15.2.2 Predicting the Direction of a Reaction Flashcards
Which statement is NOT correct about the diagram?
At Point 4, Q is equal to KEq. Therefore, the system is at equilibrium and the final concentrations for all of the products can be determined.
Which of the following statements about values for Q is NOT correct?
If Q is greater than KC, then the forward reaction will occur. The concentrations of the products will increase and the concentrations of the reactants will decrease.
Suppose you have 28 L of components in a flask (at 400 degrees C). The components include 1.5 mol N2, 2.1 mol H2, and 1.8 mol NH3. If the equilibrium equilibrium is N2(g) + 3H2(g) 2NH3(g) (where KEq = 0.50 at 400 degrees C), which statement is NOT correct?
Q = 347; the reaction will move toward the reactants to reach equilibrium.
Suppose you have a 38 L flask containing the following components: 1.8 mol HI, 2.7 mol H2, and 1.1 mol I2, all at 417 degrees C. If the equilibrium equation is I2(g) + H2(g) 2HI(g) (where Kc = 54 at 417 degrees C), which statement about this reaction is NOT correct?
Q is less than KEq. The reverse reaction is favored.
Look at the following general reaction:
aA + bB cC + dD
Suppose that the correct expression for KEq (or Kc) for this reaction was:
KEq = [D]^d / [B]^b
Which of the following gives a reasonable explanation for this expression?
A and C are solids.
Which statement about Q and KEq is not correct?
If Q < KEq, a shift toward the reactants is favored as the reaction moves to equilibrium.
Which of the following statements about values for Q is not correct?
If Q = 4.0 • KEq, then the reaction must shift toward the reactants. In addition, the product of the reactant concentrations (to their respective powers) is four times the product of the product concentrations (to their respective powers).
Look at the diagram. Which statement about Point 3 is NOT true?
The concentration of the reactants will increase as the reaction moves toward equilibrium.
What is the value of Q for the following reaction? Also, decide which way the reaction will shift to reach equilibrium. There are 35 L of 0.7 mol BrCl, 2.0 mol Br2, and 1.3 mol Cl2.
2BrCl(g) Br2(g) + Cl2(g)
Where Kc = 32 at 217 degree C.
Q is 5.27. The reaction will shift toward products to reach equilibrium.
Suppose that you have 25 L of components in a flask at 400 degrees C. The components include 1.8 mol Cl2, 2.2 mol H2, and 1.0 mol HCl.
Cl2(g) + H2(g) 2HCl(g)
Where Kc = 5.1 x 10^8 at 400 degrees C.
Which statement is NOT correct?
Q is 6.31, which is less than Kc. So the reaction will shift toward the products to reach equilibrium.
