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WorksheetsChemistry Final Review Game
Total questions: 60
Worksheet time: 33mins
Name
Class
Date
1.
In a spacecraft, the carbon dioxide exhaled by astronauts can be removed by its reaction with Lithium hydroxide, LiOH, according to the following chemical equation. How many moles of lithium hydroxide are required to react with 20 mol CO2, the average amount exhaled by a person each day?
CO2+2LiOH--> Li2CO3+H2O
CO2+2LiOH--> Li2CO3+H2O
a)
39 mol
b)
40 mol
c)
41 mol
d)
42 mol
2.
2Al + 3H2SO4 -> Al2(SO4)3 + 3H2
How many grams of aluminum sulfate would be formed if 250g H2SO4 completely reacted with aluminum?
How many grams of aluminum sulfate would be formed if 250g H2SO4 completely reacted with aluminum?
a)
0.85 g
b)
290 g
c)
450 g
d)
870 g
3.
How many grams of CO are needed to react with Fe2O3 to produce 558 g Fe? The equation for the reaction is: Fe2O3(s) + 3CO(g) → 3CO2(g) + 2Fe(s)
a)
280 g
b)
5 g
c)
55 g
d)
420 g
4.
Calculate the number of moles of water produced when 3.3 mol of Cu(NO3)2 are formed in the reaction. 3Cu(s) + 8HNO3(aq) → 3Cu(NO3)2(s) + 2NO(g) + 4H2O(l)
a)
4.4 mol
b)
4.5 mol
c)
4.6 mol
d)
4.7 mol
5.
How many grams of Cu would be needed to react with 2.0 mol HNO3?3Cu(s) + 8HNO3(aq) → 3Cu(NO3)2(s) + 2NO(g) + 4H2O(l)
a)
45.6 g
b)
46.6 g
c)
47.6 g
d)
48.6 g
6.
When the limiting reactant in a chemical reaction is completely used, the
a)
the reaction stops
b)
the reaction speeds up
c)
excess reactants being used
d)
reaction slows down
7.
Which is Avogadro's number?
a)
6.02 X 10^23
b)
6.02 X 10^24
c)
6.02 X 10^25
8.
The mass of one mole of a substance
a)
gram
b)
Molar mass
c)
calorie
9.
Amount of substance
a)
Mole
b)
Chemistry
10.
the conditions under which the volume of a gas is usually measured
a)
Volume
b)
Standard Pressure and Temperature (STP)
11.
A rigid container of O2 has a pressure of 388 kPa at a temperature of 713 K. What is the pressure at 273 K?
a)
148.56 kPa
b)
150 kPa
c)
160 kPa
d)
170 kPa
12.
A gas occupies a volume of 0.2 L at 25 kPa. What volume will the gas occupy at 2.5 kPa?
a)
2 L
b)
4 L
c)
1 L
d)
10 L
13.
If 30.5 L of nitrogen at 705 mm Hg are compressed to 285 mm Hg at constant temperature. What is the new volume?
a)
69 L
b)
80 L
c)
70 L
d)
75 L
14.
A sample of hydrogen occupies a volume of 1.20 L at a pressure of 4.2 atm. If the temperature of the gas is kept constant, what would the new volume of the gas be at 6.0 atm?
a)
0.8 atm
b)
1 atm
c)
1.5 atm
d)
0.5 atm
15.
A gas occupies 40.0 mL at 123 C. What volume does it occupy at 27 C, assuming pressure is constant?
a)
20 mL
b)
25 mL
c)
30 mL
d)
35 mL
16.
As the temperature of a gas increases, the pressure will _______.
a)
decrease
b)
increase
17.
The conversion of a liquid to a gas is called ___________.
a)
precipitation
b)
condensation
c)
evaporation
18.
The device for measuring atmospheric pressure is ___________.
a)
barometer
b)
thermometer
c)
meter stick
d)
internet
19.
The temperature 0 K or -273 oC is called _________________.
a)
absolute positive
b)
absolute negative
c)
absolute zero
20.
Boyles’ law
a)
P1V1=P2V2
b)
V1/T1=V2/T2
21.
Amount of solute that dissolves in a given quantity of solvent to produce a saturated solution
a)
molarity
b)
solvent
c)
solute
d)
solubility
22.
Solution that contains the maximum amount of sugar for that given temperature
a)
unsaturated solution
b)
saturated solution
23.
Substance to be dissolved
a)
solute
b)
solvent
24.
Substance doing the dissolving
a)
solute
b)
solvent
25.
Solution that will still dissolve more sugar without raising the temperature
a)
saturated solution
b)
unsaturated solution
26.
One has 0.90 g NaCl in 100 mL of solution. What is the molarity of the NaCl solution?
a)
0.00001 M
b)
15 M
c)
0.15 M
d)
0.0000000001 M
27.
A solution has a volume of 2.0 L and contains 36.0 g of glucose (C6H12O6). If the molar mass of glucose is 180 g/mol, then what is the molarity of the solution?
a)
0.1 M
b)
1 M
c)
0.01 M
28.
How many milliliters of water would you need to prepare 250 mL of 0.20 M NaCl from a solution of 1.0 M NaCl?
a)
0.5 mL
b)
5 mL
c)
50 mL
d)
100 mL
29.
To 225 mL of a 0.80M solution of KI, a student adds enough water to make 1 L of a more dilute KI solution. What is the molarity of the new solution?
a)
18 M
b)
0.18 M
c)
0 018 M
30.
