For a reaction a A + bB cC + dD the equilibrium constant K is defined as the rat

Question

For a reaction a A + bB cC + dD the equilibrium constant K is defined as the ratio of products to reactants at equilibrium: K = [c]c[D]d/[A]a[B]b Because K represents the ratio of products to reactants, the magnitude of K is an indicator of the levels of products and reactants present when the reaction is at equilibrium. Some chemical reactions proceed almost fully to product, whereas other chemicals hardly react with each other at all, or react so as to have significant amounts of both reactants and products at equilibrium. The industrial production of lime (CaO) from calcium carbonate is accomplished via the following reaction: CaCO3(s) CaO(s) + CO2(g) Given the following data: What can be said about this reaction? Lower temperatures result in more lime formation. The reaction makes more lime at higher temperatures. Q The reaction goes to completion at 1200 K. The equilibrium lies far to the right at room temperature.

Explanation / Answer

K at 1200 K (higher temperature) is > 1 --> products favoured K at 298 K (lower temperature) is < 1 --> reactants favoured The correct answer is B.

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