6.2 gm of Mg (At. mass 24) will produce MgO equal to:

Options

A. 40 mole
B. 1.2 mole
C. 0.26 mole
D. 0.35 mole

Explanation

To solve the problem of how much magnesium oxide (MgO) is produced from 6.2 grams of magnesium (Mg), follow these steps:

### Step 1: Write the Balanced Chemical Equation
The reaction of magnesium with oxygen can be represented as:
\[ 2 \text{Mg} + \text{O}_2 \rightarrow 2 \text{MgO} \]
From this equation, we can see that 1 mole of magnesium reacts with 0.5 moles of oxygen to produce 1 mole of magnesium oxide.

### Step 2: Calculate the Number of Moles of Magnesium
To find the number of moles of magnesium in 6.2 grams, use the formula:
\[ \text{Number of moles} = \frac{\text{Given mass (g)}}{\text{Molar mass (g/mol)}} \]
The molar mass of magnesium (Mg) is 24 g/mol. Thus,
\[ \text{Number of moles of Mg} = \frac{6.2 \text{ g}}{24 \text{ g/mol}} \]
Calculating this gives:
\[ \text{Number of moles of Mg} = 0.2583 \text{ moles} \approx 0.26 \text{ moles} \]

### Step 3: Relate Moles of Magnesium to Moles of Magnesium Oxide
From the balanced equation, we see that 1 mole of magnesium produces 1 mole of magnesium oxide. Therefore, the number of moles of magnesium oxide produced will be equal to the number of moles of magnesium used:
\[ \text{Number of moles of MgO} = \text{Number of moles of Mg} = 0.26 \text{ moles} \]

### Step 4: Conclusion
Thus, 6.2 grams of magnesium will produce 0.26 moles of magnesium oxide (MgO).

### Final Answer
The amount of magnesium oxide produced is **0.26 moles**.

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