Domanda del libro di testo
Balance the following equation, and tell how many moles of nickel will react with 9.81 mol of hydrochloric acid.
Ni(s) + HCl(aq) → NiCl2(aq) + H2(g)
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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 8b
McMurry 8th EditionCh.6 Chemical Reactions: Mole and Mass RelationshipsProblema 8bCapitolo 6, Problema 8b
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)
Guida verificata passo dopo passo1
Write the balanced chemical equation for the reaction: Ni + 2HCl → NiCl₂ + H₂. This equation shows that 1 mole of Ni reacts with 2 moles of HCl to produce 1 mole of NiCl₂ and 1 mole of H₂.
Determine the limiting reactant by comparing the mole ratio of the reactants to the stoichiometric ratio in the balanced equation. From the equation, 1 mole of Ni requires 2 moles of HCl.
Calculate the amount of HCl required to react with 6.00 moles of Ni. Using the stoichiometric ratio, multiply the moles of Ni by the ratio of HCl to Ni: (6.00 mol Ni) × (2 mol HCl / 1 mol Ni).
Compare the calculated amount of HCl required to the amount of HCl available (12.0 mol). If the available HCl is greater than or equal to the required amount, Ni is the limiting reactant. Otherwise, HCl is the limiting reactant.
Using the limiting reactant, calculate the moles of NiCl₂ formed. If Ni is the limiting reactant, the moles of NiCl₂ formed will be equal to the moles of Ni (1:1 ratio from the balanced equation). If HCl is the limiting reactant, divide the moles of HCl by 2 (stoichiometric ratio) to find the moles of NiCl₂ formed.
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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 us to calculate how much of each substance is needed or produced based on balanced chemical equations. Understanding stoichiometry is essential for determining the amounts of reactants and products involved in a reaction.
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01:16
Stoichiometry
Balanced Chemical Equation
A balanced chemical equation represents a chemical reaction with equal numbers of each type of atom on both sides of the equation. It provides the mole ratios of reactants and products, which are crucial for stoichiometric calculations. For the reaction involving Ni and HCl to form NiCl2, the balanced equation will indicate how many moles of NiCl2 can be produced from the given amounts of Ni and HCl.
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01:32Balancing Chemical Equations (Simplified) Concept 1
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. Identifying the limiting reactant is critical in stoichiometric calculations, as it dictates the extent of the reaction. In this case, knowing which reactant (Ni or HCl) limits the formation of NiCl2 will help calculate the moles of product formed.
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Percorso guidato
01:30Limiting Reagent
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