Question

classify each reaction below as either formation, decomposition, replacement (single or double), or combustion. note that the equations are not balanced.

1. nh₃ + hcl → nh₄cl
2. c₁₂h₂₂o₁₁ + o₂ → co₂ + h₂o
3. al₂s₃ → al + s
4. naoh + cuso₄ → na₂so₄ + cu(oh)₂
5. fe + o₂ → fe₂o₃
6. cl₂ + kbr → kcl + br₂
7. nh₄no₃ → n₂o + h₂o
8. mg₃(po₄)₂ + h₂ → mg + h₃po₄
9. c₄h₁₂ + o₂ → h₂o + co₂
10. alcl₃ + na₂so₄ → al₂(so₄)₃ + nacl

Explanation:

Step1: Recall reaction - type definitions

Formation reaction: two or more substances combine to form one product. Decomposition reaction: one substance breaks down into two or more substances. Replacement reaction: a more reactive element replaces a less reactive element in a compound (single - replacement) or the positive and negative ions in two ionic compounds exchange places (double - replacement). Combustion reaction: a substance reacts with oxygen, usually producing carbon dioxide and water.

Step2: Analyze reaction 6

In the reaction $Cl_2+KBr
ightarrow KCl + Br_2$, chlorine ($Cl_2$) is a more reactive non - metal than bromine ($Br_2$). Chlorine replaces bromine in potassium bromide ($KBr$), so it is a single - replacement reaction.

Step3: Analyze reaction 7

In the reaction $NH_4NO_3
ightarrow N_2O + H_2O$, ammonium nitrate ($NH_4NO_3$) breaks down into dinitrogen monoxide ($N_2O$) and water ($H_2O$), so it is a decomposition reaction.

Step4: Analyze reaction 8

In the reaction $Mg_3(PO_4)_2+H_2
ightarrow Mg + H_3PO_4$, hydrogen ($H_2$) replaces magnesium ($Mg$) in magnesium phosphate ($Mg_3(PO_4)_2$), so it is a single - replacement reaction.

Answer:

1. Single - replacement
2. Decomposition
3. Single - replacement