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Final Math Review

Total questions: 77

Worksheet time: 3hrs 11mins

Name
Class
Date
1.
CH4  +  2O2  →  CO2  +  2H2O
24 grams of CH4 was added to the above reaction. Calculate the theoretical yield of CO2.
a)
66 grams
b)
132 grams
c)
33 grams
d)
8.72
2.
N2 +  3H2 → 2NH3 
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
a)
6
b)
2
c)
3
d)
1
3.
B2H6 + 3O2 -->2 HBO2 + 2 H2O
 What mass of O2 will be needed to burn 36.1 g of B2H6?
a)
13.8 g O2
b)
3.86 mol of O2
c)

125 g O2

4.
2CO  +  O2  −-> 2CO2
How many liters of carbon dioxide are produced from 10L of carbon monoxide?
a)
10
b)
20
c)
1
d)
5
5.

How many grams of oxygen must be placed in a 3.00 liter container in order to exert a pressure of 2.00 atmospheres at 25 °C?

a)

3.92 grams

b)

7.84 grams

c)

93.8 grams

d)

46.9 grams

6.

What is the percent composition by mass of sulfur (S) in the compound MgSO4?

a)

20.22%

b)

19.85%

c)

26.64%

d)

28.64%

7.

Calculate the number of moles of BaCl2 that are in 436 g of the compound.

a)

3.51 mol

b)

2.09 mol

c)

4.63 mol

d)

2.72 mol

8.

A rigid plastic container holds 1.00 L methane gas at 0.90 atm pressure when the temperature is 22.0°C. How much more pressure will the gas exert if the temperature is raised to 44.6°C and volume remains at 1.00 L?

a)

0.97 atm

b)

1.82 atm

c)

0.97oC

d)

1.82oC

9.

What volume of hydrogen(H2) will be produced at STP by the reaction 67.3 g of magnesium with excess water according to the following reaction?

1Mg (s) + 2H2O (l) --> Mg(OH)2 (aq) + H2 (g)

a)

62.0 L

b)

65.0L

c)

31.0 L

d)

124 L

10.
Cl2 + 2KBr → Br2 + 2KCl
How many grams of potassium chloride (KCl) can be produced from 356 g of potassium bromide (KBr)?
a)
749 g
b)
223 g
c)
479 g
d)
814 g
11.
N2 +  3H2 −->  2NH3 
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
a)
6
b)
2
c)
3
d)
1
12.
2 KClO3 → 2 KCl + 3 O2
How many moles of oxygen are produced when 6.7 moles of KClO3 decompose completely?
a)
6.7 mol
b)
1.0 mol
c)

10. mol

d)
4.5 mol
13.

Determine the temperature required for 0.0470 mol of gas to fill a balloon to 1.20 L under 0.998 atm pressure. 

a)

200 K 

b)
107 K 
c)
207 K 
d)

310. K 

e)

310K

14.
An 18 liter container holds 16.00 grams of oxygen gas (O2) at 45 °C. What is the pressure in the container?
a)
0.725 atm
b)
11.0 atm
c)
23.2 atm
d)
1.45 atm
15.

Given the combustion reaction C3H8 + 5O2 ​​→ 3CO2 + 4H2O, how many liters of carbon dioxide can be produced from 1.00 liter of O2 at standard temperature and pressure?

a)

0.600 L

b)

0.825 L

c)

1.21 L

d)

1.67 L

16.

A sample of oxygen gas occupies 5.0 L at 760 mmHg and a temperature 273 K. What is the mass of the oxygen gas in this sample?

a)

7.1 g

b)

5.0 g

c)

32 g

d)

There is not enough information to determine the mass of the oxygen gas.

17.

What is the percent composition of sodium in sodium hypochlorite?

a)

21.80% Na

b)

30.88% Na

c)

30.90% Na

d)

21.61% Na

18.

Convert 0.830 atm to mmHg

Use sig figs of given

space between number and pressure unit

(a)  

19.

Convert 1.75 atm to kPa

use sig figs of given

space between number and pressure unit

Make sure to type exact pressure unit!

(a)  

20.

What is the pressure in atmospheres exerted by a 0.500 mol sample of nitrogen gas in a 10.0 L container at 298 K?

(a)  

21.

8Zn + S8 --> 8ZnS

If 2.00 mol of Zn are heated with 1.00 mol of sulfur, what is the limiting reactant?

Type full name of limiting reactant.

(a)  

22.

Methanol can be produced through the reaction of CO and H2 in presence of a catalyst.

CO + 2H2 ---> CH3OH

If 75.0 grams of carbon monoxide reacts to produce 68.4 grams of methanol, what is the percentage yield?

Use sig figs for the answer, space then %

(a)  

23.

How many grams of copper are in 3.50 mol?

