QuestionFor the reaction of 0.213 moles of CO and 0.510 moles of H₂O, find the limiting reagent and max moles of CO₂ produced.
Studdy Solution
STEP 1
Assumptions1. The reaction is balanced and proceeds as given.
. The number of moles of carbon monoxide (CO) is0.213.
3. The number of moles of water (H) is0.510.
4. The reaction goes to completion.
STEP 2
The balanced chemical equation for the reaction isThis tells us that one mole of carbon monoxide reacts with one mole of water to produce one mole of carbon dioxide and one mole of hydrogen.
STEP 3
To find the limiting reagent, we need to compare the ratio of the number of moles of each reactant to the stoichiometric coefficients in the balanced chemical equation.
For carbon monoxide, the ratio isFor water, the ratio is
STEP 4
The reactant with the smallest ratio is the limiting reagent. In this case, carbon monoxide (CO) is the limiting reagent because its ratio (0.213) is smaller than that of water (0.510).
Limiting reagent Carbon monoxide (CO)
STEP 5
The maximum amount of carbon dioxide (CO2) that can be produced is determined by the stoichiometry of the reaction and the amount of the limiting reagent.
From the balanced chemical equation, we see that one mole of carbon monoxide produces one mole of carbon dioxide. Therefore, the maximum amount of carbon dioxide that can be produced is equal to the number of moles of the limiting reagent.
The maximum amount of carbon dioxide that can be produced is0.213 moles.
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