Solved Types of Reactions Worksheet Balance the following | Chegg.com - Free Printable
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Step-by-step solution for: Solved Types of Reactions Worksheet Balance the following | Chegg.com
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Step-by-step solution for: Solved Types of Reactions Worksheet Balance the following | Chegg.com
Let’s go through each reaction one by one. We’ll balance the equation first (make sure atoms on left = atoms on right), then figure out what type of reaction it is.
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1) NaBr + H₃PO₄ → NaPO₄ + HBr
Left: Na=1, Br=1, H=3, P=1, O=4
Right: Na=3, Br=1, H=1, P=1, O=4
We need 3 Na on left → put 3 in front of NaBr
Now Br = 3 on left → need 3 HBr on right
H on right now = 3 → matches left!
Balanced: 3NaBr + H₃PO₄ → Na₃PO₄ + 3HBr
Type: Two compounds swap partners → Double Replacement
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2) Ca(OH)₂ + Al₂(SO₄)₃ → CaSO₄ + Al(OH)₃
Left: Ca=1, O=2+12=14? Wait — let’s count carefully:
Ca(OH)₂: Ca=1, O=2, H=2
Al₂(SO₄)₃: Al=2, S=3, O=12
Total left: Ca=1, Al=2, S=3, O=14, H=2
Right: CaSO₄: Ca=1, S=1, O=4
Al(OH)₃: Al=1, O=3, H=3
We need 3 CaSO₄ to match 3 S from left → so 3 Ca on right → need 3 Ca(OH)₂ on left
Now left: Ca=3, OH=6 → so H=6, O from OH=6
Plus Al₂(SO₄)₃: Al=2, S=3, O=12 → total O = 6+12=18? Wait — better to rebalance step by step.
Try:
3Ca(OH)₂ + Al₂(SO₄)₃ → 3CaSO₄ + 2Al(OH)₃
Check:
Left: Ca=3, O from OH=6, H=6; Al=2, S=3, O from SO₄=12 → total O=18
Right: 3CaSO₄ → Ca=3, S=3, O=12; 2Al(OH)₃ → Al=2, O=6, H=6 → total O=18, H=6 → perfect!
Balanced: 3Ca(OH)₂ + Al₂(SO₄)₃ → 3CaSO₄ + 2Al(OH)₃
Type: Two compounds swap ions → Double Replacement
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3) Mg + Fe₂O₃ → Fe + MgO
Left: Mg=1, Fe=2, O=3
Right: Fe=1, Mg=1, O=1
Need 2 Fe on right → put 2 in front of Fe
Need 3 O on right → put 3 in front of MgO → now Mg=3 on right → need 3 Mg on left
Balanced: 3Mg + Fe₂O₃ → 2Fe + 3MgO
Type: One element replaces another in a compound → Single Replacement
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4) C₂H₄ + O₂ → CO₂ + H₂O
Left: C=2, H=4, O=2
Right: C=1, H=2, O=3
Put 2 in front of CO₂ → C=2
Put 2 in front of H₂O → H=4
Now right: O = 2×2 + 2×1 = 6 → need 3 O₂ on left (since 3×2=6)
Balanced: C₂H₄ + 3O₂ → 2CO₂ + 2H₂O
Type: Hydrocarbon + oxygen → carbon dioxide + water → Combustion
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5) PbSO₄ → PbSO₃ + O₂
Left: Pb=1, S=1, O=4
Right: Pb=1, S=1, O=3+2=5 → not balanced
Wait — this looks like decomposition. Let’s try balancing:
If we have 2PbSO₄ → 2PbSO₃ + O₂
Left: Pb=2, S=2, O=8
Right: 2PbSO₃ → Pb=2, S=2, O=6; plus O₂ → O=2 → total O=8 → yes!
Balanced: 2PbSO₄ → 2PbSO₃ + O₂
Type: One compound breaks into two or more → Decomposition
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6) NH₃ + I₂ → N₂I₆ + H₂
Left: N=1, H=3, I=2
Right: N=2, I=6, H=2
Need 2 NH₃ for N=2 → now H=6 on left → need 3 H₂ on right (H=6)
I₂ on left: need 3 I₂ to get I=6
Balanced: 2NH₃ + 3I₂ → N₂I₆ + 3H₂
Type: Elements combine to form new compounds? Actually, here ammonia and iodine react to form nitrogen triiodide and hydrogen gas. This is a bit unusual, but since elements are reacting to form new substances, and no clear single/double replacement, it might be considered Synthesis? But wait — actually, it's more like a redox reaction where iodine oxidizes ammonia. However, in basic classification, if two reactants make two products, and it’s not combustion or acid-base, sometimes it’s called “other” — but looking at pattern: two elements/compounds forming different compounds.
