How many number of oxygen molecules are required to produce 220 mg of CO2 according to the reaction? C + O2 CO2

To determine the number of oxygen molecules required to produce 220 mg of $\mathrm{CO}{}_2$, follow these steps:

1. Convert mass of $\mathrm{CO}{}_2$ to moles: Molar mass of $\mathrm{CO}{}_2=12+2\times 16=44$ g/mol. Mass of $\mathrm{CO}{}_2=220$ mg = $0.220$ g. Moles of $\mathrm{CO}{}_2=\frac{0.220}{44}=0.005$ mol.

2. Use stoichiometry from the balanced equation: $\mathrm{C}+\mathrm{O}{}_2\to \mathrm{CO}{}_2$ 1 mole of $\mathrm{CO}{}_2$ requires 1 mole of $\mathrm{O}{}_2$. Thus, 0.005 mol of $\mathrm{CO}{}_2$ requires 0.005 mol of $\mathrm{O}{}_2$.

3. Convert moles of $\mathrm{O}{}_2$ to molecules: Avogadro’s number = $6.022\times 10^{23}$ molecules/mol. Number of $\mathrm{O}{}_2$ molecules = $0.005\times 6.022\times 10^{23}=3.011\times 10^{21}$ molecules.

Final answer: $3.01\times 10^{21}$ oxygen molecules are required.