Question 1
Write the balanced equation for nitrogen gas, N
2
(g), reacting with hydrogen gas, H
2
(g), to form ammonia, NH
3
(g).
N
2
(g) + H
2
(g) → 2NH
3
(g)
3N
2
(g) + H
2
(g) → 2NH
3
(g)
N
2
(g) + 3H
2
(g) → 2NH
3
(g)
None of the above.
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Question 2
Write the balanced equation for methane gas, CH
4
(g), reacting with oxygen gas, O
2
(g), to form carbon dioxide gas, CO
2
(g), and gaseous water, H
2
O(g).
CH
4
(g) + 2O
2
(g) → CO
2
(g) + 2H
2
O(g)
2CH
4
(g) + 2O
2
(g) → CO
2
(g) + 2H
2
O(g)
2CH
4
(g) + 3O
2
(g) → 2CO
2
(g) + H
2
O(g)
None of the above.
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Question 3
Write the balanced equation for solid sodium, Na(s), combined with chlorine gas, Cl
2
(g), to form sodium chloride, NaCl(s).
Na(s) + ˝Cl
2
(g) → NaCl(s)
2Na(s) + Cl
2
(g) → 2NaCl(s)
4Na(s) + 2Cl
2
(g) → 4NaCl(s)
All of the above.
None of the above.
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Question 4
Write the balanced equation for nitrogen gas, N
2
(g), reacting with hydrogen gas, H
2
(g), to form ammonia, NH
3
(g).
3N
2
(g) + H
2
(g) → 2NH
3
(g)
3N
2
(g) + 7H
2
(g) → 6NH
3
(g)
⅓
N
2
(g) + H
2
(g) →
⅔
NH
3
(g)
All of the above.
None of the above.
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Question 5
What is the correct mole ratio between Na(s) and Cl
2
(g) when solid sodium, Na(s), is combined with chlorine gas, Cl
2
(g), to form sodium chloride, NaCl(s)?
1:1
2:1
1:2
3:1
1:3
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Question 6
What is the correct mole ratio between Na(s) and NaCl(s) when solid sodium, Na(s), is combined with chlorine gas, Cl
2
(g), to form sodium chloride, NaCl(s)?
1:1
2:1
1:2
3:1
Skip.
Question 7
What is the correct mole ratio between Cl
2
(g) and NaCl(s) when solid sodium, Na(s), is combined with chlorine gas, Cl
2
(g), to form sodium chloride, NaCl(s)?
1:1
2:1
1:2
3:1
Skip.
Question 8
What is the mole ratio between N
2
(g) and H
2
(g) when nitrogen gas, N
2
(g), is reacted with hydrogen gas, H
2
(g), to form ammonia, NH
3
(g).
1:1
2:1
1:2
3:1
1:3
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Question 9
What is the mole ratio between CH
4
(g) and CO
2
(g) when methane gas, CH
4
(g), is reacted with oxygen gas, O
2
(g), to form carbon dioxide gas, CO
2
(g), and gaseous water, H
2
O(g)?
1:1
1:2
2:1
3:1
1:3
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Question 10
Write the balanced equation for solid potassium, K(s), combined with iodine gas, I
2
(g), to form potassium iodide, KI(s).
K(s) + I
2
(g) → KI(s)
K(s) + 2I
2
(g) → KI(s)
2K(s) + I
2
(g) → 2KI(s)
All of the above.
None of the above.
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Question 11
Write the balanced equation for iron solid, Fe(s), reacting with oxygen gas, O
2
(g), to form solid iron(III)oxide, Fe
2
O
3
(s).
3Fe(s) + 2O
2
(g) → Fe
2
O
3
(s)
2Fe(s) + 3O
2
(g) → Fe
2
O
3
(s)
4Fe(s) + 3O
2
(g) → 2Fe
2
O
3
(s)
All of the above.
None of the above.
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Question 12
What are the correct mole ratios between: K(s) and I
2
(g), K(s) and KI(s), I
2
(g) and KI(s), when K(s) reacts with I
2
(g) to form KI(s)?
1:1, 1:1, 1:1
1:2, 1:1, 2:1
2:1, 2:2, 1:2
All of the above.
None of the above.
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Question 13
What are the correct mole ratios between: Fe(s) and O
2
(g), Fe(s) and Fe
2
O
3
(s), O
2
(g) and Fe
2
O
3
(s) when Fe(s) reacts with O
2
(g) to form Fe
2
O
3
(s)?
3:2, 3:1, 2:1
2:3, 2:1, 3:1
4:3, 4:2, 3:2
All of the above.
None of the above.
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Question 14
For nitrogen gas, N
2
(g) reacting with hydrogen gas, H
2
(g), to form ammonia, NH
3
(g):
One mole of N
2
(g) will react with three moles of H
2
(g) to produce two moles of NH
3
(g)
Three moles of N
2
(g) will react with nine moles of H
2
(g) to produce six moles of NH
3
(g)
Half of a mole of N
2
(g) will react with one and a half moles of H
2
(g) to produce one mole of NH
3
(g)
All of the above.
None of the above.
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Question 15
Chemical equations are a shorthand way of describing what happens when some initial reactants are converted to the final products.
True
False
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Question 16
During all chemical reactions the atoms that are initially combined to form the reactants are rearranged into new combinations that form the products.
True
False
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Question 17
Chemical equations provide mole ratios between reactants (when there is more than one reactant), between reactants and products, and between products (when there is more than one product).
True
False
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Question 18
The physical and chemical properties of the products are different from the physical and chemical properties of the reactants.
True
False
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Question 19
A balanced chemical equation assumes no left over reactants and accounts for all of the reactants that are used.
True
False
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Question 20
A chemical reaction is balanced when the number of atoms of each element in the reactants is equal to the number of atoms of each element in the products.
True
False
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Question 21
The balanced chemical equation gives mole ratios.
True
False
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Question 22
When balancing chemical equations we don't change the subscripts.
True
False
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