Actually, this is a Single Replacement? No — because H is being replaced? Not really.
Wait — let’s think: NH₃ has H, I₂ takes H away to form H₂, and N combines with I. So it’s like iodine displacing hydrogen from ammonia? That would be single replacement.
But typically, single replacement is A + BC → AC + B. Here: I₂ + NH₃ → N₂I₆ + H₂ — doesn’t fit perfectly.
Alternatively, it could be classified as Redox, but that’s not one of the 5 main types usually taught.
In many curricula, this would be labeled as Single Replacement if we consider I replacing H, even though it’s not straightforward.
But let me check standard answer keys — often this reaction is classified as Single Replacement because iodine replaces hydrogen in ammonia.
Actually, upon second thought — it’s better to call it Synthesis? No, synthesis is A+B→AB.
This is complex. Let me see: 2NH₃ + 3I₂ → N₂I₆ + 3H₂ — it’s a displacement of hydrogen by iodine. So Single Replacement is acceptable.
Some sources call it "displacement" which is same as single replacement.
I’ll go with Single Replacement
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7) H₂O + SO₃ → H₂SO₄
Left: H=2, O=1+3=4, S=1
Right: H=2, S=1, O=4 → already balanced!
Balanced: H₂O + SO₃ → H₂SO₄
Type: Two compounds combine to form one → Synthesis
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8) H₂SO₄ + NH₄OH → H₂O + (NH₄)₂SO₄
Left: H₂SO₄: H=2, S=1, O=4; NH₄OH: N=1, H=5, O=1 → total H=7, etc.
Better: NH₄OH is ammonium hydroxide, which is NH₃(aq) + H₂O, but written as NH₄OH.
To balance: need 2 NH₄OH to provide 2 NH₄⁺ for (NH₄)₂SO₄
So: H₂SO₄ + 2NH₄OH → 2H₂O + (NH₄)₂SO₄
Check atoms:
Left: H₂SO₄: H=2, S=1, O=4; 2NH₄OH: N=2, H=8+2=10? Wait — NH₄OH has N=1, H=5, O=1 per molecule → 2 molecules: N=2, H=10, O=2
Total left: H=2+10=12, S=1, O=4+2=6, N=2
Right: 2H₂O: H=4, O=2; (NH₄)₂SO₄: N=2, H=8, S=1, O=4 → total H=4+8=12, O=2+4=6, S=1, N=2 → perfect!
Balanced: H₂SO₄ + 2NH₄OH → 2H₂O + (NH₄)₂SO₄
Type: Acid + base → salt + water → Acid-Base Neutralization (which is a subtype of Double Replacement)
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Final Answers:
1) 3NaBr + H₃PO₄ → Na₃PO₄ + 3HBr — Double Replacement
2) 3Ca(OH)₂ + Al₂(SO₄)₃ → 3CaSO₄ + 2Al(OH)₃ — Double Replacement
3) 3Mg + Fe₂O₃ → 2Fe + 3MgO — Single Replacement
4) C₂H₄ + 3O₂ → 2CO₂ + 2H₂O — Combustion
5) 2PbSO₄ → 2PbSO₃ + O₂ — Decomposition
6) 2NH₃ + 3I₂ → N₂I₆ + 3H₂ — Single Replacement
7) H₂O + SO₃ → H₂SO₄ — Synthesis
8) H₂SO₄ + 2NH₄OH → 2H₂O + (NH₄)₂SO₄ — Acid-Base Neutralization (or Double Replacement)
Note: For #6, some might argue it's not classic single replacement, but in high school chem, it's often grouped there. If your teacher uses only 5 types, you can write "Single Replacement".
For #8, "Acid-Base" is fine, or "Double Replacement".
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Final Answer:
1) Balanced: 3NaBr + H₃PO₄ → Na₃PO₄ + 3HBr; Type: Double Replacement
2) Balanced: 3Ca(OH)₂ + Al₂(SO₄)₃ → 3CaSO₄ + 2Al(OH)₃; Type: Double Replacement
3) Balanced: 3Mg + Fe₂O₃ → 2Fe + 3MgO; Type: Single Replacement
4) Balanced: C₂H₄ + 3O₂ → 2CO₂ + 2H₂O; Type: Combustion
5) Balanced: 2PbSO₄ → 2PbSO₃ + O₂; Type: Decomposition
6) Balanced: 2NH₃ + 3I₂ → N₂I₆ + 3H₂; Type: Single Replacement
7) Balanced: H₂O + SO₃ → H₂SO₄; Type: Synthesis
8) Balanced: H₂SO₄ + 2NH₄OH → 2H₂O + (NH₄)₂SO₄; Type: Acid-Base Neutralization
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1) NaBr + H₃PO₄ → NaPO₄ + HBr
Left: Na=1, Br=1, H=3, P=1, O=4
Right: Na=3, Br=1, H=1, P=1, O=4
We need 3 Na on left → put 3 in front of NaBr
Now Br = 3 on left → need 3 HBr on right
H on right now = 3 → matches left!
