Question

classify each chemical reaction: reaction type of reaction (check all that apply) 2h₂o(g) → 2h₂(g) + o₂(g) combination single replacement double replacement decomposition precipitation combustion acid - base hbr(aq) + naoh(aq) → nabr(aq) + h₂o(l) combination single replacement double replacement decomposition precipitation combustion acid - base 2ch₃(ch₂)₂ch₃(g) + 13o₂(g) → 8co₂(g) + 10h₂o(g) combination single replacement double replacement decomposition precipitation combustion acid - base koh(aq) + hbro(aq) → kbro(aq) + h₂o(l) combination single replacement double replacement decomposition precipitation combustion acid - base

Explanation:

Step1: Analyze first reaction

A single compound ($2H_2O$) breaks down into two simpler substances ($2H_2$ and $O_2$), which is decomposition.

Step2: Analyze second reaction

$HBr$ (acid) reacts with $NaOH$ (base) to form a salt ($NaBr$) and water ($H_2O$), an acid - base reaction. Also, the ions in the reactants exchange partners, a double - replacement reaction.

Step3: Analyze third reaction

A hydrocarbon ($2CH_3(CH_2)_2CH_3$) reacts with oxygen ($13O_2$) to produce carbon dioxide ($8CO_2$) and water ($10H_2O$), which is a combustion reaction.

Step4: Analyze fourth reaction

$KOH$ (base) reacts with $HBrO$ (acid) to form a salt ($KBrO$) and water ($H_2O$), an acid - base reaction. Also, the ions in the reactants exchange partners, a double - replacement reaction.

Answer:

$2H_2O(g)\to2H_2(g)+O_2(g)$: decomposition
$HBr(aq)+NaOH(aq)\to NaBr(aq)+H_2O(l)$: double replacement, acid - base
$2CH_3(CH_2)_2CH_3(g)+13O_2(g)\to8CO_2(g)+10H_2O(g)$: combustion
$KOH(aq)+HBrO(aq)\to KBrO(aq)+H_2O(l)$: double replacement, acid - base