on quotient Q has a smaller value than the related equilibrium c onstant, K, the

Question

on quotient Q has a smaller value than the related equilibrium c onstant, K, the reaction is at equilibrium. b) the reaction will continue to make c, the d. th c. the value of K will decrease until it is equal to reaction will consume products and make reactants. e reaction will release heat to achieve equilibrium 20. Addition of reactants to a chemical reaction in solution or gas phase at equilibrium a. an increase in K and a shift in equilibrium to produce more products. b. an increase in K and a shift in equilibrium to produce more reactants. c. a decrease in K and a shift in equilibrium to produce more products. d. a decrease in K and a shift in equilibrium to produce more reactants. e. no change in K and a shift in equilibrium to produce more products 21. Increasing the temperature of an exothermic reaction results in a. more products and fewer reactants. D more reactants and fewer products. c. more reactants and products. d. fewer reactants and products. e. no change in the quantities of reactants and products. For a chemical reaction at equilibrium, which of the following will change equilibrium constant K? 22. Changing the temperature Changing the total concentration of reactants and products Changing the reaction coefficients I. II. III. a. I only b. Il only c. III only d. 1 and lI only eI and III only

Explanation / Answer

Q19

Note that the concentrations MUST be in equilibrium. If these are not in equilibrium, then the reaction will take place until there is equilibrium achieved.

For this, we use Q, the reaction quotient of products/reactants, it allows us to understand the ratio distribution and the direction/shit of equilibrium

Q is defined as:

Q = [C]^c * [D]^d / ([A]^a * [B]^b)

In this Case, the concentrations are NOT in equilibrium

Therefore:

If Q < Keq; this has much more reactants than products, therefore expect reactants to form more product in order to achieve equilibrium

If Q > Keq; this has much more products than reactants, therefore expect products to form more reactants in order to achieve equilibrium

If Q = Keq; this has the same ratio in equilibrium for reactants and products. Expect no reaction. It is safe to assume this is already in equilibrium.

therefore...

choose c

Q20

addition of reactants will favour more product formation

K will NEVER change, since it is constant at such temperature, choose "E"

Q21

if exothermic, it releases heat

increasing T, will not favour product sformation

then

choose B, more reactants form

Q22

note that, K is constant in equilbirium

I --> change of T will chang eK

II --> never, total concentration has nothing to do

III ---> reaciton coefficients will imply another reaction, therefore ignore this

choose I only

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