Questions: If 4.9 kg of CO2 are produced during a combustion reaction, how many molecules of CO2 would be produced?

Solution Steps

The molar mass of CO\(_2\) can be calculated by summing the atomic masses of carbon (C) and oxygen (O):

• Atomic mass of C: 12.01 g/mol
• Atomic mass of O: 16.00 g/mol

Since CO\(_2\) has one carbon atom and two oxygen atoms: \[ \text{Molar mass of CO}_2 = 12.01 \, \text{g/mol} + 2 \times 16.00 \, \text{g/mol} = 44.01 \, \text{g/mol} \]

Given the mass of CO\(_2\) is 4.9 kg, we first convert this to grams: \[ 4.9 \, \text{kg} = 4900 \, \text{g} \]

Next, we use the molar mass to convert grams to moles: \[ \text{Moles of CO}_2 = \frac{4900 \, \text{g}}{44.01 \, \text{g/mol}} = 111.34 \, \text{mol} \]

Using Avogadro's number, which is \(6.022 \times 10^{23}\) molecules/mol, we convert moles to molecules: \[ \text{Molecules of CO}_2 = 111.34 \, \text{mol} \times 6.022 \times 10^{23} \, \text{molecules/mol} = 6.703 \times 10^{25} \, \text{molecules} \]

Final Answer