Equilibrium Constant Concepts

This tutorial explores the concept of equilibrium reactions and the equilibrium constant (Kc). It explains how to write the Kc expression for a reaction, the effect of reversing a reaction on Kc, and the impact of multiplying a reaction by a factor on Kc. The tutorial emphasizes that Kc is dimensionless and provides examples to illustrate these concepts.

What is the main focus of the tutorial?

• Exploring the effects of temperature on reaction rates

• Understanding the equilibrium constant Kc and its manipulation

• Learning about the production of methanol

• Studying the properties of carbon monoxide

In the equilibrium constant expression, what is placed in the denominator?

• Only solids and liquids

• Products raised to their coefficients

• Only gases

• Reactants raised to their coefficients

What is the equilibrium constant expression for the reaction CO + 3H2 -> CH4 + H2O?

• CH4 * H2O / (CO * H2^3)

• CO * H2^3 / (CH4 * H2O)

• CH4 * H2O / (CO^2 * H2^6)

• CO^2 * H2^6 / (CH4 * H2O)

What is the initial value of Kc given in the tutorial?

• 1

• 0.04

• 25

• 0.16

What happens to the equilibrium constant when the reaction is reversed?

• It is halved

• It remains the same

• It doubles

• It becomes the inverse of the original Kc

What is the value of Kc when the reaction is reversed?

• 1

• 0.16

• 25

• 0.04

What is the effect of temperature on the equilibrium constant?

• It remains constant

• It changes with temperature

• It halves with temperature decrease

• It doubles with temperature increase

If the original reaction is multiplied by a factor, how is the new equilibrium constant determined?

• It is half of the original Kc

• It is the same as the original Kc

• It is the square of the original Kc

• It is the inverse of the original Kc

What is the new Kc when the reaction is multiplied by two?

• 0.0016

• 0.08

• 0.04

• 0.16

What is the significance of the equilibrium constant being dimensionless?

• It has units of concentration

• It has no units

• It is independent of the reaction

• It does not change with temperature