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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 35
4장, 문제 35

For each of the acid–base reactions, calculate the mass (in grams) of each acid necessary to completely react with and neutralize 4.85 g of the base. b. 2 HNO3(aq) + Ca(OH)2(aq) → 2 H2O(l) + Ca(NO3)2(aq)

검증된 단계별 안내
1
Identify the balanced chemical equation: 2 \(\text{HNO}\)_3(aq) + \(\text{Ca(OH)}\)_2(aq) \(\rightarrow\) 2 \(\text{H}\)_2\(\text{O}\)(l) + \(\text{Ca(NO}\)_3\(\text{)}\)_2(aq)
Calculate the molar mass of the base, \(\text{Ca(OH)}\)_2, using the periodic table: \(\text{Ca}\) = 40.08 \, \(\text{g/mol}\), \(\text{O}\) = 16.00 \, \(\text{g/mol}\), \(\text{H}\) = 1.01 \, \(\text{g/mol}\)
Determine the number of moles of \(\text{Ca(OH)}\)_2 in 4.85 \, \(\text{g}\) by dividing the mass by the molar mass of \(\text{Ca(OH)}\)_2.
Use the stoichiometry of the balanced equation to find the moles of \(\text{HNO}\)_3 needed. According to the equation, 2 moles of \(\text{HNO}\)_3 react with 1 mole of \(\text{Ca(OH)}\)_2.
Calculate the mass of \(\text{HNO}\)_3 required by multiplying the moles of \(\text{HNO}\)_3 by its molar mass (\(\text{H}\) = 1.01 \, \(\text{g/mol}\), \(\text{N}\) = 14.01 \, \(\text{g/mol}\), \(\text{O}\) = 16.00 \, \(\text{g/mol}\)).

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

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 the amount of substances needed or produced. In this case, stoichiometry will help calculate the mass of nitric acid required to neutralize a given mass of calcium hydroxide.
추천 영상:
가이드 코스
01:16
Stoichiometry Concept

Acid-Base Neutralization

Acid-base neutralization is a chemical reaction where an acid reacts with a base to produce water and a salt. This process typically involves the transfer of protons (H+) from the acid to the base. Understanding the nature of the reactants, such as HNO3 being a strong acid and Ca(OH)2 being a strong base, is essential for predicting the products and calculating the amounts needed for complete reaction.
추천 영상:
가이드 코스
05:04
Lewis Acids and Bases

Molar Mass

Molar mass is the mass of one mole of a substance, expressed in grams per mole (g/mol). It is crucial for converting between grams and moles in stoichiometric calculations. To find the mass of nitric acid needed, one must first determine its molar mass and then use it in conjunction with the stoichiometric ratios from the balanced equation to find the required mass to neutralize the specified amount of base.
추천 영상:
가이드 코스
02:11
Molar Mass Concept
관련 실천
교과서 질문

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 15.2 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?

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교과서 질문

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

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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교과서 질문

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

d. 12.6 mol Na, 6.9 mol Br2

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교과서 질문

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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