Domanda del libro di testo
How many moles of NiCl2 can be formed in the reaction of 6.00 mol of Ni and 12.0 mol of HCl?
Ni(s) + HCl(aq) → NiCl2(aq) + H2(g)
2015
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Ch.6 Chemical Reactions: Mole and Mass Relationships
McMurry8th EditionFundamentals of General, Organic, and Biological ChemistryISBN: 9780134015187
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TOC.tableOfContents
- Ch.1 Matter and Measurements27
- Ch.2 Atoms and the Periodic Table20
- Ch.3 Ionic Compounds8
- Ch.4 Molecular Compounds23
- Ch.5 Classification & Balancing of Chemical Reactions12
- Ch.6 Chemical Reactions: Mole and Mass Relationships28
- Ch.7 Chemical Reactions: Energy, Rate and Equilibrium64
- Ch.8 Gases, Liquids and Solids24
- Ch.9 Solutions52
- Ch.10 Acids and Bases25
- Ch.11 Nuclear Chemistry22
- Ch.12 Introduction to Organic Chemistry: Alkanes57
- Ch.13 Alkenes, Alkynes, and Aromatic Compounds47
- Ch.14 Some Compounds with Oxygen, Sulfur, or a Halogen50
- Ch.15 Aldehydes and Ketones45
- Ch.16 Amines42
- Ch.17 Carboxylic Acids and Their Derivatives57
- Ch.18 Amino Acids and Proteins82
- Ch.19 Enzymes and Vitamins63
- Ch.20 Carbohydrates44
- Ch.21 The Generation of Biochemical Energy65
- Ch.22 Carbohydrate Metabolism45
- Ch.23 Lipids42
- Ch.24 Lipid Metabolism33
- Ch.25 Protein and Amino Acid Metabolism24
- Ch.26 Nucleic Acids and Protein Synthesis45
McMurry8th EditionFundamentals of General, Organic, and Biological ChemistryISBN: 9780134015187Non è quello che usi tu?Cambia libro di testo
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McMurry 8th EditionCh.6 Chemical Reactions: Mole and Mass RelationshipsProblema 17
McMurry 8th EditionCh.6 Chemical Reactions: Mole and Mass RelationshipsProblema 17Capitolo 6, Problema 17
Consider the balanced chemical equation: 2A + B2 → 2AB. Given the following reaction vessel, determine the theoretical yield of product.
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Guida verificata passo dopo passo1
Step 1: Analyze the balanced chemical equation provided: 2A + B₂ → 2AB. This indicates that two molecules of A react with one molecule of B₂ to produce two molecules of AB.
Step 2: Count the number of reactant molecules in the reaction vessel. From the image, identify the red spheres as A (Y) and the blue pairs as B₂ (X₂). Count the total number of A molecules and B₂ molecules.
Step 3: Determine the limiting reactant. Use the stoichiometric ratio from the balanced equation (2A:1B₂). Compare the available quantities of A and B₂ to find which reactant will be completely consumed first.
Step 4: Calculate the theoretical yield of AB. Based on the limiting reactant, use the stoichiometric ratio to determine how many AB molecules can be formed. For every 2A and 1B₂, 2AB molecules are produced.
Step 5: Verify the calculation by ensuring that the number of AB molecules formed does not exceed the amount dictated by the limiting reactant. Confirm that any excess reactant remains unreacted.
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Stoichiometry
Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced equation. It allows chemists to determine the proportions of substances involved in a reaction, which is essential for predicting the theoretical yield of products. In the given equation, the coefficients indicate the molar ratios of reactants A and B2 to product AB.
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01:16
Stoichiometry
Limiting Reagent
The limiting reagent is the reactant that is completely consumed first in a chemical reaction, thus determining the maximum amount of product that can be formed. Identifying the limiting reagent is crucial for calculating the theoretical yield, as it dictates how much product can be produced based on the available quantities of reactants A and B2 in the reaction vessel.
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01:30Limiting Reagent
Theoretical Yield
Theoretical yield is the maximum amount of product that can be generated from a given amount of reactants, assuming complete conversion and no losses. It is calculated using stoichiometric relationships from the balanced equation and the amounts of the limiting reagent. Understanding theoretical yield is important for evaluating the efficiency of a reaction and for practical applications in laboratory and industrial settings.
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03:09Percent Yield
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a. <IMAGE>
b. <IMAGE>
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<IMAGE>
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