Which of the following reactions will be spontaneous at standard state? Not all the reactions are balanced, so make sure they are balanced first. The ΔG of formation data can be found in an appendix in your text book. You may select multiple answers.


Any reaction with positive a ΔG value for the reaction.

K + H2O(l) = KOH + 1/2H2

S(rhombic) + O2 = SO2

H2(g) + I2(s) = 2HI(g)

Balance the equations.

dGorxn = (n*dGoformation products) - (n*dGo formation reactants)
The rxn is not spontaneous if dGo rxn at std conditions is +.

To determine if a reaction will be spontaneous at standard state, we need to calculate the Gibbs free energy change (ΔG) for each reaction. If the ΔG value is negative, the reaction will be spontaneous.

Let's calculate the ΔG for each reaction:

1. K + H2O(l) = KOH + 1/2H2

This reaction is not balanced, so let's balance it first:

2K + 2H2O(l) = 2KOH + H2

Now we can calculate the ΔG using the ΔG of formation data for each species involved. Unfortunately, since you mentioned that the ΔG of formation data can be found in an appendix in your textbook, I don't have access to that information. Therefore, I cannot calculate the ΔG for this reaction.

2. S(rhombic) + O2 = SO2

This equation is already balanced. Again, I don't have access to the ΔG of formation data, so I cannot calculate the ΔG for this reaction.

3. H2(g) + I2(s) = 2HI(g)

This reaction is balanced. Similarly, without the ΔG of formation data, I cannot determine the ΔG for this reaction.

In conclusion, since I don't have the necessary ΔG of formation data, I cannot determine which of the reactions will be spontaneous at standard state.

To determine which of the given reactions will be spontaneous at standard state, we need to analyze the change in Gibbs free energy (ΔG) for each reaction.

But before that, let's balance the reactions:

1. K + H2O(l) = KOH + 1/2H2:

The balanced equation is 2K + 2H2O(l) = 2KOH + H2.

2. S(rhombic) + O2 = SO2:

The balanced equation is 2S(rhombic) + 3O2 = 2SO2.

3. H2(g) + I2(s) = 2HI(g):

The balanced equation is H2(g) + I2(g) = 2HI(g).

Now, we can determine the spontaneity of each reaction by comparing the ΔG values with zero:

1. Reaction: 2K + 2H2O(l) = 2KOH + H2

To find the ΔG for this reaction, we need the ΔG of formation values for each compound involved, which can be found in the appendix of your textbook. Calculate the ΔG using the formula:

ΔG = ΣΔGf(products) - ΣΔGf(reactants)

If the calculated ΔG is negative, the reaction is spontaneous at standard state.

2. Reaction: 2S(rhombic) + 3O2 = 2SO2

Again, use the same formula to calculate ΔG using the ΔG of formation values for each compound.

3. Reaction: H2(g) + I2(g) = 2HI(g)

Calculate ΔG using the formula mentioned above.

Once you have the ΔG values for each reaction, compare them to zero. If the ΔG value is negative, the reaction is spontaneous at standard state. If the ΔG value is positive, the reaction is not spontaneous.

Remember to consult the ΔG of formation data in the appendix of your textbook to calculate the ΔG for each reaction.