Answer:
1) Decomposition
2)Double-replacement reaction
3)synthesis
4)Double-replacement reaction
5)single-replacement reaction
6)Double-replacement reaction
Explanation:
Step 1: Data given
Synthesis: This is a reaction where two or more reactants will combine to form a new, single product. This is occurs when two or more reactants combine to form a single product. This can be shown with the following equation.
A + B → C
A and B are the reactants to form a new product C
Decomposition: This is a reaction where 1 (more complex) compound will be broken down into 2 or more (more simple) products.
This can be shown by the following equation:
AB → A + B
A single replacement: This is a reaction where one element wil be replaced by another element in the same compound. This can be shown by the following equation:
A + BC → B + AC
Here is the elemnt B in the compound BC, replaced by the element A, to form a new compound AC
A double-replacement: This is a reaction where the positive and negative ions of two ionic compounds will be exchanged and 2 new compounds willbe formed. This can be shown by the following equation:
AB+CD→AD+BC
A combustion reaction requires oxygen gas (O2) to produce the products CO2 and H2O
Step 2:
1) 2HgO(s) → 2Hg(l) + O2(g)
⇒ Decomposition
2) KCl(aq) + AgNO3(aq) → AgCl(s) + KNO3(aq)
⇒ Double-replacement reaction
3) 2Na(s) + H2(g) → 2NaH(s)
⇒ synthesis
4) Mg(OH)2(aq) + 2HNO2(aq) → Mg(NO2)2(aq) + 2 H2O(l)
⇒ Double-replacement reaction
5) Ca(s) + 2AgNO3(aq) → Ca(NO3)2(aq) + Ag(s)
⇒ Single-replacement reaction
6) Al2O3(s) + H2SO4(aq) → Al2(SO4)3(aq) + H2O(l)
⇒ Double-replacement reaction
= 0.0725 = 
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