1. Balanced Chemical Equation:
We need the balanced chemical equation to know the stoichiometric ratio of reactants. Unfortunately, you haven't provided the complete chemical equation for the reaction between NaClO3 and Cr2O3.
2. Molar Masses:
* NaClO3: 106.44 g/mol
* Cr2O3: 151.99 g/mol
3. Calculation:
Let's assume a hypothetical balanced equation for illustration (this might not be the actual balanced equation):
2 NaClO3 + Cr2O3 → Products
To determine the limiting reactant, we'll calculate the moles of each reactant:
* Moles of NaClO3: (15.0 g) / (106.44 g/mol) = 0.141 mol
* Moles of Cr2O3: (20.0 g) / (151.99 g/mol) = 0.132 mol
Now, we'll compare the mole ratios of the reactants based on the balanced equation. The equation suggests a 2:1 mole ratio of NaClO3 to Cr2O3.
* From the moles calculated: We have 0.141 mol of NaClO3 and 0.132 mol of Cr2O3.
* From the balanced equation: For every 2 moles of NaClO3, we need 1 mole of Cr2O3.
Since we have a slightly higher mole ratio of NaClO3 than what the equation requires, Cr2O3 is the limiting reactant. This is because we don't have enough Cr2O3 to react with all of the NaClO3.
Important Note: This explanation is based on a hypothetical balanced equation. To determine the actual limiting reactant, you need the correct balanced chemical equation for the reaction between NaClO3 and Cr2O3.
