Semester 2 Final Exam
... energy, its temperature increases from 10°C to 47°C. What is the mass of this block? (c of Al = 0.900 J/g·°C) (A) 0.055 g (B) 14.6 g (C) 18.0 g (D) 33.3 g 6. The units for heat are: (A) J (B) J/g (C) J/g·°C (D) J/°C 7. 20.0 gram samples of each of the following metals are originally at 10°C. They ar ...
... energy, its temperature increases from 10°C to 47°C. What is the mass of this block? (c of Al = 0.900 J/g·°C) (A) 0.055 g (B) 14.6 g (C) 18.0 g (D) 33.3 g 6. The units for heat are: (A) J (B) J/g (C) J/g·°C (D) J/°C 7. 20.0 gram samples of each of the following metals are originally at 10°C. They ar ...
AS Paper 1 Practice Paper 12 - A
... Write an expression for the equilibrium constant, Kc, for this reaction. Calculate the value of this constant at temperature T and give its units. Expression for Kc .......................................................................................... ...
... Write an expression for the equilibrium constant, Kc, for this reaction. Calculate the value of this constant at temperature T and give its units. Expression for Kc .......................................................................................... ...
Chapter 2 Chemical Reactions
... Atoms can not be created or destroyed (Law of Conservation of Mass) A reaction can be described several ways: #1. In a sentence every item is a word Copper reacts with chlorine to form copper (II) ...
... Atoms can not be created or destroyed (Law of Conservation of Mass) A reaction can be described several ways: #1. In a sentence every item is a word Copper reacts with chlorine to form copper (II) ...
Equilibrium STUDY GUIDE by Keshara Senanayake ---
... equilibrium can be described by the same equilibrium constant. You can see that the equilibrium state can be attained beginning with either product or reactant -- so the equilibrium state can be reached from either direction the forward or reverse reaction. Each set of equilibrium concentrations is ...
... equilibrium can be described by the same equilibrium constant. You can see that the equilibrium state can be attained beginning with either product or reactant -- so the equilibrium state can be reached from either direction the forward or reverse reaction. Each set of equilibrium concentrations is ...
Unit 5 Study Guide
... Unit 5 Study Guide: Chemical Reactions 1. What are the 7 diatomic molecules? ...
... Unit 5 Study Guide: Chemical Reactions 1. What are the 7 diatomic molecules? ...
Acid-Base Theories Arrhenius Acids and Bases • An acid is a
... between an electron-pair donor and an electron-pair acceptor. ...
... between an electron-pair donor and an electron-pair acceptor. ...
File
... One that proceeds without any outside assistance; spontaneous in one direction but not the opposite ...
... One that proceeds without any outside assistance; spontaneous in one direction but not the opposite ...
Physical Chemistry
... Intensive and extensive properties Equation of state (brief review) Ideal gas properties Gas Mixtures: Dalton’s law and Partial Pressure Condensed phase Properties of liquid Thermal compressibility and volume expansivity Vapor pressure Thermodynamic terms Heat and work 1st law thermodynamics basic c ...
... Intensive and extensive properties Equation of state (brief review) Ideal gas properties Gas Mixtures: Dalton’s law and Partial Pressure Condensed phase Properties of liquid Thermal compressibility and volume expansivity Vapor pressure Thermodynamic terms Heat and work 1st law thermodynamics basic c ...
List Definition Chemistry - A Level / Secondary Chemistry Tuition
... increases when the matter or energy in the system becomes more random in its arrangement. A system that has a high degree of disorder/randomness is said to have a large entropy. Gases have the highest entropy followed by liquids and solids. ...
... increases when the matter or energy in the system becomes more random in its arrangement. A system that has a high degree of disorder/randomness is said to have a large entropy. Gases have the highest entropy followed by liquids and solids. ...
Nature of chemical reaction - Environmental-Chemistry
... between the reactants and products of a reaction. CH4 + 2O2 → CO2 + 2H2O + ENERGY CH4 + 2O2 are called reactants that participate in reaction, and reactants are always written at left side of equation. CO2 + 2H2O called products that is formed as a result of reaction and products are always written ...
... between the reactants and products of a reaction. CH4 + 2O2 → CO2 + 2H2O + ENERGY CH4 + 2O2 are called reactants that participate in reaction, and reactants are always written at left side of equation. CO2 + 2H2O called products that is formed as a result of reaction and products are always written ...
Chapter 6-student notes
... Magnesium metal reacts with nitric acid (HNO3) to form hydrogen gas and magnesium nitrate. Step 1: Write the word equation for the reaction ...
... Magnesium metal reacts with nitric acid (HNO3) to form hydrogen gas and magnesium nitrate. Step 1: Write the word equation for the reaction ...
CHEMISTRY
... supplied by electricity or heat ex. electrolysis – decomposition of a substance by an electric current ...
... supplied by electricity or heat ex. electrolysis – decomposition of a substance by an electric current ...
Equilibrium at constant temperature and pressure: Gibbs Free
... Thus, instead of keeping the internal energy of the system constant, we would like to keep the temperature and pressure or temperature and volume constant, and predict how the system changes when various thermodynamic driving forces are applied (for our test tube example, perhaps we want to carry ou ...
... Thus, instead of keeping the internal energy of the system constant, we would like to keep the temperature and pressure or temperature and volume constant, and predict how the system changes when various thermodynamic driving forces are applied (for our test tube example, perhaps we want to carry ou ...
Chemical equilibrium
In a chemical reaction, chemical equilibrium is the state in which both reactants and products are present in concentrations which have no further tendency to change with time. Usually, this state results when the forward reaction proceeds at the same rate as the reverse reaction. The reaction rates of the forward and backward reactions are generally not zero, but equal. Thus, there are no net changes in the concentrations of the reactant(s) and product(s). Such a state is known as dynamic equilibrium.