Question

How many molecules of carbon dioxide are formed when 0.6 g carbon is burnt in air?

• A. 3.01 $\times$ 10$^{22}$
• B. 2.01 $\times$ 10$^{23}$
• C. 6.02 $\times$ 10$^{23}$
• D. 5.06 $\times$ 10$^{23}$

Hint:

To calculate the number of molecules produced in a chemical reaction, first determine the moles and then multiply by Avogadro's number.

Answer 1

The Correct Option is C

The molar mass of carbon (C) is 12 g/mol. First, calculate the moles of carbon: \[ \text{moles of C} = \frac{0.6 \, \text{g}}{12 \, \text{g/mol}} = 0.05 \, \text{mol} \] According to the balanced equation for the combustion of carbon: \[ C + O_2 \rightarrow CO_2 \] For every mole of carbon, one mole of CO2 is produced. Therefore, 0.05 moles of carbon will produce 0.05 moles of CO2. To find the number of molecules, multiply by Avogadro's number: \[ \text{molecules of CO}_2 = 0.05 \, \text{mol} \times 6.02 \times 10^{23} \, \text{molecules/mol} = 3.01 \times 10^{22} \, \text{molecules} \]