CaO + C --> CaC2 + CO2 [unbalanced]
If 244 g of CaO is combined with 318 g C, how many grams of CO2 could be produced if the reaction goes to completion?
To find the number of grams of CO2 that could be produced, we need to balance the chemical equation first. The balanced equation for the given reaction is:
CaO + 3C -> CaC2 + CO2
Now, let's calculate the molar masses of all the substances involved.
Molar mass of CaO (Calcium oxide) = 40.08 g/mol
Molar mass of C (Carbon) = 12.01 g/mol
Molar mass of CaC2 (Calcium carbide) = 64.10 g/mol
Molar mass of CO2 (Carbon dioxide) = 44.01 g/mol
Next, we need to convert the given masses of CaO and C to moles.
Number of moles of CaO = mass / molar mass = 244 g / 40.08 g/mol
Number of moles of C = mass / molar mass = 318 g / 12.01 g/mol
Now, we can use the balanced equation to determine the ratio of moles converted.
From the balanced equation, we see that 1 mole of CaO reacts with 3 moles of C to produce 1 mole of CO2.
Therefore, the limiting reactant is the one that produces fewer moles of product. To determine which reactant is limiting, we need to compare the moles of CaO and C.
Assuming CaO is the limiting reactant, the number of moles of CO2 produced is 1 mole.
Assuming C is the limiting reactant, the number of moles of CO2 produced is (1 mole of CO2 / 3 moles of C) * (number of moles of C)
Now we compare the two results to determine the correct answer.
To find the number of grams of CO2, we multiply the number of moles of CO2 by its molar mass:
Number of grams of CO2 = number of moles of CO2 * molar mass of CO2
Using this information, you can calculate the final answer.