What volume of carbon (II) oxide is produced by reacting excess carbon with \( 10 \mathrm{dm}^{3} \) of oxygen?

To find the volume of carbon (II) oxide (CO) produced when reacting with oxygen, we start with the balanced chemical equation: \[ 2C + O_2 \rightarrow 2CO \] From the equation, we see that 1 mole of \( O_2 \) produces 2 moles of \( CO \). Under normal conditions, 1 mole of gas occupies 22.4 dm³. Since you have \( 10 \mathrm{dm}^{3} \) of oxygen, you first find the moles of \( O_2 \): \[ \text{Moles of } O_2 = \frac{10 \, \text{dm}^3}{22.4 \, \text{dm}^3/\text{mol}} \approx 0.446 \, \text{mol} \] Given that 1 mol of \( O_2 \) produces 2 moles of \( CO \): \[ \text{Moles of } CO = 2 \times 0.446 \, \text{mol} \approx 0.892 \, \text{mol} \] Finally, the volume of \( CO \) produced would be: \[ \text{Volume of } CO = 0.892 \, \text{mol} \times 22.4 \, \text{dm}^3/\text{mol} \approx 20 \, \text{dm}^3 \] So, approximately \( 20 \mathrm{dm}^{3} \) of carbon (II) oxide is produced.