To create a balanced chemical equation for the reaction between solid magnesium and water to form magnesium hydroxide and hydrogen gas, we first need to write the unbalanced equation:
\[ \text{Mg (s)} + \text{H}_2\text{O (l)} \rightarrow \text{Mg(OH)}_2\text{ (s)} + \text{H}_2\text{ (g)} \]
Next, we will balance the equation.
- We start with one magnesium atom on each side.
- In the products, magnesium hydroxide contains two hydroxide ions (OH), so we need two water molecules to provide those hydroxide ions:
\[ \text{Mg (s)} + 2\text{H}_2\text{O (l)} \rightarrow \text{Mg(OH)}_2\text{ (s)} + \text{H}_2\text{ (g)} \]
Now, let's check:
- Reactants: 1 Mg, 4 H, 2 O
- Products: 1 Mg, 4 H, 2 O
The equation is balanced.
Type of Reaction
This reaction is classified as a single displacement reaction (or single replacement reaction) where magnesium displaces hydrogen in water, forming magnesium hydroxide and hydrogen gas. In this reaction, magnesium has a higher reactivity than the hydrogen in water, resulting in the release of hydrogen gas.
If you need a visual representation of the balancing process, you can create an image or diagram based on these steps. Unfortunately, I can't create or include images, but you could sketch out the reactants and products along with the balancing process using the information provided!
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