Elite QandA


What does it mean when Q is bigger than KC?


  1. What does it mean when Q is bigger than KC?
  2. What is favored when q is greater than K?
  3. What is Q compared to K?
  4. How does Q affect K?
  5. What happens when K is greater than Q?
  6. How does Q compare to KEQ?
  7. What happens if k is greater than Q?
  8. What does it mean if q is greater than 1?
  9. What happens if q is greater than K?
  10. What does it mean when K is greater than 1?
  11. What if Q is less than 1?
  12. What does a large K value mean?
  13. What happens if Q is greater than K?
  14. What does it mean if Q is greater than 1?

What does it mean when Q is bigger than KC?

The value of the reaction quotient Q is greater than the value of the equilibrium constant K. Hence, the equilibrium will shift in the backward direction. Thus, it is true that If concentration quotient, Q is greater than \[{K_C}\] , the net reaction is taking place in a backward direction.

What is favored when q is greater than K?

If Q is greater than K, then that means we have more product than we need and we need more reactant to reach equilibrium. As a result, the reverse reaction is favored to maintain balance.

What is Q compared to K?

It is important to understand the distinction between Q and K. Q is a quantity that changes as a reaction system approaches equilibrium. K is the numerical value of Q at the "end" of the reaction, when equilibrium is reached.

How does Q affect K?

When Q=K, the system is at equilibrium and there is no shift to either the left or the right. The value of Kc at 483 K is 14.5. If Q=14.5, the reaction is in equilibrium and will be no evolution of the reaction either forward or backwards.

What happens when K is greater than Q?

If K > Q, a reaction will proceed forward, converting reactants into products. If K < Q, the reaction will proceed in the reverse direction, converting products into reactants. If Q = K then the system is already at equilibrium.

How does Q compare to KEQ?

What is the difference between Q and Keq? Q is what is. Keq is what will be. Q and Keq both have the same algebraic form: basically, products over reactants, with coefficients as exponents.

What happens if k is greater than Q?

Q can be used to determine which direction a reaction will shift to reach equilibrium. If K > Q, a reaction will proceed forward, converting reactants into products. If K < Q, the reaction will proceed in the reverse direction, converting products into reactants. If Q = K then the system is already at equilibrium.

What does it mean if q is greater than 1?

This means that in the Q equation, the ratio of the numerator (the concentration or pressure of the products) to the denominator (the concentration or pressure of the reactants) is larger than that for K, indicating that more products are present than there would be at equilibrium.

What happens if q is greater than K?

Q can be used to determine which direction a reaction will shift to reach equilibrium. If K > Q, a reaction will proceed forward, converting reactants into products. If K < Q, the reaction will proceed in the reverse direction, converting products into reactants. If Q = K then the system is already at equilibrium.

What does it mean when K is greater than 1?

If the value of K is greater than 1, the products in the reaction are favored. If the value of K is less than 1, the reactants in the reaction are favored. If K is equal to 1, neither reactants nor products are favored.

What if Q is less than 1?

if Q<1 or Q>1 then certainly you know something about the ratio of products to reactants. But without comparing to K, there's no knowing which way it will shift or proceed.

What does a large K value mean?

The value of K indicates the equilibrium ratio of products to reactants. In an equilibrium mixture both reactants and products co-exist. Large K > 1 products are "favored" K = 1 neither reactants nor products are favored. Small K < 1 reactants are "favored"

What happens if Q is greater than K?

Q can be used to determine which direction a reaction will shift to reach equilibrium. If K > Q, a reaction will proceed forward, converting reactants into products. If K < Q, the reaction will proceed in the reverse direction, converting products into reactants. If Q = K then the system is already at equilibrium.

What does it mean if Q is greater than 1?

This means that in the Q equation, the ratio of the numerator (the concentration or pressure of the products) to the denominator (the concentration or pressure of the reactants) is larger than that for K, indicating that more products are present than there would be at equilibrium.



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