Question

determine the type of reaction.
synthesis, decomposition, single replacement, double replacement,or combustic
list type of reaction:

1. __ li₃n + nh₄no₃ → lino₃ + __ (nh₄)₃n double replacement
2. __ pb + h₃po₄ → h₂ + __ pb₃(po₄)₂
3. __ c₅h₉o + o₂ → co₂ + __ h₂o
4. __ nh₃+ h₂so₄ → __ (nh₄)₂so₄
5. __ nabr + ca(oh)₂ → cabr₂ + __ naoh
6. __ hbr + al(oh)₃ → h₂o + __ albr₃
7. __ n₂ + h₂ → __ nh₃
8. __ kclo₃ → kcl + __ o₂
9. __ nacl + f₂ → naf + __ cl₂
10. __ h₂ + o₂ → __ h₂o
11. __ pb(oh)₂ + hcl → h₂o + __ pbcl₂
12. __ albr₃ + k₂so₄ → kbr + __ al₂(so₄)₃
13. __ ch₄ + o₂ → co₂ + __ h₂o

Explanation:

Step1: Balance & classify reaction 2

Balance: $3\text{Pb} + 2\text{H}_3\text{PO}_4
ightarrow 3\text{H}_2 + \text{Pb}_3(\text{PO}_4)_2$
Type: Single Replacement (metal replaces H in acid)

Step2: Balance & classify reaction 3

Balance: $4\text{C}_5\text{H}_9\text{O} + 27\text{O}_2
ightarrow 20\text{CO}_2 + 18\text{H}_2\text{O}$
Type: Combustion (reacts with $\text{O}_2$ to form $\text{CO}_2/\text{H}_2\text{O}$)

Step3: Balance & classify reaction 4

Balance: $2\text{NH}_3 + \text{H}_2\text{SO}_4
ightarrow (\text{NH}_4)_2\text{SO}_4$
Type: Synthesis (two reactants form one product)

Step4: Balance & classify reaction 5

Balance: $2\text{NaBr} + \text{Ca(OH)}_2
ightarrow \text{CaBr}_2 + 2\text{NaOH}$
Type: Double Replacement (cations/anions swap)

Step5: Balance & classify reaction 6

Balance: $3\text{HBr} + \text{Al(OH)}_3
ightarrow 3\text{H}_2\text{O} + \text{AlBr}_3$
Type: Double Replacement (acid-base neutralization)

Step6: Balance & classify reaction 7

Balance: $\text{N}_2 + 3\text{H}_2
ightarrow 2\text{NH}_3$
Type: Synthesis (two elements form a compound)

Step7: Balance & classify reaction 8

Balance: $2\text{KClO}_3
ightarrow 2\text{KCl} + 3\text{O}_2$
Type: Decomposition (one reactant breaks down)

Step8: Balance & classify reaction 9

Balance: $2\text{NaCl} + \text{F}_2
ightarrow 2\text{NaF} + \text{Cl}_2$
Type: Single Replacement (halogen replaces another halogen)

Step9: Balance & classify reaction 10

Balance: $2\text{H}_2 + \text{O}_2
ightarrow 2\text{H}_2\text{O}$
Type: Synthesis (two elements form a compound)

Step10: Balance & classify reaction 11

Balance: $\text{Pb(OH)}_2 + 2\text{HCl}
ightarrow 2\text{H}_2\text{O} + \text{PbCl}_2$
Type: Double Replacement (acid-base neutralization)

Step11: Balance & classify reaction 12

Balance: $2\text{AlBr}_3 + 3\text{K}_2\text{SO}_4
ightarrow 6\text{KBr} + \text{Al}_2(\text{SO}_4)_3$
Type: Double Replacement (cations/anions swap)

Step12: Balance & classify reaction 13

Balance: $\text{CH}_4 + 2\text{O}_2
ightarrow \text{CO}_2 + 2\text{H}_2\text{O}$
Type: Combustion (hydrocarbon reacts with $\text{O}_2$)

Answer:

1. $\boldsymbol{1\text{Li}_3\text{N} + 3\text{NH}_4\text{NO}_3

ightarrow 3\text{LiNO}_3 + 1(\text{NH}_4)_3\text{N}}$; Double Replacement

1. $\boldsymbol{3\text{Pb} + 2\text{H}_3\text{PO}_4

ightarrow 3\text{H}_2 + 1\text{Pb}_3(\text{PO}_4)_2}$; Single Replacement

1. $\boldsymbol{4\text{C}_5\text{H}_9\text{O} + 27\text{O}_2

ightarrow 20\text{CO}_2 + 18\text{H}_2\text{O}}$; Combustion

1. $\boldsymbol{2\text{NH}_3 + 1\text{H}_2\text{SO}_4

ightarrow 1(\text{NH}_4)_2\text{SO}_4}$; Synthesis

1. $\boldsymbol{2\text{NaBr} + 1\text{Ca(OH)}_2

ightarrow 1\text{CaBr}_2 + 2\text{NaOH}}$; Double Replacement

1. $\boldsymbol{3\text{HBr} + 1\text{Al(OH)}_3

ightarrow 3\text{H}_2\text{O} + 1\text{AlBr}_3}$; Double Replacement

1. $\boldsymbol{1\text{N}_2 + 3\text{H}_2

ightarrow 2\text{NH}_3}$; Synthesis

1. $\boldsymbol{2\text{KClO}_3

ightarrow 2\text{KCl} + 3\text{O}_2}$; Decomposition

1. $\boldsymbol{2\text{NaCl} + 1\text{F}_2

ightarrow 2\text{NaF} + 1\text{Cl}_2}$; Single Replacement

1. $\boldsymbol{2\text{H}_2 + 1\text{O}_2

ightarrow 2\text{H}_2\text{O}}$; Synthesis

1. $\boldsymbol{1\text{Pb(OH)}_2 + 2\text{HCl}

ightarrow 2\text{H}_2\text{O} + 1\text{PbCl}_2}$; Double Replacement

1. $\boldsymbol{2\text{AlBr}_3 + 3\text{K}_2\text{SO}_4

ightarrow 6\text{KBr} + 1\text{Al}_2(\text{SO}_4)_3}$; Double Replacement

1. $\boldsymbol{1\text{CH}_4 + 2\text{O}_2

ightarrow 1\text{CO}_2 + 2\text{H}_2\text{O}}$; Combustion