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WorksheetsMoles, Percents & Stoichiometry Practice
Total questions: 15
Worksheet time: 26mins
Name
Class
Date
1.
N2 + 3H2 → 2NH3
What is the mole ratio between N2 and NH3 in the above reaction?
a)
1 moles NH3 / 2 moles N2
b)
2 moles NH3 / 1 moles N2
c)
2 moles N2 / 3 moles NH3
d)
1 moles N2 / 3 moles NH3
2.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from 6 moles H2?
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from 6 moles H2?
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
3.
Given the reaction: 4Al + 3O2 --> 2Al2O3
How many moles of Aluminum oxide, Al2O3, can you produce if you have 2 moles of Al?
a)
3 mole
b)
2 mole
c)
1 mole
d)
0.5 mole
4.
What is the molar mass of (NH4)2CO3 ?
a)
144 g
b)
138 g
c)
96 g
d)
78 g
5.
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
6.
4NH3 + 5O2-->4NO + 6H2O
What is the total number of moles of H2O produced when 12 mole of NH3 is completely consumed?
What is the total number of moles of H2O produced when 12 mole of NH3 is completely consumed?
a)
15
b)
18
c)
20
d)
24
7.
Which of the following would have more mass?
a)
1 mole of Li
b)
1 mole of Au
c)
1 mole of Si
d)
None, all are equal
8.
Calculate the % composition by mass of oxygen present in H2SO4.
a)
16.3%
b)
65.25%
c)
32.6%
d)
57.14%
9.
What is the molar mass of calcium hydroxide, Ca(OH)2?
a)
74.1 g/mole
b)
57.1 g/mole
c)
58.1 g/mole
d)
57.1 u
10.
Determine the mass of 2.40 moles of C6H12
a)
201 g
b)
115 g
c)
230. g
d)
353 g
11.
What is the empirical formula of a compound if the molecular formula is W18O9?
a)
W18O9
b)
W2O
c)
W6O3
d)
none of the above
12.
What is the percent by mass of oxygen in MgO?
a)
20%
b)
40%
c)
50%
d)
60%
13.
What is the percent by mass of fluorine in CaF2 (gram-formula mass = 78 g/mol)?
a)
24%
b)
49%
c)
51%
d)
65%
14.
What is the percent composition of Benzene, C6H6?
a)
C = 50%
H = 50%
H = 50%
b)
C = 85.7 %
H = 14.3%
H = 14.3%
c)
C = 92.2%
H = 7.8%
H = 7.8%
d)
C = 71.9%
H = 28.1%
H = 28.1%
15.
If 15.6 g of hydrate are heated and only 11.7 g of anhydrous salt remain, calculate the % of water lost.
a)
25.9%
b)
19.2%
c)
37.9%
d)
76.3%
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