₂O
The above reactions is a typical acid-base neutralization reaction.
A reaction in which oxidation-reduction did not take place is called a non-redox reaction. In such a reaction, there is no transfer of electrons between reactants, that is, none of the atoms of the reactants changes its oxidation number in forming the products.
Most neutralization reactions are non-redox reactions.
I’m not 100% sure, but I think hydrogen gas is also produced :)