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103 solutions

Balancing Redox Reactions

Q. Balance the following redox equation, for a reaction that takes place in acidic solution. Co2^2+(aq) + Au^3+(aq) → Au(s) + Co^3+(aq) Answer the following questions to balance the equation. Which species is reduced? a) Co^2+ b) Au^3+

Solved • Nov 14, 2019

Balancing Redox Reactions

Q. Potassium permanganate, KMnO4, is a powerful oxidizing agent. The products of a given redox reaction with the permanganate ion depend on the reaction condition used. In basic solution, the following equation represents the reaction of this ion with a solution containing sodium sulfite: MnO4^-(aq) + SO3^2-(aq) → MnO2(s) +SO4^2-(aq) Since this reaction takes place in basic solution, H2O(l) and OH^-(aq) will be shown in the reaction. Places for these species are indicated by the blanks in the following restatement of the question: MnO4^-(aq) + SO3^2-(aq) + ___ → MnO2(s) + SO4^2-(aq) ___ What are the coefficients of the reactants and products in the balanced equation above? Remember to include H2O(l) and OH^-(aq) in the blanks where appropriate. Your answer should have six terms. Enter the equation coefficients in order separated by commas (e.g., 2, 2, 1, 4, 4, 3). Include coefficients of 1, as required, for grading purposes.

Solved • Oct 12, 2019

Balancing Redox Reactions

Q. In acidic solution, the nitrate ion can be used to react with a number of metal ions. One such reaction is N03^-(aq) + Sn^2+(aq) → NO2(aq) + Sb^4+(aq) Since this reaction takes place in acidic solution, H2O(l) and H+ (aq) will be involved in the reaction. Places for these species are indicated by the blanks in the following restatement of the question. NO3^-(aq) +Sn^2+(aq) + ___ → NO2(aq) + Sn^4+(aq) ___ What are the coefficients of the reactants and products in the balanced equation above? Remember to include H2O(l) and H+(aq) in the appropriate blanks. Your answer should have six terms. Enter the equation coefficients in order separated by commas (e.g., 2, 2, 1, 4, 4, 3). Include coefficients of 1, as required, for grading purposes.

Solved • Oct 12, 2019

Balancing Redox Reactions

Q. 13. The following redox reaction is not balanced. Using the half reaction method, balance the following redox reaction under basic conditions: Zn(s) + NO3^-(aq) → Zn(OH)4^2-(s) + NH3(aq)

Solved • Oct 11, 2019

Balancing Redox Reactions

Q. Consider the unbalanced redox reaction: Cr2O2−7(aq)+Cu(s)→Cr3+(aq)+Cu2+(aq) Part A: Balance the equation. Express your answer as a chemical equation. Identify all of the phases in your answer. part B Determine the volume of a 0.775 M K2Cr2O7 solution required to completely react with 3.86 g of Cu. Express your answer using three significant figures.

Solved • Nov 7, 2019

Balancing Redox Reactions

Q. Balance the following equation in basic solution using the lowest possible integers and give the coefficient of water. Cr^3+(aq) + MnO2(s) → Mn^2+(aq) + CrO4^2-(aq) a) 4 b) 1 c) 3 d) 0 e) 2

Solved • Oct 30, 2019

Balancing Redox Reactions

Q. Balance the following equation in acidic solution using the lowest possible integers and give the coefficient of water. CrO4^2-(aq) + Fe^2+(aq) → Fe^3+(aq) + Cr^3+(aq) a) 4 b) 7 c) 5 d) 1

