balance the reactions and state the type of reaction described.
1. sodium metal reacts vigorously with water giving off a gas.
2. hydrogen chloride gas is commercially made by reacting table salt with sulfuric acid.
3. molten iron produced by the highly exothermic thermite reaction was used to weld railroad rails.

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Accepted Answer

# Explanation:
## Step1: Analyze the first reaction
Sodium ($Na$) reacts with water ($H_2O$). The un - balanced equation is $Na(s)+H_2O(l)
ightarrow H_2(g)+NaOH(aq)$.
For sodium: On the left - hand side, there is 1 $Na$ atom, and on the right - hand side, there is 1 $Na$ atom in $NaOH$.
For hydrogen: On the left - hand side, there are 2 $H$ atoms in $H_2O$, and on the right - hand side, there are 3 $H$ atoms ($2$ in $H_2$ and $1$ in $NaOH$).
For oxygen: On the left - hand side, there is 1 $O$ atom in $H_2O$, and on the right - hand side, there is 1 $O$ atom in $NaOH$.
We start by balancing hydrogen. If we put a coefficient of $2$ in front of $Na$ and $2$ in front of $H_2O$ and $2$ in front of $NaOH$, the equation becomes $2Na(s)+2H_2O(l)
ightarrow H_2(g)+2NaOH(aq)$. Now, for sodium: $2$ on the left and $2$ on the right. For hydrogen: $4$ on the left ($2\times2$ from $H_2O$) and $4$ on the right ($2$ from $H_2$ and $2$ from $2NaOH$). For oxygen: $2$ on the left ($2\times1$ from $H_2O$) and $2$ on the right ($2\times1$ from $2NaOH$).

## Step2: Analyze the second reaction
Hydrogen chloride ($HCl$) is made by reacting table salt ($NaCl$) with sulfuric acid ($H_2SO_4$). The un - balanced equation is $NaCl(s)+H_2SO_4(aq)
ightarrow HCl(g)+Na_2SO_4(aq)$.
For sodium: $1$ on the left and $2$ on the right.
For chlorine: $1$ on the left and $1$ on the right.
For hydrogen: $2$ on the left and $1$ on the right.
For sulfur: $1$ on the left and $1$ on the right.
For oxygen: $4$ on the left and $4$ on the right.
We put a coefficient of $2$ in front of $NaCl$ and $2$ in front of $HCl$. The balanced equation is $2NaCl(s)+H_2SO_4(aq)
ightarrow 2HCl(g)+Na_2SO_4(aq)$

## Step3: Analyze the third reaction
The thermite reaction $Al + Fe_2O_3
ightarrow Fe+Al_2O_3$.
For aluminum: $1$ on the left and $2$ on the right.
For iron: $2$ on the left and $1$ on the right.
For oxygen: $3$ on the left and $3$ on the right.
We put a coefficient of $2$ in front of $Al$ and $2$ in front of $Fe$. The balanced equation is $2Al(s)+Fe_2O_3(s)
ightarrow 2Fe(l)+Al_2O_3(s)$

# Answer:
1. $2Na(s)+2H_2O(l)
ightarrow H_2(g)+2NaOH(aq)$
2. $2NaCl(s)+H_2SO_4(aq)
ightarrow 2HCl(g)+Na_2SO_4(aq)$
3. $2Al(s)+Fe_2O_3(s)
ightarrow 2Fe(l)+Al_2O_3(s)$

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Explanation:

Step1: Analyze the first reaction

Step2: Analyze the second reaction

Step3: Analyze the third reaction

Answer: