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Chemical calculations review
2/7/12 9:53 PM
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Teacher: Mr. gerraputa
Name: ____________________________________
1.
5.
A chemical formula is an expression used to represent
What is the total number of atoms of oxygen in the formula
Al(ClO3)3 . 6H2O?
1. mixtures, only
3. compounds, only
2. elements, only
4. compounds and elements
--------------
1. 6
3. 10
2. 9
4. 15
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2.
What is the total number of moles of atoms in one mole of
(NH4)2SO4?
6.
Which quantity is equivalent to 39 grams of LiF?
1. 10
3. 14
1. 1.0 mole
3. 0.50 mole
2. 11
4. 15
2. 2.0 mole
4. 1.5 mole
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3.
7.
Given the equation: __FeCl2 + __Na2CO3 → __FeCO3 +
__NaCl
What is the percent by mass of oxygen in Fe2O3 (formula mass =
160)?
When the equation is correctly balanced using the smallest whole
numbers, the coefficient of NaCl is
1. 16%
3. 56%
2. 30.%
4. 70.%
1. 6
3. 3
2. 2
4. 4
---------------------------
8.
What is the molecular formula of a compound with the empirical
formula P2O5 and a gram-molecular mass of 284 grams?
4.
In the compound Al2O3, the ratio of aluminum to oxygen is?
1.
2.
3.
4.
2 grams of aluminum to 3 grams of oxygen
3 grams of aluminum to 2 grams of oxygen
2 moles of aluminum to 3 moles of oxygen
3 moles of aluminum to 2 moles of oxygen
1.
2.
3.
4.
P 2O 5
P 5O 2
P10O4
P4O10
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Chemical calculations review
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9.
13.
What is the total number of moles of oxygen atoms present in one What is the total mass of oxygen in 1.00 mole of Al2(CrO4)3?
mole of Mg(ClO3)2?
1. 192 g
3. 64.0 g
1. 5
3. 3
2. 112 g
4. 48.0 g
2. 2
4. 6
--------------------------14.
10.
Which quantity is represented by the symbol Ne?
When the equation
__C8H16 + __O2 → __CO2 + __H2O
is correctly balanced using the smallest whole number
coefficient, the coefficient of O2 is
1. 1
3. 12
2. 8
4. 16
1.
2.
3.
4.
1 gram of neon
1 liter of neon
1 mole of neon
1 atomic mass unit of neon
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--------------
15.
When the equation: __Al2(SO4)3 + __ZnCl2 → __AlCl3 +
__ZnSO4
11.
Which substance has the same molecular and empirical formulas? is correctly balanced using the smallest whole number
coefficients, the sum of the coefficients is
1. C6H4
2. C2H4
1. 9
3. 5
3. CH4
2. 8
4. 4
4. C6H12O6
--------------------------16.
12.
Which equation illustrates conservation of mass?
1.
2.
3.
4.
H2 + Cl2 → HCl
H2 + Cl2 → 2HCl
H2 + O2 → H2O
H2 + O2 → 2H2O
--------------
Given the unbalanced equation: ___Ca(OH)2 + ___(NH4)2SO4
→ ___CaSO4 + ___NH3 + ___H2O
What is the sum of the coefficients when the equation is
completely balanced using the smallest whole-number
coefficients?
1. 5
3. 9
2. 7
4. 11
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Chemical calculations review
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17.
22.
Which is an empirical formula?
Vitamin C has an empirical formula of C3H4O3 and a molecular
mass of 176. What is the molecular formula of Vitamin C?
1.
2.
3.
4.
H2O2
H2O
C2H2
C3H6
1.
2.
3.
4.
--------------
C3H4O3
C6H8O6
C9H12O9
C10H8O3
--------------
18.
What is the gram formula mass of Li2SO4?
23.
What is the percent by mass of sulfur in sulfur dioxide?
1. 54g
3. 110g
2. 55g
4. 206g
--------------
1. 32
3. 50
2. 33
4. 67
--------------
19.
Given the reaction: Ca + 2H2O → Ca(OH)2 + H2
What is the total number of moles of Ca needed to react
completely with 4.0 moles of H2O?
1. 1.0
3. 0.50
2. 2.0
4. 4.0
--------------
24.
Given the reaction: CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)
How many moles of oxygen are needed for the complete
combustion of 3.0 moles of CH4(g)?
1. 6.0 moles
3. 3.0 moles
2. 2.0 moles
4. 4.0 moles
--------------
20.
The percent by mass of Ca in CaCl2 is equal to
1. (40/111) × 100
3. (3/1) × 100
2. (111/40) × 100
4. (1/3) × 100
--------------
25.
How many moles of N2(g) would contain exactly 4.0 moles of
nitrogen atoms?
1. 1.0
3. 3.0
2. 2.0
4. 4.0
--------------
21.
What is the formula mass of Al2(SO4)3?
26.
1. 123
3. 214
What is the gram formula mass of (NH4)2SO4?
2. 150.
4. 342
--------------
1. 66.0 g
3. 114 g
2. 94.0 g
4. 132 g
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Chemical calculations review
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27.
32.
What is the percent by mass of nitrogen in the compound
NH4NO3 (formula mass = 80.)?
