From Gibbs free energy , if our delta G is found to be negative the process is s

Question

From Gibbs free energy , if our delta G is found to be negative the process is said to be spontaneous in the forward manner; so it’s a one way streak because the reverse process is said to be non spontaneous, and to be non spontaneous,( the process won’t occur on it s own with out outside intervention).
Question- a negative delta G refers to reaction that will occur on its own with out any outside intervention, and thus it s assumes to be not at equilibrium, so for it to be at equilibrium both process should be spontaneous, and therefore delta G should equal zero.
If a process is said to be non spontaneous in forward direction, will their be any products (even a tiny bit)? And will the rate of the forward direction be equal to the reverse direction for both process to be at some type of equilibrium?
If you have more things to add it, I would greatly appreciate it!
Thank you From Gibbs free energy , if our delta G is found to be negative the process is said to be spontaneous in the forward manner; so it’s a one way streak because the reverse process is said to be non spontaneous, and to be non spontaneous,( the process won’t occur on it s own with out outside intervention).
Question- a negative delta G refers to reaction that will occur on its own with out any outside intervention, and thus it s assumes to be not at equilibrium, so for it to be at equilibrium both process should be spontaneous, and therefore delta G should equal zero.
If a process is said to be non spontaneous in forward direction, will their be any products (even a tiny bit)? And will the rate of the forward direction be equal to the reverse direction for both process to be at some type of equilibrium?
If you have more things to add it, I would greatly appreciate it!
Thank you
Question- a negative delta G refers to reaction that will occur on its own with out any outside intervention, and thus it s assumes to be not at equilibrium, so for it to be at equilibrium both process should be spontaneous, and therefore delta G should equal zero.
If a process is said to be non spontaneous in forward direction, will their be any products (even a tiny bit)? And will the rate of the forward direction be equal to the reverse direction for both process to be at some type of equilibrium?
If you have more things to add it, I would greatly appreciate it!
Thank you
Question- a negative delta G refers to reaction that will occur on its own with out any outside intervention, and thus it s assumes to be not at equilibrium, so for it to be at equilibrium both process should be spontaneous, and therefore delta G should equal zero.
If a process is said to be non spontaneous in forward direction, will their be any products (even a tiny bit)? And will the rate of the forward direction be equal to the reverse direction for both process to be at some type of equilibrium?
If you have more things to add it, I would greatly appreciate it!
Thank you

Explanation / Answer

delta G negative means the reaction is spontaneous and positive means non spontaneous . Now , at equilibrium which means forward and backward rates are equal. Here delta G is zero.

Now start with mathematical equation,

delta G = delta G0 - RT ln K

now for spontaneous ( + value ) of delta G, the vaue of K will be less than 1 .. More postive means more small value of K

K means products / reactants.

so, yes there will be some very tiny products when compared to reactants. As K is very small, very few products will form and large values of reactants remain.

now at equilibrium,

delta G = delta G0 - RT ln Keq

0 = delta G0 - RT ln Keq

delta G0 = RT ln Keq

there will be some value for Keq greater or lesser than 1

At equilibrium the condition should be always rate of forward = rate of backward.

and this conversion is called equilibrium conversion.

eq.

A <--> B

On reaction, amount of B is higher than A.

then K = greater than 1

then delta G is negative.

This reaction favours forward.

case-2:

only some amount of B is formed

K is smaller (B/A)

delta G is positive.

reaction not favor forward.So, it favours backwards.

If it is equilibrium . it settles undisturbed at some point where no B is formed and no A is reacted.

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