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Term 3 Quiz 2
Test Description: This is a quiz to review chemical equilibrium
Instructions: Answer all questions to get your test result.
1) What key factor could affect the rate in liquids?
A
surface area
B
pressure
C
concentration
D
shape of container
2) What could lower the activation energy?
A
increasing temperature
B
adding a catalyst
C
decreasing the concentration
D
increasing surface area
3) What is an example of an exothermic reaction?
A
freezing
B
photosynethesis
C
rusting
D
fireworks
4) Hydrogen Peroxide will slowly break down from H2O2 into H2O and O2. This is a relatively slow reaction, but when combined with Potassium Iodide Hydrogen peroxide will break down much more quickly. What conclusion can be drawn from this reaction.
A
The temperature was increased to speed up the reaction.
B
Potassium Iodide acts as a catalyst to speed up the reaction
C
Hydrogen Peroxide acts as a catalyst to speed up the reaction.
D
Potassium Iodide acts as a stir bar increasing the turbulence of the solution
5) If I were to add a teaspoon of sugar and into a cup of water and it were to dissolve what statement could I make?
A
Sugar acts as a solvent and water acts as a solute
B
Sugar and water will form a heterogeneous solution
C
Sugar acts as a solute and water acts as a solvent.
D
Sugar and water can be used to blow really big bubbles.
6) What could make the reaction faster between solid calcium carbonate and acid?
A
make the lumps of calcium carbonate larger
B
make the calcium carbonate powdered
C
make the acid weaker
D
cool it down
7) What would happen if I were to perform the reaction below in a refrigerator? N2(g) + 3H2(g) ⇆ 2NH3(g) + energy
A
Equilibrium will shift to the right and create more products.
B
Equilibrium will shift to the left and create more reactants.
C
Equilibrium will shift to the left and create more products.
D
Equilibrium will shift to the right and create more reactants.
8) What is the Molarity(Moles/Liter) of a solution, when 4.78 moles of C6H12O6 has been dissolved in 500.0 mL of H2O?
A
9.56 M
B
4.78M
C
19.12 M
D
8.37 M
9) gunpowder exploding ...
A
Exothermic
B
Endothermic
10) What does Dynamic Equilibrium mean?
A
Forward and reverse reactions are occurring at same rate
B
All reactants are used up to form products
C
Everything is equal
D
Acids have reacted with bases to form a neutral compound
11) According to Chemical Collision Theory
A
A Particle must be very small for a reaction to occur
B
Particles must collide to cause a reaction
C
A Catalyst must be present for a reaction to occur
D
Particles must be warm for a reaction to occur
12) The solubility of NaCl is 36g/100g of water at 20°C. How many grams of NaCl can dissolve in 200 g of water at the same temperature?
A
555 grams
B
18 grams
C
36 grams
D
72 grams
13) The __________of a solution is the measure of how much of a given solute is dissolved in a given amount of solvent.
A
boiling point
B
concentration
C
percent composition
D
solubility
14) Increasing the concentration of a reactant in a reaction at equilibrium will__________.
A
cause the equilibrium to shift to the left
B
decrease the amount of collisions between reactant molecules and decrease the amount of product formed
C
increase the amount of collisions between reactant molecules and increase the amount of product formed
D
increase the amount of collisions between reactant molecules and decrease the amount of product formed
15) Which of the following gives the best definition of a solvent?
A
a homogeneous mixture
B
a polar substance in which a solute is dissolved
C
a liquid in which a substance can be dissolved
D
the substance in which the solute is dissolved
*select an answer for all questions
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