What is the molarity of a solution that contains 8 moles of solute in 2 L of solution?
a)
10 M
b)
2 M
c)
1 M
d)
4 M
31.
What is the proper Keq for the following reaction?
2 NO(g) + O2(g) ⇌2 NO2(g)
2 NO(g) + O2(g) ⇌2 NO2(g)
a)
Keq = [NO2]2 / [NO]2[O2]
b)
Keq = [NO]2[O2] / [NO2]2
c)
Keq = [NO]2[O2][NO2]2
d)
Keq = 2[NO][O2] / 2[NO2]
32.
Which is not a factor influencing rate of reaction?
a)
Temperature
b)
Concentration
c)
particle size
d)
wieght
33.
Is one in which the conversions of reactants to products and the conversion of products to reactants occur at the same time
a)
reversible reaction
b)
chemical equillibrium
c)
product
d)
reactant
34.
Is when the rates of the forward and reverse reactions are equal, and the reaction has reached a state of balance.
a)
Reversible reaction
b)
Chemical Equillibrium
c)
products
d)
reactants
35.
If a stress is applied to a system is in dynamic equilibrium, the system changed in a way that relives the stress.
a)
Le Chatelier's principle
b)
Boyle's law
36.
When Keq has a large value, such as 2.7 x 10^9, what will the reaction at equilibrium mainly consist of?
a)
Reactants
b)
Products
37.
When Keq has a small value, such as 2.7 x 10^9, what will the reaction at equilibrium mainly consist of?
a)
Reactants
b)
Products
38.
What is the effect of adding more H2CO3 to the following reaction: CO2+H2O-->H2CO3
a)
increase reactants
b)
decrease reactants
39.
In the equation where will the shift be:
N2+O2-->2NO
O2 is added
N2+O2-->2NO
O2 is added
a)
right
b)
left
40.
In the equation where will the shift be:
N2+O2-->2NO
NO is removed
N2+O2-->2NO
NO is removed
a)
right
b)
left
41.
________ is the measurement of the heat flow into or out of a system.
a)
caloriemeter
b)
thermochemistry
42.
In an exothermic reaction, enthalpy change is considered a __________
a)
product
b)
reactant
43.
In an endothermic reaction, enthalpy change is considered a _________
a)
product
b)
reactant
44.
The SI unit of energy is
a)
Joules
b)
Calories
45.
_______________ states that in any chemical or physical process, energy is neither created nor destroyed.
a)
Law of conservation of energy
b)
Law of conservation of mass
46.
The temperature of a piece of iron with a mass of 18.0 g increases from 25.0*C to 40.0*C when the metal absorbs 124.2 J of heat. What is the specific heat of the iron?
a)
46 J/g*C
b)
4.6 J/g*C
c)
0.46 J/g*C
47.
Determine the specific heat, in units of cal/g⁰C, of a material if a 12 g sample absorbed 96 J as it was heated from 20 to 40. Report your answer to 1 decimal place!
a)
0.1
b)
1
c)
10
48.
The temperature of a 6.0 g sample of glass changed from 20 to 45 when it absorbed 550 J of heat. What is the specific heat of this glass sample?
a)
3.67 J/gC
b)
4.8 J/gC
c)
6.9 J/gC
49.
How much heat (in calories) is needed to raise 20 grams of water from 5 ⁰C to 40 ⁰C? The specific heat of water is 1 cal/g⁰C.
a)
750 cal
b)
700 cal
c)
800 cal
d)
850 cal
50.
300 grams of ethanol at 10 °C is heated with 14640 Joules of energy. What is the final temperature of the ethanol? The specific heat of ethanol is 2.44 J/g·°C.
a)
30 C
b)
40 C
c)
50 C
51.
A substance that can act as either an acid or a base is said to be
a)
monophoteric
b)
diphoteric
c)
Amphoteric
52.
A substance with a pH of 7 would be considered a/an
a)
neutral
b)
acid
c)
base
53.
A substance with a pH of 4.3 would be considered a/an
a)
base
b)
acid
c)
neutral
54.
A substance with a pH of 10.5 would be considered a/an
a)
base
b)
acid
c)
neutral
55.
when the number of moles of hydrogen ions equals the number of moles of hydroxide ions in titration
a)
equivalence point
b)
balance point
56.
What is the molarity of a sodium hydroxide solution if 38 mL of the solution is titrated to the end point with 14 mL of 0.75M sulfuric acid? NaOH + H2SO4 --> Na2SO4 + H2O (unbalanced)
a)
0.55 M
b)
5.5 M
57.
What volume (in mL) of 0.25 M Ba(OH)2 is needed to neutralize 52.2 mL of 0.19 M HCl?Ba(OH)2 + HCl --> BaCl2 + H2O (unbalanced)
a)
18.9 mL
b)
19.8 mL
58.
Among the following Ka values, which represents the strongest acid?
a)
Ka = 3.4 x 10-5
b)
Ka = 5.8 x 10-10
c)
Ka = 1.2 x 10-3
59.
Which of these solutions is most basic?
a)
[H+] = 1 × 10–11
b)
[OH–] = 1 × 10−13
c)
[OH–] = 1 × 10–4
60.
If the [H+] in a solution is 1 × 10−11 mol/L, then the pH is
a)
11
b)
1
c)
4
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