The left side of a balanced chemical equation is shown below:
K2Cr2O7 + 4H2SO4 + 3SeO2
If 0.600 moles of K2Cr2O7, 2.800 moles of H2SO4 and 1.500 moles of SeO2 are brought together and allowed to react, then
To determine the limiting reactant and the amount of product formed, we need to compare the mole ratios of the reactants in the balanced chemical equation to the given amounts. The balanced equation is:
K2Cr2O7 + 4H2SO4 + 3SeO2 → Cr2(SO4)3 + K2SO4 + 3H2O + SeO2
The mole ratios of the reactants in the balanced equation are 1:4:3 for K2Cr2O7, H2SO4, and SeO2, respectively.
Given:
- K2Cr2O7: 0.600 moles
- H2SO4: 2.800 moles
- SeO2: 1.500 moles
Let's calculate the moles of each reactant that would be required based on the mole ratios:
Moles of K2Cr2O7 required = 0.600 moles
Moles of H2SO4 required = 4 * 0.600 moles = 2.400 moles
Moles of SeO2 required = 3 * 0.600 moles = 1.800 moles
Comparing the required moles to the actual moles given:
K2Cr2O7 is in excess (0.600 moles given, 0.600 moles required)
H2SO4 is in excess (2.800 moles given, 2.400 moles required)
SeO2 is the limiting reactant (1.500 moles given, 1.800 moles required)
Therefore, SeO2 is the limiting reactant, and the amount of product formed will be determined by its mole ratio to the other reactants. The balanced equation shows that 3 moles of SeO2 react to form 1 mole of the product Cr2(SO4)3.
Thus, based on the given amounts of reactants, the amount of product formed will depend on the stoichiometry of the reaction and the limiting reactant.
To find out what happens when 0.600 moles of K2Cr2O7, 2.800 moles of H2SO4, and 1.500 moles of SeO2 react, we need to determine the limiting reactant.
First, we need to calculate the moles of each reactant required to fully react with K2Cr2O7. From the balanced equation coefficient, we can see that the molar ratio between K2Cr2O7 and H2SO4 is 1:4 and the molar ratio between K2Cr2O7 and SeO2 is 1:3.
Moles of H2SO4 required = 4 * (0.600 moles of K2Cr2O7) = 2.400 moles
Moles of SeO2 required = 3 * (0.600 moles of K2Cr2O7) = 1.800 moles
Now, let's compare the moles of reactants we have with the calculated moles required:
For K2Cr2O7, we have 0.600 moles, which is less than the calculated moles required (2.400 moles of H2SO4 and 1.800 moles of SeO2).
For H2SO4, we have 2.800 moles, which is more than the calculated moles required (2.400 moles).
For SeO2, we have 1.500 moles, which is more than the calculated moles required (1.800 moles).
Since K2Cr2O7 is the limiting reactant (the reactant that is completely consumed first and determines the maximum amount of product that can be formed), the reaction will stop when all 0.600 moles of K2Cr2O7 have reacted.
To calculate the amount of product formed, we must refer back to the balanced equation and assess the stoichiometric coefficient ratio.
From the balanced equation, the molar ratio between K2Cr2O7 and the product is:
2 mol K2Cr2O7 : 6 mol product
Therefore, the moles of product formed from the reaction of 0.600 moles of K2Cr2O7 will be:
6 * (0.600 moles of K2Cr2O7) = 3.600 moles of product
Therefore, 3.600 moles of product will be formed when 0.600 moles of K2Cr2O7, 2.800 moles of H2SO4, and 1.500 moles of SeO2 react.