Final answer:
To find out how many grams of Cr2O3 are produced from 24.8 g of Cr, we calculate the moles of Cr, use the stoichiometric ratio to convert to moles of Cr2O3, and then convert back to grams, yielding approximately 36.26 grams of Cr2O3.
Step-by-step explanation:
The student asked how many grams of Cr2O3 are produced when 24.8 g of Cr reacts according to the equation 4Cr + 3O2 -> 2Cr2O3. To solve this, we use stoichiometry based on the balanced chemical equation. First, we calculate the molar mass of the reactants and products:
- Molar mass of Cr = 51.9961 g/mol
- Molar mass of Cr2O3 = 151.9904 g/mol
Next, we convert grams of Cr to moles, use the molar ratio from the balanced equation, and then convert moles of Cr2O3 back to grams:
Moles of Cr = 24.8 g / 51.9961 g/mol
= 0.477 moles of Cr
Molar ratio from equation: 4 mol Cr :
2 mol Cr2O3, so moles of Cr2O3 = (0.477 moles Cr) / (4 moles Cr) x (2 moles Cr2O3)
= 0.2385 moles of Cr2O3
Grams of Cr2O3 = 0.2385 moles x 151.9904 g/mol
= 36.26 g of Cr2O3
Therefore, 24.8 g of Cr will produce approximately 36.26 g of Cr2O3.