During a spontaneous chemical reaction, it is found that ΔSsys is less than 0. This means that Group of answer choices ΔSsurr is
1 answer:
Answer:
The correct option is: ΔSsurr is greater than 0 and its magnitude is greater than ΔSsys.
Explanation:
For a <u>chemical reaction to be spontaneous, the change in the</u> <u>Gibbs free energy should be negative (ΔG = -ve).</u>
At constant temperature (T) and pressure, the Gibbs free energy is given by the equation:
Here, is the enthalpy change and
is the entropy change of the system.
Also, <u>according to the second law of thermodynamics</u>, <u>for a spontaneous process, the total entropy</u>,
Therefore, <u>for a reaction to be spontaneous</u>, if is less than 0 or negative; then <u>
should be greater than 0 or positive. </u>Also,
>
.
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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.