The balanced chemical equation for the reaction between antimony trioxide (Sb2O3) and carbon monoxide (CO) is:
Sb2O3 + 3CO → 2Sb + 3CO2
From the equation, we can see that 1 mole of Sb2O3 reacts with 3 moles of CO to produce 3 moles of CO2. The molar mass of Sb2O3 is 291.52 g/mol, so 0.465 g of Sb2O3 is equal to 0.465 g / 291.52 g/mol = 0.001592 mol.
Since 1 mole of Sb2O3 reacts with 3 moles of CO, we need 3 * 0.001592 = 0.004776 mol of CO to react completely with 0.465 g of Sb2O3.
The molar mass of CO is 28.01 g/mol, so 0.004776 mol of CO is equal to 0.004776 mol * 28.01 g/mol = 0.1338 g of CO.
Therefore, 0.465 g of Sb2O3 will produce 0.1338 g of CO. To convert this to liters of CO at a given temperature and pressure, we would need to know the volume of 0.1338 g of CO under those conditions using the ideal gas law.
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