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
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McMurry 8th EditionCh.3 - Mass Relationships in Chemical ReactionsProblema 72b
McMurry 8th EditionCh.3 - Mass Relationships in Chemical ReactionsProblema 72bCapitolo 3, Problema 72b
Nickel(II) sulfate, used for nickel plating, is prepared by treat-ment of nickel(II) carbonate with sulfuric acid: NiCO3 + H2SO4 → NiSO4 + CO2 + H2O
(b) How many grams of NiSO4 are obtained if the yield is 78.9%?
Guida verificata passo dopo passo1
Identify the balanced chemical equation: \( \text{NiCO}_3 + \text{H}_2\text{SO}_4 \rightarrow \text{NiSO}_4 + \text{CO}_2 + \text{H}_2\text{O} \).
Determine the molar mass of each compound involved: \( \text{NiCO}_3 \), \( \text{H}_2\text{SO}_4 \), and \( \text{NiSO}_4 \).
Calculate the theoretical yield of \( \text{NiSO}_4 \) using stoichiometry based on the initial amount of \( \text{NiCO}_3 \) or \( \text{H}_2\text{SO}_4 \) provided.
Apply the percentage yield formula: \( \text{Actual Yield} = \text{Theoretical Yield} \times \frac{\text{Percentage Yield}}{100} \).
Convert the actual yield from moles to grams using the molar mass of \( \text{NiSO}_4 \).
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Stoichiometry
Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows chemists to determine the amount of product formed from a given amount of reactant. In this case, understanding the stoichiometric ratios from the reaction between nickel(II) carbonate and sulfuric acid is essential to calculate the theoretical yield of nickel(II) sulfate.
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Percorso guidato
01:16
Stoichiometry Concept
Percent Yield
Percent yield is a measure of the efficiency of a chemical reaction, calculated by comparing the actual yield of a product to the theoretical yield. It is expressed as a percentage and is crucial for evaluating how much of the expected product was actually produced. In this question, the yield of 78.9% indicates that only a portion of the theoretical amount of NiSO4 was obtained.
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Percorso guidato
03:09Percent Yield in Reactions
Molar Mass
Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is essential for converting between the number of moles of a substance and its mass. To find the mass of NiSO4 produced, one must first calculate its molar mass and then apply it to the stoichiometric calculations involving the yield.
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Percorso guidato
02:11Molar Mass Concept
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Nickel(II) sulfate, used for nickel plating, is prepared by treat-ment of nickel(II) carbonate with sulfuric acid: NiCO3 + H2SO4 → NiSO4 + CO2 + H2O (a) How many grams of H2SO4 are needed to react with 14.5 g of NiCO3?
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Assume that you have 1.39 mol of H2 and 3.44 mol of N2. How many grams of ammonia (NH3) can you make, and how many grams of which reactant will be left over?
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An alternative method for producing hydriodic acid is the reaction of iodine with hydrogen sulfide:H2S + I2 → 2 HI + S (b) How many grams of HI are produced from the reaction of 95.4 g of H2S with excess I2?
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Hydrazine, N2H4, once used as a rocket propellant, reacts with oxygen: N2H4 + O2 → N2 + 2 H2O (a) How many grams of O2 are needed to react with 50.0 g of N2H4?
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Hydrazine, N2H4, once used as a rocket propellant, reacts with oxygen: N2H4 + O2 → N2 + 2 H2O (b) How many grams of N2 are obtained if the yield is 85.5%?
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