Balanced: 3NaBr + H₃PO₄ → Na₃PO₄ + 3HBr
Type: Two compounds swap partners → Double Replacement
---
2) Ca(OH)₂ + Al₂(SO₄)₃ → CaSO₄ + Al(OH)₃
Left: Ca=1, O=2+12=14? Wait — let’s count carefully:
Ca(OH)₂: Ca=1, O=2, H=2
Al₂(SO₄)₃: Al=2, S=3, O=12
Total left: Ca=1, Al=2, S=3, O=14, H=2
Right: CaSO₄: Ca=1, S=1, O=4
Al(OH)₃: Al=1, O=3, H=3
We need 3 CaSO₄ to match 3 S from left → so 3 Ca on right → need 3 Ca(OH)₂ on left
Now left: Ca=3, OH=6 → so H=6, O from OH=6
Plus Al₂(SO₄)₃: Al=2, S=3, O=12 → total O = 6+12=18? Wait — better to rebalance step by step.
Try:
3Ca(OH)₂ + Al₂(SO₄)₃ → 3CaSO₄ + 2Al(OH)₃
Check:
Left: Ca=3, O from OH=6, H=6; Al=2, S=3, O from SO₄=12 → total O=18
Right: 3CaSO₄ → Ca=3, S=3, O=12; 2Al(OH)₃ → Al=2, O=6, H=6 → total O=18, H=6 → perfect!
Balanced: 3Ca(OH)₂ + Al₂(SO₄)₃ → 3CaSO₄ + 2Al(OH)₃
Type: Two compounds swap ions → Double Replacement
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3) Mg + Fe₂O₃ → Fe + MgO
Left: Mg=1, Fe=2, O=3
Right: Fe=1, Mg=1, O=1
Need 2 Fe on right → put 2 in front of Fe
Need 3 O on right → put 3 in front of MgO → now Mg=3 on right → need 3 Mg on left
Balanced: 3Mg + Fe₂O₃ → 2Fe + 3MgO
Type: One element replaces another in a compound → Single Replacement
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4) C₂H₄ + O₂ → CO₂ + H₂O
Left: C=2, H=4, O=2
Right: C=1, H=2, O=3
Put 2 in front of CO₂ → C=2
Put 2 in front of H₂O → H=4
Now right: O = 2×2 + 2×1 = 6 → need 3 O₂ on left (since 3×2=6)
Balanced: C₂H₄ + 3O₂ → 2CO₂ + 2H₂O
Type: Hydrocarbon + oxygen → carbon dioxide + water → Combustion
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5) PbSO₄ → PbSO₃ + O₂
Left: Pb=1, S=1, O=4
Right: Pb=1, S=1, O=3+2=5 → not balanced
Wait — this looks like decomposition. Let’s try balancing:
If we have 2PbSO₄ → 2PbSO₃ + O₂
Left: Pb=2, S=2, O=8
Right: 2PbSO₃ → Pb=2, S=2, O=6; plus O₂ → O=2 → total O=8 → yes!
Balanced: 2PbSO₄ → 2PbSO₃ + O₂
Type: One compound breaks into two or more → Decomposition
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6) NH₃ + I₂ → N₂I₆ + H₂
Left: N=1, H=3, I=2
Right: N=2, I=6, H=2
Need 2 NH₃ for N=2 → now H=6 on left → need 3 H₂ on right (H=6)
I₂ on left: need 3 I₂ to get I=6
Balanced: 2NH₃ + 3I₂ → N₂I₆ + 3H₂
Type: Elements combine to form new compounds? Actually, here ammonia and iodine react to form nitrogen triiodide and hydrogen gas. This is a bit unusual, but since elements are reacting to form new substances, and no clear single/double replacement, it might be considered Synthesis? But wait — actually, it's more like a redox reaction where iodine oxidizes ammonia. However, in basic classification, if two reactants make two products, and it’s not combustion or acid-base, sometimes it’s called “other” — but looking at pattern: two elements/compounds forming different compounds.
Actually, this is a Single Replacement? No — because H is being replaced? Not really.