Given the unbalanced equation: N2(g) + H2(g) → NH3(g)
When the equation is balanced using the smallest whole-number
coefficients, the ratio of moles of hydrogen consumed to moles of
ammonia produced is
1. 5.7%
3. 29%
2. 18%
4. 35%
--------------
1. 1:3
3. 3:1
2. 2:3
4. 3:2
--------------
28.
What is the total mass in grams of 0.75 mole of SO2?
33.
1. 16 g
3. 32 g
An example of an empirical formula is
2. 24 g
4. 48 g
1.
2.
3.
4.
-------------29.
Given the reaction: 2Al + 3H2SO4 → 3H2 + Al2(SO4)3
The total number of moles of H2SO4 needed to react completely
with 5.0 moles of Al is
1. 2.5 moles
3. 7.5 moles
2. 5.0 moles
4. 9.0 moles
C4H10
C6H12O6
HC2H3O2
CH2O
--------------
34.
What is the empirical formula of the compound whose molecular
formula is P4O10?
1.
2.
3.
4.
-------------30.
PO
PO2
P 2O 5
P8O20
What is the total number of hydrogen atoms required to form one
molecule of C3H5(OH)3?
1. 1
3. 3
2. 5
4. 8
-------------35.
What is the gram formula mass of K2CO3?
-------------31.
1. 138 g
3. 99 g
2. 106 g
4. 67 g
--------------
What is the gram formula mass of Ca3(PO4)2?
1. 135 g/mol
3. 278 g/mol
2. 215 g/mol
4. 310. g/mol
--------------
36.
What is the percent by mass of oxygen in magnesium oxide,
MgO?
1. 20%
3. 50%
2. 40%
4. 60%
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Chemical calculations review
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37.
41.
Given the reaction: CH4 + 2O2 → CO2 + 2H2O
What amount of oxygen is needed to completely react with 1
mole of CH4?
Given the reaction: C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2(l)
How many moles of C6H12O6(s) are needed to produce 24 moles
of carbon dioxide?
1. 2 moles
3. 2 grams
1. 1.0 mole
3. 24 moles
2. 2 atoms
4. 2 molecules
2. 12 moles
4. 4.0 moles
--------------
--------------
38.
42.
If an equation is balanced properly, both sides of the equation
must have the same number of
What is the percent by mass of oxygen in Ca(OH)2? [formula
mass = 74.1]
1. atoms
3. molecules
1. 21.6%
3. 45.9%
2. coefficients
4. moles of molecules
2. 43.2%
4. 54.1%
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--------------
39.
43.
A hydrated salt is a solid that includes water molecules within its
crystal structure. A student heated a 9.10-gram sample of a
hydrated salt to a constant mass of 5.41 grams. What percent by
mass of water did the salt contain?
The gram-formula mass of (NH4)2CO3 is
1. 3.69%
3. 40.5%
2. 16.8%
4. 59.5%
1. 46.0 g
3. 78.0 g
2. 64.0 g
4. 96.0 g
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--------------
44.
40.
What is the total number of moles of atoms contained in 1 mole
of NH3?
Given the unbalanced equation:
1. 1 mole
3. 3 moles
2. 2 moles
4. 4 moles
What is the coefficient of O2 when the equation is balanced
correctly using the smallest whole-number coefficients?
1. 1
3. 3
2. 2
4. 4
-------------45.
Which equation is correctly balanced?
--------------
1.
2.
3.
4.
H2 + O2 → H2O
Ca + Cl2 → CaCl
2H2 + O2 → 2H2O
Ca + Cl2 → Ca2Cl
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Chemical calculations review
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46.
50.
What is the molecular formula of a compound that has a
molecular mass of 54 and the empirical formula C2H3?
Base your answer on the balanced chemical equation:
1.
2.
3.
4.
C2H3
C4H6
C6H9
C8H12
What is the total number of moles of O2 produced when 8 moles
of H2O is completely consumed?
--------------
Answer:
mol
--------------
47.
What is the empirical formula of a compound with the molecular
formula N2O4?
1.
2.
3.
4.
NO
NO2
N2O
N2O3
--------------
48.
Given the reaction:
What is the mole-to-mole ratio between nitrogen gas and
hydrogen gas?
1. 1:2
3. 2:2
2. 1:3
4. 2:3
--------------
49.
What is the empirical formula for the compound C6H12O6?
1.
2.
3.
4.
CH2O
C2H4O2
C3H6O3
C6H12O6
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Chemical calculations review
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Answer Key for Chemical calculations review
1. 4
18. 3
35. 1
2. 4
19. 2
36. 2
3. 2
20. 1
37. 1
4. 3
21. 4
38. 1
5. 4
22. 2
39. 3
6. 4
23. 3
40. 3
7. 2
24. 1
41. 4
8. 4
25. 2
42. 2
9. 4
26. 4
43. 4
10. 3
27. 4
44. 4
11. 3
28. 4
45. 3
12. 2
29. 3
46. 2
13. 1
30. 4
47. 2
14. 3
31. 4
48. 2
15. 1
32. 4
49. 1
16. 2
33. 4
50. 4
17. 2
34. 3
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