Textbook Question
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?
3. Chemical Reactions
Limiting Reagent
Multiple Choice
Suppose 0.0350 g of Mg is reacted with 10.00 mL of 6 M HCl to produce aqueous magnesium chloride and hydrogen gas according to the reaction: Mg(s) + 2HCl(aq) → MgCl₂(aq) + H₂(g). What is the limiting reactant in this reaction?
A
Magnesium chloride (MgCl₂)
B
Hydrogen gas (H₂)
C
Hydrochloric acid (HCl)
D
Magnesium (Mg)
Verified step by step guidance1
Step 1: Begin by writing the balanced chemical equation for the reaction: .
Step 2: Calculate the moles of magnesium (Mg) using its molar mass. The molar mass of Mg is approximately 24.31 g/mol. Use the formula: .
Step 3: Calculate the moles of hydrochloric acid (HCl) using its concentration and volume. Use the formula: . Remember to convert the volume from mL to L by dividing by 1000.
Step 4: Compare the mole ratio of the reactants to the coefficients in the balanced equation. The balanced equation shows that 1 mole of Mg reacts with 2 moles of HCl. Determine which reactant is present in a smaller stoichiometric amount.
Step 5: Identify the limiting reactant as the one that will be completely consumed first based on the stoichiometric calculations. The reactant with fewer moles than required by the balanced equation is the limiting reactant.
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