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Ch.3 - Chemical Reactions and Reaction Stoichiometry
All textbooksBrown 14th EditionCh.3 - Chemical Reactions and Reaction StoichiometryProblem 77a
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Chapter 3, Problem 77a

Sodium hydroxide reacts with carbon dioxide as follows: 2 NaOH(s) + CO2(g) → Na2CO3(s) + H2O(l) Which is the limiting reactant when 1.85 mol NaOH and 1.00 mol CO2 are allowed to react?

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Identify the balanced chemical equation: 2 NaOH(s) + CO2(g) → Na2CO3(s) + H2O(l). This equation shows that 2 moles of NaOH react with 1 mole of CO2.
Determine the mole ratio from the balanced equation: For every 2 moles of NaOH, 1 mole of CO2 is required.
Calculate the moles of NaOH needed to completely react with the given moles of CO2: Since you have 1.00 mol of CO2, you need 2.00 moles of NaOH (using the 2:1 ratio).
Compare the available moles of NaOH to the moles required: You have 1.85 mol of NaOH available, but you need 2.00 mol to react with all of the CO2.
Conclude which reactant is limiting: Since you do not have enough NaOH to react with all the CO2, NaOH is the limiting reactant.

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