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.
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Calculate the moles of O₂: The molar mass of oxygen (O₂) is approximately 32.00 g/mol.
\[ \text{Moles of O}_2 = \frac{\text{mass of O}_2}{\text{molar mass of O}_2} = \frac{4.80 , \text{g}}{32.00 , \text{g/mol}} = 0.150 , \text{mol} \]
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Use the stoichiometry of the reaction: The balanced equation is: \[ 2 , \text{CO} + \text{O}_2 \rightarrow 2 , \text{CO}_2 \]
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.
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