Equilibrium Constants and ICE Method

The video tutorial covers advanced equilibrium concepts, focusing on calculating the equilibrium constant (KC) at different temperatures and predicting reaction types. It introduces the ICE method for determining equilibrium concentrations and explores the relationship between Gibbs free energy and KC, explaining how spontaneity affects equilibrium.

What is the general form of the equilibrium constant expression Kc?

• Reactants over products, with coefficients as exponents

• Products over reactants, with coefficients as exponents

• Products over reactants, without coefficients

• Reactants over products, without coefficients

If the value of Kc increases with temperature, what can be inferred about the reaction?

• The reaction is endothermic

• The reaction is at equilibrium

• The reaction is spontaneous

• The reaction is exothermic

In the ICE method, what does the 'C' stand for?

• Concentration

• Change in concentration

• Constant

• Coefficient

When using the ICE method, what is the initial concentration of products?

• One mole

• Zero

• Equal to the reactants

• Depends on the reaction

Which method is used to calculate equilibrium concentrations in a reaction?

• Spontaneity method

• Delta G method

• Kc method

• ICE method

In a reaction where the initial concentration of N2 is 1 mole and at equilibrium it is 0.8 moles, what is the change in concentration?

• 0.4 moles

• 0.8 moles

• 0.6 moles

• 0.2 moles

How does a positive Delta G affect the equilibrium constant Kc?

• Kc is equal to 1

• Kc is less than 1

• Kc is greater than 1

• Kc is not affected

What does a negative Delta G indicate about a reaction?

• The reaction is at equilibrium

• The reaction is exothermic

• The reaction is non-spontaneous

• The reaction is spontaneous

What is the relationship between Delta G and Kc when Delta G is negative?

• Kc is greater than 1

• Kc is not defined

• Kc is equal to 1

• Kc is less than 1

What is the significance of the equilibrium constant Kc being greater than 1?

• The reaction is non-spontaneous

• More products than reactants

• More reactants than products

• Equal amounts of reactants and products