(a)  

24.

What is the formula for phosphoric acid?

a)

HPO3

b)

H3PO4

c)

H2PO4

d)

H3PO3

25.

perchloric acid

a)

HClO4

b)

HClO2

c)

HClO

d)

HClO3

26.

What is the name of the compound with the formula NiBr2

a)

nitrogen bromide

b)

nickel bromine

c)

nickel (II) bromide

d)

nickel bromide

27.

Name the following ionic compound: Ru(P2O7)2

a)

ruthenium (II) phosphate

b)

ruthenium (II) pyrophosphate

c)

ruthenium (IV) pyrophosphate

d)

ruthenium (VIII) pyrophosphate

28.

Name the following ionic compound: CrC6H4O6

a)

chromium citrate

b)

chromium (II) citrate

c)

chromium (III) citrate

d)

chromium (IV) citrate

29.

What is the formula for ammonium sulfate?

a)

NH3SO4

b)

(NH4)2SO4

c)

NH4(SO4)2

d)

NH42SO4

30.

What is the name of the following compound: Pb3(PO4)4

a)

Lead IV Phosphte

b)

Lead Phosphate

c)

Lead IV Phosphide

d)

Lead Phosphide

31.
silicon dioxide
a)
SO2
b)
NaO2
c)
SiO2
d)
SiO
32.

PCl3

a)

phosphorous trichloride

b)

monophosphorous trichloride

c)

phosphorous tetrachloride

d)

phosphorous chloride

33.
The chemical formula of tetraphosphorus heptaoxide is
a)
F₄O₁₀
b)
P₄O7
c)
PO
d)
P₁₀O₄
34.

A limiting reactant is a reactant that.....

a)

runs out during a chemical reaction

b)

causes a reaction to stop

c)

determines the amount of products that can be made

d)

all of these

35.

Which of the following is NOT a diatomic

a)

H2

b)

N2

c)

P

d)

Cl2

36.

What type of reaction is the following:
Na2S +2HCl −> H2S+2NaClNa_2S\ +2HCl\ ->\ H_2S+2NaCl

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

e)

Combustion

37.

The families/groups of the periodic table contain(s) only metals.

a)

alkali metals

b)

boron family

c)

alkaline earth metals

d)

halogens

38.

Based on their locations on the periodic table, one can infer that calcium and strontium have

a)

the same number of neutrons

b)

the same number of electrons

c)

the same conductivity

d)

similar properties

39.

Argon, krypton and xenon have full outer s and p sublevels. They belong to the

a)

noble gases

b)

alkali metals

c)

alkali earth metals

d)

actinides

40.

The group that has metals that are shiny, soft, have electron configurations that end in s1 and violently react with water to form bases are the

a)

alkali metals

b)

alkali earth metals

c)

aluminum family

d)

lanthanides

41.

The highly reactive group that contains elements in all three states of matter and are all non-metals are the

a)

halogens

b)

carbon family

c)

noble gases

d)

boron family

42.

Elements that are brittle, dull and poor conductors of electricity are

a)

metals

b)

non-metals

c)

metalloids

43.

The only element that does not have a family is (a)   .

44.

The periodic table is set up by

a)

increasing atomic mass

b)

increasing atomic number

c)

increasing atomic radius

d)

decreasing atomic number

45.

The father of the periodic table was _______ and he set it up by _________

a)

Mendelev, increasing atomic mass

b)

Mendelev, increasing atomic number

c)

Moseley, increasing atomic mass

d)

Moseley, increasing atomic number

46.

The modern periodic table used today was created by _______ and is set up by ____________.

a)

Moseley, increasing atomic mass

b)

Moseley, increasing atomic number

c)

Mendelev, increasing atomic mass

d)

Mendelev, increasing atomic number

47.

The elements on the periodic table that are good electrical conductors, malleable, ductile(used to make wire), have luster and make up most of the elements on the periodic table are the

a)

metals

b)

non-metals

c)

metalloids

48.

The elements that touch the zig zag line and have intermediate properties of metals and non-metals are the

a)

metals

b)

non-metals

c)

metalloids

49.

The family that forms bases with water but do not dissolve well and have electron configurations that end in s2 are the

a)

alkali metals

b)

alkaline earth metals

c)

oxygen family

d)

halogens

50.

The family that is all non-metals, have configurations that end in s2p5 and are known as the "salt formers" are the

a)

alkali metals

b)

carbon family

c)

noble gases

d)

halogens

51.

Electronegativity tends to increase _____ and decreases _____

a)

left to right across a period, down a group

b)

up a period, left to right across a group

c)

down a group, down a period

d)

right to left across a group, up a period

52.

