Which of the following reactions would have the smallest value of K at 298 K? Which of the following reactions would have the sm
1 answer:
Answer:
The reaction with smallest value of K is :
A + B → 2 C; E°cell = -0.030 V
Explanation:
where :
n = number of electrons transferred
F = Faraday's constant = 96500 C
= standard electrode potential of the cell
R = Gas constant = 8.314 J/K.mol
T = temperature of the reaction =
= equilibrium constant of the reaction
As we cans see, that standard electrode potential of the cell is directly linked to the equilibrium constant of the reaction.
- Higher
higher will be the value of K.
- Lower
So, the reaction with smallest value of electrode potential will have smallest value of equilibrium constant. And that reaction is:
A + B → 2 C;
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Answer:
a) The relationship at equivalence is that 1 mole of phosphoric acid will need three moles of sodium hydroxide.
b) 0.0035 mole
c) 0.166 M
Explanation:
Phosphoric acid is tripotic because it has 3 acidic hydrogen atom surrounding it.
The equation of the reaction is expressed as:
1 mole 3 mole
The relationship at equivalence is that 1 mole of phosphoric acid will need three moles of sodium hydroxide.
b) if 10.00 mL of a phosphoric acid solution required the addition of 17.50 mL of a 0.200 M NaOH(aq) to reach the endpoint; Then the molarity of the solution is calculated as follows
10 ml 17.50 ml
(x) M 0.200 M
Molarity =
= 0.0035 mole
c) What was the molar concentration of phosphoric acid in the original stock solution?
By stoichiometry, converting moles of NaOH to H₃PO₄; we have
=
= 0.00166 mole of H₃PO₄
Using the molarity equation to determine the molar concentration of phosphoric acid in the original stock solution; we have:
Molar Concentration =
Molar Concentration =
Molar Concentration = 0.166 M
∴ the molar concentration of phosphoric acid in the original stock solution = 0.166 M