A chemist uses 0.25 L of 2.00 M H2SO4 to completely neutralize a 2.00 L of solution of NaOH. The balanced chemical equation of t
2 answers:
Answer: The molarity of the NaOH solution is 0.5 M.
Explanation:
Moles of in 0.25 L of 2.00 M solution:
Moles of = 2.00 mol/L × 0.25 L = 0.5 moles
Moles of in 2.00 L of an unknown Molarity :
1 mole gives 2 moles of
ions.
Then 0.5 mole will give: 0.5 mol × 2 = 1.0 mol
1.0 mol of will neutralize the 1.0 mol of
ions.
Moles of = Moles of
= 1.0 moles
1 mol of are produced by 1 mol of NaOH
The 1 mole of will be produced from = 1 mol of NaOH
The molarity of the NaOH solution is 0.5 M.
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Answer:
Explanation:
From the given information;
The chemical reaction can be well presented as follows:
⇄
Now, K is known to be the equilibrium constant and it can be represented in terms of each constituent activity:
i.e
However, since we are dealing with liquids solutions;
since the activity of
is equivalent to 1
Hence, under standard conditions(i.e at a pressure of 1 bar)
(b)
From the CRC Handbook, we are meant to determine the value of the Gibb free energy by applying the formula:
Thus, for this reaction; the Gibbs frree energy = -68 kJ/mol
(c)
Le's recall that:
At equilibrium, the instantaneous free energy is usually zero &
Q(reaction quotient) is equivalent to K(equilibrium constant)
So;
(d)
The direction by which the reaction will proceed can be determined if we can know the value of Q(reaction quotient).
This is because;
If Q < K, then the reaction will proceed in the right direction towards the products.
However, if Q > K , then the reaction goes to the left direction. i.e to the reactants.
So;
Since we are dealing with liquids;
Q = 1
Since Q < K; Then, the reaction proceeds in the right direction.
Hence, SO2 as well O2 will combine to yield SO3, then condensation will take place to form liquid.