0.6 g of carbon was burnt in the air to form `CO_(2)`. The number of molecules of `CO_(2)` introduced into the will be : `C+O_(2)toCO_(2)`

Options

A. (a)`6.02xx10^(23`
B. (b)`3.01 xx10^(23)`
C. (c)`6.02xx10^(22)`
D. (d)`3.01xx10^(22)`

Answer

To solve the problem of how many molecules of CO₂ are produced from the combustion of 0.6 g of carbon, we can follow these steps:

### Step 1: Write the balanced chemical equation
The reaction for the combustion of carbon in air is:
\[ C + O_2 \rightarrow CO_2 \]
From this equation, we can see that 1 mole of carbon produces 1 mole of carbon dioxide (CO₂).

### Step 2: Calculate the number of moles of carbon
To find the number of moles of carbon, we use the formula:
\[ \text{Number of moles} = \frac{\text{mass (g)}}{\text{molar mass (g/mol)}} \]
The molar mass of carbon (C) is 12 g/mol. Given that we have 0.6 g of carbon:
\[ \text{Number of moles of carbon} = \frac{0.6 \, \text{g}}{12 \, \text{g/mol}} = 0.05 \, \text{moles} \]

### Step 3: Determine the number of moles of CO₂ produced
From the balanced equation, we know that 1 mole of carbon produces 1 mole of CO₂. Therefore, the number of moles of CO₂ produced is the same as the number of moles of carbon:
\[ \text{Number of moles of CO₂} = 0.05 \, \text{moles} \]

### Step 4: Calculate the number of molecules of CO₂
To find the number of molecules, we use Avogadro's number, which is approximately \( 6.02 \times 10^{23} \) molecules/mole. The formula is:
\[ \text{Number of molecules} = \text{Number of moles} \times \text{Avogadro's number} \]
Substituting the values we have:
\[ \text{Number of molecules of CO₂} = 0.05 \, \text{moles} \times 6.02 \times 10^{23} \, \text{molecules/mole} \]
\[ \text{Number of molecules of CO₂} = 3.01 \times 10^{22} \, \text{molecules} \]

### Final Answer
The number of molecules of CO₂ produced from burning 0.6 g of carbon is:
\[ 3.01 \times 10^{22} \, \text{molecules} \]

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