Suppose a reaction has the equilibrium constant K = 2.3 10-7 at a particular temperature. Will there be a large or small amount of unreacted starting material present when this reaction reaches equilibrium?
a)There will be a small amount of unreacted starting material present at equilibrium.
b)This reaction will not ever reach equilibrium due the the K value.
c)The products and reactants will be equal at equilibrium.
d)There will be a large amount of unreacted starting material present at equilibrium.
Is this reaction likely to be a good source of products at this temperature?
Yes
No
To determine the amount of unreacted starting material present at equilibrium, we need to analyze the value of the equilibrium constant (K) for the reaction. In this case, the given value is K = 2.3 × 10^(-7).
The equilibrium constant (K) is a measure of the extent to which a reaction proceeds towards the product or reactant side at equilibrium. It is calculated as the ratio of the concentration (or pressure) of the products raised to their stoichiometric coefficients, divided by the concentration (or pressure) of the reactants raised to their stoichiometric coefficients.
For this reaction, a K value of 2.3 × 10^(-7) indicates a very small value close to zero. Therefore, the products of the reaction will be favored over the reactants at equilibrium. This means that there will be a small amount of unreacted starting material present at equilibrium.
Based on the K value, it suggests that this reaction is not very favorable to the formation of products. The very small K value indicates that the reaction predominantly favors the reactants. Therefore, this reaction may not be a good source of products at this particular temperature.
So, the correct answers would be:
- There will be a small amount of unreacted starting material present at equilibrium.
- No, this reaction is not likely to be a good source of products at this temperature.