5I.27

[Emily Vainberg 1D]

For 51. 27 I got Q< k which means the reaction proceeds left, but I don't get part C. It asks "What is the equilibrium composition of the reaction system?"
Can someone explain what this means?

[Selena Yu 1H]

Part c is asking for the amount of each product and reactant at equilibrium. So you would use the ICE method to figure out the concentrations of the reactants and products.

[Asia Yamada 2B]

Yes Q < K, but that means that the reaction would proceed to the right, forming products. For part C, since you are given the initial concentrations and the value of Kc, you can use the ICE table to determine the concentrations at equilibrium.

[shevanti_kumar_1E]

Because Q<K the forward reaction is favored (towards products). You would use an ICE table to find the concentrations of the reactants and products. You would use expression Kc = [Products]/[Reactants]. You can use -x to represent the change in molar concentration of the reactants and +x to represent the change in molar concentration of the product.

[Cora Chun 2D]

To find the equilibrium composition, use an ICE table to find the equilibrium concentrations of each of the substances in the reaction!

[Praneetha Kakarla 3A]

Hey, others already answered your question but I wanted to point out that if Q < K, then the rxn should actually proceed to the right, not the left like you mentioned. It might've been a typo, but I figured I would clarify just in case :)

[Mary Gallo 1G]

When Q<K, this means that there is a greater concentration of reactants than there would be at equilibrium. Therefore, the reaction would actually proceed right, towards the products, to achieve equilibrium.