The factors that determine trends of the periodic table is/are ________ for groups and _______ for periods.

a)

nuclear charge, number of energy levels

b)

number of energy levels and shielding, nuclear charge

c)

nuclear charge and shielding, number of neutrons

d)

number of electrons, number of neutrons

53.

The group found down between groups IIA and IIIA, numbered 3-12, are good examples of everyday metals. They are the

a)

inner transition metals

b)

transition metals

c)

lanthanides

d)

halogens

54.

Which of the following would have an atomic radius larger than cobalt?

a)

copper

b)

palladium

c)

barium

d)

silver

55.

Which of the following is more electronegative than silicon?

a)

sodium

b)

nickel

c)

selenium

d)

nitrogen

56.

The horizontal row on the periodic table is called a (a)   .

57.

A vertical column is called a (a)   .

58.

What is the name group number IIA?

a)

transition metals

b)

halogens

c)

alkali metals

d)

alkaline earth metals

59.

In this equation,
CuCl2 + NaOH  → Cu(OH)2 + NaCl
Which product is the precipitate?

a)
copper(II) hydroxide
b)
sodium chloride
c)
sodium hydroxide
d)
copper(II) chloride
60.

Considering the following precipitation reaction:

Pb(NO3)2(aq) + KI(aq) → PbI2(s) + KNO3(aq)

What is the correct complete ionic equation?

a)

Pb2+ + (NO3)21- + K1+ + I1- → PbI2(s) + K1+ + NO31-

b)

Pb2+ + NO31- + K1+ + I1- → PbI2(s) + K1+ + NO31-

c)

Pb2+ + NO3- + K1+ + I1- → Pb2+ + I1- + K1+ + NO31-

61.

What type of reaction is this?

Al(OH)3 → Al2O3 + H2O

a)

Combination

b)

Decomposition

c)

Single Replacement

d)

Double Replacement

62.

What type of chemical reaction is this one?

CuO + CO2 --> CuCO3

a)

Decomposition

b)

Combustion

c)

Synthesis

d)

Single Replacement

63.

Which type of reaction is shown?

a)

Combustion

b)

Combination (or Synthesis)

c)

Decomposition

d)

Double replacement

64.

Which is the correct net ionic equation ?

AgNO3 and CaCl2--> AgCl + Ca(NO3)2

a)

Ca2+ +  Cl- → CaCl

b)

Ag+  +  Cl-  → AgCl

c)
Ag +  Cl  →  AgCl
d)

Ag+  +  Ca2+   →Ag2Ca

65.

According to the law of conservation of mass, the mass of the reactants must be________ the mass of the reactants.

a)

greater than

b)

unequal to

c)

less than

d)

the same as

66.

Match the following elements to the group they belong to.

a)

sodium

1.

alkali metal

b)

calcium

2.

alkaline earth metal

c)

chlorine

3.

halogen

d)

argon

4.

noble gas

e)

iron

5.

transition metal

67.

The roman numerals at the top of a column of the periodic table represents the number of ________ ________.

(a)  

68.

CaCO3(s) + 2HCl(aq) →

Pick the correct products

a)

CO2

b)

H2O

c)

CaCl2

d)

HCO3

69.

Label the reactants and products in the chemical equation shown.

a)

Reactants

b)

Products

1
2
1)
2)
70.

In this reaction the products have ​ (a)   ​ Iron (Fe) and ​ (b)   oxygen (O)

Choose from the below words
4
8
2
6
10
71.

A chemist determines that 1.26 g of iron reacts with 0.54 g of oxygen to form rust. The percent composition of each element in the product is: ​ (a)   % iron and ​ (b)   % oxygen.

Choose from the below words
70.0
30.0
3.4
2.23
42.9
57.1
72.

How many of each type of atom are in Na2SO4?

​ (a)   Na

​ (b)   S

​ (c)   O

​ (d)   atoms total

Choose from the below words
2
1
4
7
3
5
6
73.

3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe

Identify the mole ratios for the following pairs:

​ ​ ​ (a)   Mg : ​ (b)   Fe

​ (c)   Fe2O3 : ​ (d)   Fe

​ 1 Fe2O3 : ​ (e)   MgO

Choose from the below words
3
2
1
74.
What pressure in kPa is equal to 2.65 atm?
a)
268 kPa
b)
0.0261 kPa
c)
39.0 kPa
d)
265 kPa
75.

Which of the following is NOT a factor in the ideal gas law?

a)

pressure

b)

temperature in Kelvins

c)

amount of a substance in moles

d)

type of container

76.
In chemistry, a "mole" is:
a)
The mass of an atom
b)
a large number used to count particles
c)
based on the volume of a substance
77.

Match the following units to their correct category.

a)

Grams

1.

Mass

b)

Liters at STP

2.

Volume

c)

Units, Atomes, Molecules

3.

Particles

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