Question 1 Select one: Explanation Question 2 Select one: Look above!

Question 3 Select one: f. -

Explanation

Look above!

* Remember NOT to include liquids and/or solids in the expression.

Question 4 Select one: Explanation

Look above!

Again tricky tricky no solids and/or liquids.

Question 5 Select one: Explanation

YOU GOT THIS KIDDOS

Question 6

Consider the reaction: 3A(g) + B(s) ↔ 5C(s) + 2D(g).
In a 5.00 L container the reactants and products are at equilibrium. There are 0.44 mol A, 0.30 mol B, 1.43 mol C, and 0.47 mol D. What is the equilibrium constant?

Help: Equilibrium constant Explanation

Hint, remember to first write the equilibrium expression and convert the moles to concentrations.

K = [D]^2 / [A]^3
K= [0.47/5]^2/ [0.44/5]^3
K=12.966

Question 7

Consider the reaction: A(g) + 3B(s) ↔ 3C(g) + 2D(g).
In a 2.00 L container the reactants and products are at equilibrium. There are 0.47 mol A, 0.58 mol B, 1.84 mol C, and 0.27 mol D. What is the equilibrium constant? Explanation

Hint, remember to first write the equilibrium expression and convert the moles to concentrations.
K = [C]^3[D]^2 / [A]
K = [1.84/2]^3[0.27/2]^2 / [0.47/2]
K=0.06038974

Question 8  Explanation

2-x =1.14

x=0.86

y=3x=2.58

x=z=0.86

3H2 = 4 - 3(0.86) = 1.42

2NH3 = 0 + 0.86 = 0.86

Kc = [0.86]^2/ [1.14][1.42]^3= 0.145

Question 9

What is y, that is, how much hydrogen is used?

(Hint, use one of the methods used in the balance equation review problems to do the calculation. Enter amount as a positive quantity. An additional hint is given in the feedback.) Explanation

Additional hint: What is x? It is the amount of nitrogen used. What is the relationship between the amount of nitrogen used and the amount of hydrogen used?

Question 10

What is the equilibrium number of moles of hydrogen? Question 11

What is z, that is, how much ammonia is produce? Question 12

What is the equilibrium constant, Keq?

(Remember to convert the number of moles to moles per liter or concentration in the equilibrium expression.) Question 13

What is the equilibrium expression for:

Ca(OH)2(s) ↔ Ca2+(aq) + 2OH-(aq)?

Select one: Explanation

IF YOU'RE NOT A GAS YOU CANT SIT WITH US

Question 14

Determine the equilibrium constant for the above reaction.

0.1 mol of Ca(OH)2 is placed in 2 L of water and stirred. At equilibrium, at a certain temperature, 0.0224 mol of Ca(OH)2 dissolves. What is Keq? (Assume, the volume of the solution is the same as the initial volume of water.) Explanation

After determining the mol of Ca2+ and the mol of OH-, remember to convert them to concentrations.
Kc= [Ca^2+][OH-]^2
(0.0224/2)(2*0.0224/2)^2 = 5.6e6

Question 15

Consider the reaction: 3A(g) + B(s) ↔ 5C(s) + 2D(g) Keq = 0.42 M-1.
[A] = 0.73 M and [D] =0.22 M. Some B and C are present. What is Q? Explanation Question 16

For the above value of Q

Select one: Question 17

Consider the reaction: 3A(g) + B(s) ↔ 5C(s) + 2D(g) Keq = 0.42 M-1

Same reaction and Keq, but this time:
[A] = 0.94 M and [D] =0.95 M. Some B and C are present. What is Q? Explanation

Q= [0.95]^2/[0.94]^3=1.09

Question 18

For the above value of Q

Select one: Explanation

Q is large than Keq  so to obtain equilibrium the reaction must move to the left so there is more reactant and less product.