How much magnesium sulphide can be obtained from `2.00 g` of `Mg` and `2.00 g` of `S` by the reaction.
`Mg + S rarr MgS`. Which is the limiting reagent? Calculate the amount of one of the reactants which remains unreacted?

Explanation

To solve the problem of how much magnesium sulfide (MgS) can be obtained from 2.00 g of magnesium (Mg) and 2.00 g of sulfur (S), we will follow these steps:

### Step 1: Write the balanced chemical equation
The balanced chemical equation for the reaction is:
\[ \text{Mg} + \text{S} \rightarrow \text{MgS} \]

### Step 2: Calculate the number of moles of each reactant
To find the number of moles of magnesium and sulfur, we will use the formula:
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