Chemistry Homework Help

24/7 Chemistry Homework Help

Get step-by-step solutions from expert tutors.

Please include all instructions needed to answer the question and submit one question at a time to ensure faster response.

How it works?

Ask a question

Type, take a picture, or paste your question with all necessary details to ensure high-quality responses.

Get an answer in less than 24hrs

Once our tutors receive the question, they'll begin. You'll get an email once the solution is ready.

Get Notified

We will send you email and text notification to let you know when your question is answered.

Browse Homework Solutions

7 solutions

Henry's Law

Q. Calculate the mass of oxygen (in mg) dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air. Assume the mole fraction of oxygen in air to be 0.21 and the Henry's law constant for oxygen in water at this temperature to be 1.3 × 10^-3 M/atm. A) 27.3 mg B) 23.5 mg C) 13.7 mg D) 49.4 mg E) 47.0 mg

Solved • Jul 15, 2019

Henry's Law

Q. Determine the Henry's law constant for ammonia in water at 25°C if an ammonia pressure of 0.022 atm produces a solution with a concentration of 1.3 M. A) 35 M/atm B) 59 M/atm C) 0.038 M/atm D) 0.017 M/atm E) 0.029 M/atm

Solved • Jul 15, 2019

Henry's Law

Q. Determine the partial pressure of oxygen necessary to form an aqueous solution that is 4.1 × 10^-4 M O2 at 25°C. The Henry's law constant for oxygen in water at 25°C is 1.3 × 10^-3 M/atm. A) 0.24 atm B) 1.9 atm C) 0.32 atm D) 0.53 atm E) 0.77 atm

Solved • Jul 15, 2019

Henry's Law

Q. The Henrys Law constant for CO2 is 3.6x10-2 M/atm at 25oC. What pressure (jn atm) of carbon dioxide is needed to maintain a CO2 concentration of 0.083 M in a can of lemon lime soda?

Solved • Jun 25, 2019

Henry's Law

Q. At 4oC and 1.00 atm as much as 0.0641 g of O2 can dissolve in 1 L of water. At 4oC and 5.20 atm, how many grams of O2 dissolve in 1 L of water

Solved • Jun 25, 2019

Henry's Law

Q. 31) An increase in the temperature of the solution usually 32) KBr does not dissolve well in nonpolar solvents because

Solved • Jun 14, 2019

Henry's Law

Q. In which case should CO2(g) be more soluble in water? a) The total pressure is 5 atm and the partial pressure of CO2 is 1 atm b) The total pressure is 3 atm and the partial pressure of CO2 is 3 atm c) The total pressure is 1 atm and the partial pressure of CO2 is 0.5 atm a) The total pressure is 1 atm and the partial pressure of CO2 is 0.03 atm

Solved • Jun 14, 2019

Filter by topic

Ch.1 - Intro to General Chemistry
Mixtures Scientific Notation Accuracy & Precision Standard Deviation, Mean, Median & Mode Metric Prefixes Significant Figures Energy, Heat and Temperature Physical & Chemical Changes Physical & Chemical Properties Dimensional Analysis Density
Ch.2 - Atoms & Elements
Periodic Table Periodic Table Charges Mole Concept Calculating Molar Mass Isotopes Subatomic Particles Atomic Theory
Ch.3 - Chemical Reactions
Ionic and Covalent Bonds Molecular Models Polyatomic Ions Naming Covalent Compounds Naming Ionic Compounds Empirical Formula Molecular Formula Combustion Analysis Mass Percent Formula Balancing Chemical Equations Stoichiometry Theoretical Yield Limiting Reagent Limiting Reactant Percent Yield
BONUS: Lab Techniques and Procedures
Distillation & Floatation Test for Ions and Gases
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 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 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 Electron Capture Positron Emission Band of Stability First Order Half Life Nuclear Fission Mass Defect Nuclear Transmutation
Ch.20 - Organic Chemistry
Introduction to Organic Chemistry Structural Formula Stereoisomers Chirality Optical Isomers The Alkyl Group Naming Alkanes Naming Alkenes Organic Chemistry Nomenclature Functional Groups Alcohol Reactions Carboxylic Acid Derivative Reactions Polymer
Ch.23 - Transition Metals and Coordination Compounds
Transition Metals Transition Metals Electron Configuration Coordination Complexes Naming Coordination Compounds Coordination Isomers Crystal Field Theory Colors of Complex Ions