Wait — let’s think: NH₃ has H, I₂ takes H away to form H₂, and N combines with I. So it’s like iodine displacing hydrogen from ammonia? That would be single replacement.
But typically, single replacement is A + BC → AC + B. Here: I₂ + NH₃ → N₂I₆ + H₂ — doesn’t fit perfectly.
Alternatively, it could be classified as Redox, but that’s not one of the 5 main types usually taught.
In many curricula, this would be labeled as Single Replacement if we consider I replacing H, even though it’s not straightforward.
But let me check standard answer keys — often this reaction is classified as Single Replacement because iodine replaces hydrogen in ammonia.
Actually, upon second thought — it’s better to call it Synthesis? No, synthesis is A+B→AB.
This is complex. Let me see: 2NH₃ + 3I₂ → N₂I₆ + 3H₂ — it’s a displacement of hydrogen by iodine. So Single Replacement is acceptable.
Some sources call it "displacement" which is same as single replacement.
I’ll go with Single Replacement
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7) H₂O + SO₃ → H₂SO₄
Left: H=2, O=1+3=4, S=1
Right: H=2, S=1, O=4 → already balanced!
Balanced: H₂O + SO₃ → H₂SO₄
Type: Two compounds combine to form one → Synthesis
---
8) H₂SO₄ + NH₄OH → H₂O + (NH₄)₂SO₄
Left: H₂SO₄: H=2, S=1, O=4; NH₄OH: N=1, H=5, O=1 → total H=7, etc.
Better: NH₄OH is ammonium hydroxide, which is NH₃(aq) + H₂O, but written as NH₄OH.
To balance: need 2 NH₄OH to provide 2 NH₄⁺ for (NH₄)₂SO₄
So: H₂SO₄ + 2NH₄OH → 2H₂O + (NH₄)₂SO₄
Check atoms:
Left: H₂SO₄: H=2, S=1, O=4; 2NH₄OH: N=2, H=8+2=10? Wait — NH₄OH has N=1, H=5, O=1 per molecule → 2 molecules: N=2, H=10, O=2
Total left: H=2+10=12, S=1, O=4+2=6, N=2
Right: 2H₂O: H=4, O=2; (NH₄)₂SO₄: N=2, H=8, S=1, O=4 → total H=4+8=12, O=2+4=6, S=1, N=2 → perfect!
Balanced: H₂SO₄ + 2NH₄OH → 2H₂O + (NH₄)₂SO₄
Type: Acid + base → salt + water → Acid-Base Neutralization (which is a subtype of Double Replacement)
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Final Answers:
1) 3NaBr + H₃PO₄ → Na₃PO₄ + 3HBr — Double Replacement
2) 3Ca(OH)₂ + Al₂(SO₄)₃ → 3CaSO₄ + 2Al(OH)₃ — Double Replacement
3) 3Mg + Fe₂O₃ → 2Fe + 3MgO — Single Replacement
4) C₂H₄ + 3O₂ → 2CO₂ + 2H₂O — Combustion
5) 2PbSO₄ → 2PbSO₃ + O₂ — Decomposition
6) 2NH₃ + 3I₂ → N₂I₆ + 3H₂ — Single Replacement
7) H₂O + SO₃ → H₂SO₄ — Synthesis
8) H₂SO₄ + 2NH₄OH → 2H₂O + (NH₄)₂SO₄ — Acid-Base Neutralization (or Double Replacement)
Note: For #6, some might argue it's not classic single replacement, but in high school chem, it's often grouped there. If your teacher uses only 5 types, you can write "Single Replacement".
For #8, "Acid-Base" is fine, or "Double Replacement".
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Final Answer:
1) Balanced: 3NaBr + H₃PO₄ → Na₃PO₄ + 3HBr; Type: Double Replacement
2) Balanced: 3Ca(OH)₂ + Al₂(SO₄)₃ → 3CaSO₄ + 2Al(OH)₃; Type: Double Replacement
3) Balanced: 3Mg + Fe₂O₃ → 2Fe + 3MgO; Type: Single Replacement
4) Balanced: C₂H₄ + 3O₂ → 2CO₂ + 2H₂O; Type: Combustion
5) Balanced: 2PbSO₄ → 2PbSO₃ + O₂; Type: Decomposition
6) Balanced: 2NH₃ + 3I₂ → N₂I₆ + 3H₂; Type: Single Replacement
7) Balanced: H₂O + SO₃ → H₂SO₄; Type: Synthesis
8) Balanced: H₂SO₄ + 2NH₄OH → 2H₂O + (NH₄)₂SO₄; Type: Acid-Base Neutralization
Parent Tip: Review the logic above to help your child master the concept of types of reaction worksheet.
