I: The standard reaction free energy at

equilibrium is zero.
II: A reaction stops when the equilibrium is reached.
III: An equilibrium reaction is not affected by increasing the concentrations of products.
Which of these statements is/are true?

that answer is not correct

Which answer is wrong?

I plugged in the anwser and it was wrong. I tried putting in 1 and 1 and 3

these are the choices

1. Only I and III are true.
2. I, II, and III are true.
3. Only II is true.
4. Only III is true.
5. Only I and II are true.
6. None is true.
7. Only II and III are true.
8. Only I is true.

I agree with all of the answers given by Bob Pursley.

The correct choice from your list is #8. You haven't entered the correct choice; i.e., 8.

8,5, and 1 are wrong

or 4

i Figured it out. The answer is none

To determine which of the statements are true, let's analyze each statement:

I: The standard reaction free energy at equilibrium is zero.
The standard reaction free energy (ΔG°) is a measure of the spontaneity of a chemical reaction. It indicates whether a reaction is energetically favorable or not. At equilibrium, the reaction has reached a balance between the forward and reverse reactions, indicating that there is no net change in the concentration of reactants and products. In this state, ΔG° is indeed zero, indicating that the system is neither energetically favorable nor unfavorable.

II: A reaction stops when the equilibrium is reached.
This statement is not entirely accurate. When a reaction reaches equilibrium, it means that the rate of the forward reaction is equal to the rate of the reverse reaction. However, this does not mean that the reaction completely stops. Instead, it implies that the system is in a dynamic state, where reactants are continuously being converted into products and products are being converted back into reactants at the same rate.

III: An equilibrium reaction is not affected by increasing the concentrations of products.
This statement is incorrect. In an equilibrium reaction, changes in concentration, pressure, or temperature can disrupt the balance of the reaction. When the concentration of products is increased, according to Le Chatelier's principle, the system will try to counteract this change by shifting the equilibrium towards the reactants, promoting the reverse reaction to consume some of the excess product. The reaction will then adjust to establish a new equilibrium.

Therefore, the only true statement is:
I: The standard reaction free energy at equilibrium is zero.

II is not true, ever.

III is not true most times
I is always true