Solved • Oct 30, 2019

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Ch.1 - Intro to General Chemistry
The Scientific Method Mixtures Scientific Notation Accuracy & Precision Standard Deviation, Mean, Median & Mode Metric Prefixes Significant Figures Energy, Heat and Temperature Physical & Chemical Changes Physical & Chemical Properties Types of Energy Dimensional Analysis Density
Ch.2 - Atoms & Elements
Periodic Table Periodic Table Charges Mole Concept Calculating Molar Mass Isotopes Subatomic Particles Atomic Theory Oil Drop Experiment
Ch.3 - Chemical Reactions
Ionic and Covalent Bonds Molecular Models Polyatomic Ions Naming Covalent Compounds Naming Ionic Compounds Naming Acids Empirical Formula Molecular Formula Combustion Analysis Mass Percent Formula Balancing Chemical Equations Functional Groups in Chemistry Stoichiometry Theoretical Yield Limiting Reagent Limiting Reactant Percent Yield
BONUS: Lab Techniques and Procedures
Distillation & Floatation Test for Ions and Gases
BONUS: Mathematical Operations and Functions
Multiplication and Division Operations
Ch.4 - Chemical Quantities & Aqueous Reactions
Molarity Normality & Equivalent Weight Solution Stoichiometry Dilution Solubility Rules Net Ionic Equations Net Ionic Equation Electrolytes Redox Reaction Balancing Redox Reactions Redox Reactions Oxidation Reduction (Redox) Reactions Calculate Oxidation Number Oxidation Number Types of Chemical Reactions Activity Series
Ch.5 - Gases
Pressure Units Manometer Partial Pressure The Ideal Gas Law Chemistry Gas Laws Ideal Gas Law Boyle's Law Ideal Gas Law Density Ideal Gas Law Molar Mass Standard Temperature and Pressure Gas Stoichiometry Collecting Gas Over Water Effusion Root Mean Square Speed Kinetic Molecular Theory Van der Waals Equation Kinetic Energy of Gases Velocity Distribution Charles Law Combined Gas Law
Ch.6 - Thermochemistry
Units of Energy Internal Energy Endothermic & Exothermic Reactions Calorimetry Thermochemical Equation Hess's Law Enthalpy of Formation Enthalpy
Ch.7 - Quantum Mechanics
Electromagnetic Spectrum Wavelength and Frequency The Particle Nature of Light Photoelectric Effect De Broglie Wavelength Heisenberg Uncertainty Principle Bohr Model Bohr and Balmer Equations Wave Function Introduction to Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Electron Configuration Orbital Diagrams Paramagnetic and Diamagnetic Coulomb's Law Effective Nuclear Charge Quantum Numbers The Spin Quantum Number Orbital Shapes Periodic Trends Atomic Radius Periodic Trends: Atomic Radius Periodic Trends: Ionic Radius Periodic Trends: Ionization Energy Ionization Energy Periodic Trends: Electron Affinity Periodic Trends: Metallic Character Periodic Trend: Noble Gases
Ch.9 - Bonding & Molecular Structure
Chemical Bonds Lattice Energy Lattice Energy Application Born Haber Cycle Dipole Moment Lewis Dot Structure Octet Rule Formal Charge Resonance Structures Bond Energy
Ch.10 - Molecular Shapes & Valence Bond Theory
Molecular vs Electron Geometry Molecular Geometry VSEPR Theory Bond Angles Electronegativity Hybridization Benzene Orbital Overlap Molecular Orbital Theory Bond Order Delocalized Electrons Homonuclear Diatomic Molecules Heteronuclear Diatomic Molecules
Ch.11 - Liquids, Solids & Intermolecular Forces
Molecular Polarity Intermolecular Forces Intermolecular Forces and Physical Properties Phase Diagram Heating and Cooling Curves Unit Cell Atomic, Ionic, and Molecular Solids Clausius-Clapeyron Equation
Ch.12 - Solutions
Solutions, Molarity and Intermolecular Forces Making Solutions Henry's Law Calculate Molarity Mass Percent Molality Mole Fraction ppm Boiling Point Elevation Freezing Point Depression The Colligative Properties
Ch.13 - Chemical Kinetics
Rate of Reaction Average Rate of Reaction Instantaneous Rate of Change Arrhenius Equation Energy Diagram Catalyst Reaction Mechanism Rate Law Integrated Rate Law Identifying Reaction Order Collision Theory
Ch.14 - Chemical Equilibrium
Chemical Equilibrium Equilibrium Expressions ICE Chart Le Chatelier's Principle The Reaction Quotient
Ch.15 - Acid and Base Equilibrium
Identifying Acids and Bases Strong Acids and Strong Bases Arrhenius Acid and Base Bronsted Lowry Acid and Base Conjugate Acids and Bases Amphoteric Lewis Acid and Base pH and pOH Strong Acid-Base Calculations Weak Acids Weak Bases Ka and Kb Ionic Salts Diprotic Acid Polyprotic Acid
Ch.16 - Aqueous Equilibrium
Buffer Henderson Hasselbalch Equation Acid and Base Titration Curves Weak Acid Strong Base Titrations Weak Base Strong Acid Titrations Equivalence Point Strong Acid Strong Base Titrations Titrations of Diprotic and Polyprotic Acids Acid Base Indicators Ksp Selective Precipitation Formation Constant
Ch. 17 - Chemical Thermodynamics
Spontaneous Reaction First Law of Thermodynamics Second and Third Laws of Thermodynamics Entropy Gibbs Free Energy
Ch.18 - Electrochemistry
Redox Reaction Balancing Redox Reaction The Nernst Equation Faraday's Constant Galvanic Cell Cell Notation Standard Hydrogen Electrode Cell Potential Nernst Equation Batteries and Electricity Electroplating Electrolysis of Water & Mixture of Ions
Ch.19 - Nuclear Chemistry
Radioactive Decay Alpha Decay Beta Decay Gamma Emission Electron Capture Positron Emission Band of Stability First Order Half Life Nuclear Fission Mass Defect Nuclear Fusion Nuclear Transmutation
Ch.20 - Organic Chemistry
Introduction to Organic Chemistry Structural Formula Stereoisomers Chirality Optical Isomers The Alkyl Group Naming Alkanes Naming Alkenes Naming Alkynes Organic Chemistry Nomenclature Alkane Reactions Alkenes and Alkynes Functional Groups Alcohol Reactions Carboxylic Acid Derivative Reactions Polymer
Ch.22 - Chemistry of the Nonmetals
Alkali Metals
Ch.23 - Transition Metals and Coordination Compounds
Transition Metals Transition Metals Electron Configuration Oxidation States of Transition Metals Coordination Complexes Naming Coordination Compounds Coordination Isomers Crystal Field Theory Colors of Complex Ions