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Ch.4 - Chemical Quantities & Aqueous Reactions
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Tro 4th EditionCh.4 - Chemical Quantities & Aqueous Reactions문제 36
4장, 문제 36

For each precipitation reaction, calculate how many grams of the first reactant are necessary to completely react with 55.8 g of the second reactant. a. 2 KI(aq) + Pb(NO3)2(aq) → PbI2(s) + 2 KNO3(aq) b. Na2CO3(aq) + CuCl2(aq) → CuCO3(s) + 2 NaCl(aq) c. K2SO4(aq) + Sr(NO3)2(aq) → SrSO4(s) + 2 KNO3(aq)

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1
Identify the balanced chemical equation for each reaction to determine the stoichiometry between the reactants.
Calculate the molar mass of the second reactant (55.8 g) for each reaction.
Convert the mass of the second reactant to moles using its molar mass.
Use the stoichiometry from the balanced equation to find the moles of the first reactant needed to completely react with the moles of the second reactant.
Convert the moles of the first reactant to grams using its molar mass.

주요 개념

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Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It involves using mole ratios derived from the coefficients of the balanced equation to determine how much of each substance is needed or produced. Understanding stoichiometry is essential for solving problems related to the amounts of reactants and products in a reaction.
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가이드 코스
01:16
Stoichiometry Concept

Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is calculated by summing the atomic masses of all atoms in a molecule. Knowing the molar mass of reactants allows for the conversion between grams and moles, which is crucial for stoichiometric calculations in precipitation reactions.
추천 영상:
가이드 코스
02:11
Molar Mass Concept

Precipitation Reactions

Precipitation reactions occur when two aqueous solutions react to form an insoluble solid, known as a precipitate. These reactions can be represented by balanced chemical equations, which show the reactants and products involved. Understanding the formation of precipitates helps in predicting the outcome of reactions and calculating the amounts of reactants needed for complete reactions.
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가이드 코스
01:53
Selective Precipitation
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a. 1 mol Al, 1 mol O2

b. 4 mol Al, 2.6 mol O2

c. 16 mol Al, 13 mol O2

d. 7.4 mol Al, 6.5 mol O2

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Find the limiting reactant for each initial amount of reactants.

2 Na(s) + Br2(g) → 2 NaBr(s)

a. 2 mol Na, 2 mol Br2

b. 1.8 mol Na, 1.4 Br2

c. 2.5 mol Na, 1 mol Br2

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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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