How many moles of carbon monoxide are needed to react with 4.80 g of oxygen gas to produce carbon dioxide? 2CO + O2 --> 2CO2.

Answer 1

To determine the number of moles of carbon monoxide (CO) needed to react with 4.80 g of oxygen gas (O₂) to produce carbon dioxide (CO₂), we first need to find the moles of O₂.

1. Calculate the moles of O₂: The molar mass of oxygen (O₂) is approximately 32.00 g/mol.

   $${\text{Moles of O}}_2=\frac{{\text{mass of O}}_2}{{\text{molar mass of O}}_2}=\frac{4.80,\text{g}}{32.00,\text{g/mol}}=0.150,\text{mol}$$

2. Use the stoichiometry of the reaction: The balanced equation is: $$2,\text{CO}+{\text{O}}_2\to 2,{\text{CO}}_2$$

   From the equation, we see that 1 mole of O₂ reacts with 2 moles of CO. Therefore, to find the moles of CO needed, we use the following ratio: $$\text{Moles of CO}=2\times {\text{Moles of O}}_2$$

   Substituting the number of moles of O₂ we calculated: $$\text{Moles of CO}=2\times 0.150,\text{mol}=0.300,\text{mol}$$

Therefore, 0.300 moles of carbon monoxide are needed to react with 4.80 g of oxygen gas to produce carbon dioxide.