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WorksheetsChapter 1,2 Fundamentals of Chemistry and Atomic Structure
Total questions: 20
Worksheet time: 26mins
Name
Class
Date
1.
What is the mole ratio of H2O to H3PO4 in the following chemical equation? P4O10 + 6 H2O --> 4 H3PO4
a)
6:4
b)
4:6
c)
1:3
d)
3:1
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.
For the reaction represented by the equation Cl2 + 2KBr → Br2 + 2KCl, how many grams of potassium chloride can be produced from 356 grams potassium bromide?
a)
749 g
b)
225 g
c)
479 g
d)
814 g
4.
2H2 + O2 → 2H2O
How many moles of water can be produced if 8 moles H2 are used?
How many moles of water can be produced if 8 moles H2 are used?
a)
4 moles
b)
8 moles
c)
16 moles
d)
2 moles
5.
N2 + 3H2 → 2NH3
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
How many moles of hydrogen are needed to react with 2 moles of nitrogen?
a)
6
b)
2
c)
3
d)
1
6.
Fe2O3 + 3H2 → 2Fe + 3H2O
About how many grams of H2O will be produced from 150 grams of Fe2O3?
About how many grams of H2O will be produced from 150 grams of Fe2O3?
a)
50 grams H2O
b)
60 grams H2O
c)
5000 grams H2O
d)
6000 grams H2O
7.
CH4 + 2 O2 → CO2 + 2 H2O
How many moles of carbon dioxide are produced from the combustion of 110 g of CH4?
How many moles of carbon dioxide are produced from the combustion of 110 g of CH4?
a)
13.7 mol
b)
2.75 mol
c)
6.11 mol
d)
6.85 mol
8.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
9.
A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?
a)
Mg4N3
b)
MgN2
c)
Mg3N2
d)
MgN
10.
You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements.
a)
SO
b)
SO2
c)
SO3
d)
SO4
11.
What is the molecular formula if the empirical formula is CH2O and the molecular molar mass is 180.18?
a)
CH2O
b)
C2H4O2
c)
C4H8O4
d)
C6H12O6
12.
A chemical formula that shows the actual # and kinds of atoms present in one molecule of a compound is called_________
a)
ionic formula
b)
covalent formula
c)
empirical formula
d)
molecular formula
13.
An empirical formula:
a)
is a formula that calculates the coefficients of a compound in a balanced equation.
b)
is the simplest whole-number ratio of moles of elements in the compound.
14.
Subatomic particles with a negative charge
a)
Electrons
b)
Neutrons
c)
Protons
d)
Quarks
15.
Subatomic particles with a positive charge
a)
neutrons
b)
atomic mass
c)
protons
d)
isotopes
16.
Discovered the electron within the atom
a)
Thomson
b)
Chadwick
c)
Schrodinger & Heisenberg
d)
Dalton
17.
Discovered the neutron within the atom
a)
Democritus
b)
Thomson
c)
Rutherford
d)
Chadwick
18.
In an atom, electrons move in definite orbits around the nucleus.
a)
Thomson
b)
Rutherford
c)
Bohr
d)
Democritus
19.
The Gold Foil experiment was done by __________.
a)
Chadwick
b)
Bohr
c)
Rutherford
d)
Thomson
20.
In order of most to least penetrating radiation we have
a)
Alpha , Beta, Gamma
b)
Beta , Gamma , Alpha
c)
Gamma, Beta, Alpha
d)
Gamma, Alpha, Beta
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