Multiple Choice
In a stoichiometry lab, you react 2.00 mol of HCl with 1.00 mol of CaCO3. According to the balanced equation CaCO3 + 2 HCl → CaCl2 + CO2 + H2O, what is the limiting reactant?
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3. Chemical Reactions
Stoichiometry
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Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
In stoichiometry, how do you determine the mole ratio between and in the balanced equation ?
A
Use the coefficients in the balanced equation; the mole ratio is .
B
Use molar masses; the mole ratio is .
C
Use the product coefficients; the mole ratio is .
D
Use the subscripts in the formulas; the mole ratio is .
Verified step by step guidance1
Identify the balanced chemical equation: \(\mathrm{N}_2 + 3\mathrm{H}_2 \rightarrow 2\mathrm{NH}_3\).
Understand that the mole ratio between reactants is given by the coefficients in the balanced equation, which represent moles of each substance involved.
Locate the coefficients for \(\mathrm{N}_2\) and \(\mathrm{H}_2\) in the balanced equation: 1 for \(\mathrm{N}_2\) and 3 for \(\mathrm{H}_2\).
Write the mole ratio as \(\frac{1\ \mathrm{mol}\ \mathrm{N}_2}{3\ \mathrm{mol}\ \mathrm{H}_2}\), which means 1 mole of nitrogen reacts with 3 moles of hydrogen.
Note that subscripts in chemical formulas indicate the number of atoms in a molecule, not the mole ratio, and molar masses are used for mass-to-mole conversions, not mole ratios directly.
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