Chemistry Q3 Review

Logs and Anti logs – see worksheets


Balancing chemical reactions – see post

pH practice problems

 

Updated November 27, 2014.

A reversible chemical process is considered in equilibrium when the rate of the forward reaction equals the rate of the reverse reaction. The ratio of these reaction rates is calledthe equilibrium constant. Test your knowledge about equilibrium constants and their use with this ten question equilibrium constant practice test.

You may wish to review Chemical Equilibrium and Equilibrium Constants.

Answers appear at the end of the test.

Question 1

An equilibrium constant with a value K > 1 means:a. there are more reactants than products at equilibrium
b. there are more products than reactants at equilibrium
c. there are the same amount of products and reactants at equilibrium
d. the reaction is not at equilibrium

Cut down a bit of stomach fat every day by never eating these 4 foods.
1000s of Practice Assessments. Full K-12 CCSS Coverage. Try it!

Question 2

Equal amounts of reactants are poured into a suitable container. Given sufficient time, the reactants may be converted almost entirely to products if:a. K is less than 1
b. K is greater than 1
c. K is equal to 1
d. K is equal to 0

Question 3

The equilibrium constant for the reactionH2 (g) + I2 (g) ↔ 2 HI (g)

would be:

a. K = [HI]2/[H2][I2]
b. K = [H2][I2]/[HI]2
c. K = 2[HI]/[H2][I2]
d. K = [H2][I2]/2[HI]

2015 Bestselling Portable Oxygen Compare Latest Deals & Save Big
Convert Any File to a PDF – Word, Jpeg, Gif, Rtf – Free Download!

Question 4

The equilibrium constant for the reaction2 SO2 (g) + O2 (g) ↔ 2 SO3 (g)

would be:

a. K = 2[SO3]/2[SO2][O2]
b. K = 2[SO2][O2]/[SO3]
c. K = [SO3]2/[SO2]2[O2]
d. K = [SO2]2[O2]/[SO3]2

Question 5

The equilibrium constant for the reactionCa(HCO3)2 (s) ↔ CaO (s) + 2 CO2 (g) + H2O (g)

would be:

a. K = [CaO][CO2]2[H2O]/[Ca(HCO3)2]
b. K = [Ca(HCO3)2]/[CaO][CO2]2[H2O]
c. K = [CO2]2
d. K = [CO2]2[H2O]

Search Videos & Articles to Find How to Do it Yourself – Free!

Question 6

The equilibrium constant for the reactionSnO2 (s) + 2 H2 (g) ↔ Sn (s) + 2 H2O (g)

would be:

a. K = [H2O]2/[H2]2
b. K = [Sn][H2O]2/[SnO][H2]2
c. K = [SnO][H2]2/[Sn][H2O]2
d. K = [H2]2/[H2O]2

Question 7

For the reactionH2 (g) + Br2 (g) ↔ 2 HBr (g),

K = 4.0 x 10-2. For the reaction

2 HBr (g) ↔ H2 (g) + Br2 (g)

K =:

a. 4.0 x 10-2
b. 5
c. 25
d. 2.0 x 10-1

Question 8

At a certain temperature, K = 1 for the reaction2 HCl (g) → H2 (g) + Cl2 (g)

At equilibrium, you can be certain that:

a. [H2] = [Cl2]
b. [HCl] = 2[H2]
c. [HCl] = [H2] = [Cl2] = 1
d. [H2][Cl2]/[HCl]2 = 1

Question 9

For the reaction: A + B ↔ C + D6.0 moles of A and 5.0 moles of B are mixed together in a suitable container. When equilibrium is reached, 4.0 moles of C are produced.

The equilibrium constant for this reaction is:

a. K = 1/8
b. K = 8
c. K = 30/16
d. K = 16/30

Question 10

The Haber process is a method to produce ammonia from hydrogen and nitrogen gasses. The reaction is

N2 (g) + 3 H2 (g) ↔ 2 NH3 (g)

If hydrogen gas is added after the reaction has reached equilibrium, the reaction will:

a. shift to the right to produce more product
b. shift to the left to produce more reactants
c. stop. All the nitrogen gas has already been used up.
d. Need more information.

Answers

1. b. there are more products than reactants at equilibrium
2. b. K is greater than 1
3. a. K = [HI]2/[H2][I2]
4. c. K = [SO3]2/[SO2]2[O2]
5. d. K = [CO2]2[H2O]
6. a. K = [H2O]2/[H2]2
7. c. 25
8. d. [H2][Cl2]/[HCl]2 = 1
9. b. K = 8
10. a. shift to the right to produce more product

More equilibrium practice problems

Post navigation

Leave a Reply