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Ch.4 - Chemical Reactions and Chemical Quantities
All textbooksTro 6th EditionCh.4 - Chemical Reactions and Chemical QuantitiesProblem 43c
Chapter 4, Problem 43c

Find the limiting reactant for each initial amount of reactants. 2 Na(s) + Br2( g) → 2 NaBr(s) c. 1.5 mol Na, 2.1 mol Br2

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Identify the balanced chemical equation: 2 \text{Na}(s) + \text{Br}_2(g) \rightarrow 2 \text{NaBr}(s).
Determine the mole ratio from the balanced equation: 2 moles of Na react with 1 mole of Br_2.
Calculate the moles of Na required to react with the given moles of Br_2: \text{Moles of Na required} = 2 \times \text{moles of Br}_2.
Compare the moles of Na required with the moles of Na available: If \text{moles of Na available} < \text{moles of Na required}, then Na is the limiting reactant.
If \text{moles of Na available} > \text{moles of Na required}, then Br_2 is the limiting reactant.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Limiting Reactant

The limiting reactant is the substance that is completely consumed first in a chemical reaction, thus determining the maximum amount of product that can be formed. It is essential to identify this reactant to predict the yield of the reaction accurately.
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Stoichiometry

Stoichiometry involves the calculation of reactants and products in chemical reactions based on balanced chemical equations. It allows chemists to determine the proportions of each substance involved, which is crucial for identifying the limiting reactant.
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Mole Ratio

The mole ratio is derived from the coefficients of a balanced chemical equation and indicates the relative amounts of reactants and products involved in the reaction. Understanding the mole ratio is vital for comparing the available amounts of reactants to determine which one limits the reaction.
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Related Practice
Textbook Question

Hydrobromic acid dissolves solid iron according to the reaction:

Fe(s) + 2 HBr(aq) → FeBr2(aq) + H2(g)

What mass of HBr (in g) do you need to dissolve a 2.80-g pure iron bar on a padlock? What mass of H2 would the complete reaction of the iron bar produce?

Textbook Question

Sulfuric acid dissolves aluminum metal according to the reaction:

2 Al(s) + 3 H2SO4(aq) → Al2(SO4)3(aq) + 3 H2(g)

Suppose you want to dissolve an aluminum block with a mass of 11.3 g. What minimum mass of H2SO4 (in g) do you need? What mass of H2 gas (in g) does the complete reaction of the aluminum block produce?

Textbook Question

For each of the reactions, calculate the mass (in grams) of the product that forms when 15.39 g of the underlined reactant completely reacts. Assume that there is more than enough of the other reactant.

a. 2 K(s) + Cl2(g) → 2 KCl(s)

b. 2 K(s) + Br2(l) → 2 KBr(s)

c. 4 Cr(s) + 3 O2(g) → 2 Cr2O3(s)

d. 2 Sr(s) + O2(g) → 2 SrO(s)

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Textbook Question

Find the limiting reactant for each initial amount of reactants. 4 Al(s) + 3 O2( g) → 2 Al2O3(s)

a. 4 mol Al, 2 mol O2

b. 5 mol Al, 3 mol O2

c. 17 mol Al, 11 mol O2

d. 8.8 mol Al, 7.2 mol O2

Textbook Question

Consider the reaction: 4 HCl(g) + O2(g) → 2 H2O(g) + 2 Cl2(g) Each molecular diagram represents an initial mixture of reactants. How many molecules of Cl2 form from the reaction mixture that produces the greatest amount of products?

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Textbook Question

Consider the reaction: 2 CH3OH(g) + 3 O2(g) → 2 CO2(g) + 4 H2O(g) Each of the molecular diagrams represents an initial mixture of the reactants. How many CO2 molecules form from the reaction mixture that produces the greatest amount of products?

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