Domanda del libro di testo
An alternative method for producing hydriodic acid is the reaction of iodine with hydrogen sulfide: H2S + I2 → 2 HI + S (a) How many grams of I2 are needed to react with 49.2 g of H2S?
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Ch.3 - Mass Relationships in Chemical Reactions
McMurry8th EditionChemistryISBN: 9781292336145
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TOC.tableOfContents
- Ch.1 - Chemical Tools: Experimentation & Measurement170
- Ch.2 - Atoms, Molecules & Ions160
- Ch.3 - Mass Relationships in Chemical Reactions169
- Ch.4 - Reactions in Aqueous Solution199
- Ch.5 - Periodicity & Electronic Structure of Atoms102
- Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory92
- Ch.7 - Covalent Bonding and Electron-Dot Structures61
- Ch.8 - Covalent Compounds: Bonding Theories and Molecular Structure59
- Ch.9 - Thermochemistry: Chemical Energy122
- Ch.10 - Gases: Their Properties & Behavior155
- Ch.11 - Liquids & Phase Changes54
- Ch.12 - Solids and Solid-State Materials73
- Ch.13 - Solutions & Their Properties120
- Ch.14 - Chemical Kinetics98
- Ch.15 - Chemical Equilibrium125
- Ch.16 - Aqueous Equilibria: Acids & Bases110
- Ch.17 - Applications of Aqueous Equilibria147
- Ch.18 - Thermodynamics: Entropy, Free Energy & Equilibrium86
- Ch.19 - Electrochemistry154
- Ch.20 - Nuclear Chemistry96
- Ch.21 - Transition Elements and Coordination Chemistry156
- Ch.22 - The Main Group Elements187
- Ch.23 - Organic and Biological Chemistry51
Capitolo 3, Problema 68
Silver metal reacts with chlorine (Cl2) to yield silver chlo-ride. If 2.00 g of Ag reacts with 0.657 g of Cl2, what is the empirical formula of silver chloride?
Guida verificata passo dopo passo1
Step 1: The first step in determining the empirical formula is to convert the masses of the reactants to moles. The molar mass of silver (Ag) is approximately 107.87 g/mol and the molar mass of chlorine (Cl2) is approximately 70.90 g/mol. So, divide the given mass of each element by its molar mass to find the number of moles.
Step 2: Once you have the number of moles of each element, you can find the ratio of the number of moles of each element to each other. This is done by dividing each number of moles by the smallest number of moles calculated in step 1.
Step 3: If the ratio obtained in step 2 is not a whole number, it may be necessary to multiply it by an integer (for example, 2, 3, 4, etc.) to obtain whole numbers. This is because the empirical formula must be expressed in terms of whole numbers.
Step 4: The empirical formula is then written by assigning these whole numbers as subscripts to the corresponding elements in the formula.
Step 5: Check your empirical formula to make sure it makes sense. The empirical formula represents the simplest whole-number ratio of atoms in a compound. In this case, the empirical formula should represent the simplest whole-number ratio of silver (Ag) to chlorine (Cl) atoms in silver chloride.
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Stoichiometry
Stoichiometry is the branch of chemistry that deals with the quantitative relationships between the reactants and products in a chemical reaction. It allows chemists to calculate the amounts of substances consumed and produced in a reaction based on balanced chemical equations. Understanding stoichiometry is essential for determining the empirical formula, as it helps in converting masses of reactants to moles and establishing the mole ratio.
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Percorso guidato
01:16
Stoichiometry Concept
Empirical Formula
The empirical formula of a compound represents the simplest whole-number ratio of the elements present in that compound. It is derived from the mole ratio of the elements after determining the number of moles of each element involved in the reaction. For silver chloride, calculating the empirical formula involves finding the ratio of silver to chlorine based on the moles obtained from the given masses.
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Percorso guidato
02:26Empirical vs Molecular Formula
Molar Mass
Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is crucial for converting between grams and moles, which is necessary for stoichiometric calculations. For this question, knowing the molar masses of silver (Ag) and chlorine (Cl2) allows for the conversion of the given masses into moles, facilitating the determination of the empirical formula of silver chloride.
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Percorso guidato
02:11Molar Mass Concept
Pratica correlata
Domanda del libro di testo
Pure oxygen was first made by heating mercury(II) oxide:
HgO --> (heat) Hg + O2 Unbalanced
(a) Balance the equation.
(b) How many grams of mercury and how many grams of oxygen are formed from 45.5 g of HgO?
(c) How many grams of HgO would you need to obtain 33.3 g of O2
783
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Domanda del libro di testo
The industrial production of hydriodic acid takes place by treatment of iodine with hydrazine (N2H4):
2 I2 + N2H4 --> 4 HI + N2
(b) How many grams of HI are produced from the reaction of 115.7 g of N2H4 with excess iodine
722
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Domanda del libro di testo
Ethylene gas, C2H4, reacts with water at high temperature to yield ethyl alcohol, C2H6O.
(a) How many grams of ethylene are needed to react with 0.133 mol of H2O? How many grams of ethyl alcohol will result?
(b) How many grams of water are needed to react with 0.371 mol of ethylene? How many grams of ethyl alcohol will result?
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Domanda del libro di testo
Titanium dioxide (TiO2), the substance used as the pigment in white paint, is prepared industrially by reaction of TiCl4 with O2 at high temperature.
TiCl4 + O2 --> (heat) TiO2 + 2 Cl2
How many kilograms of TiO2 can be prepared from 5.60 kg of TiCl4?
1768
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