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Physical Chemistry and Nuclear Chemistry
Physical chemistry is the study of macroscopic, and particulate phenomena in chemical systems in terms of the principles, practices, and concepts of physics such as motion, energy, force, time, thermodynamics, quantum chemistry, statistical mechanics, analytical dynamics and chemical equilibrium.
- Voordeelbundel
- • 16 items •
- Radiocarbon • College aantekeningen
- Nuclear Chemistry • College aantekeningen
- Catalysis and reaction mechanism • College aantekeningen
- Collision Theory • College aantekeningen
- Activation energy • College aantekeningen
- En meer ….
Physical chemistry is the study of macroscopic, and particulate phenomena in chemical systems in terms of the principles, practices, and concepts of physics such as motion, energy, force, time, thermodynamics, quantum chemistry, statistical mechanics, analytical dynamics and chemical equilibrium.
Introduction to Physical Chemistry
Physical chemistry is the study of macroscopic, and particulate phenomena in chemical systems in terms of the principles, practices, and concepts of physics such as motion, energy, force, time, thermodynamics, quantum chemistry, statistical mechanics, analytical dynamics and chemical equilibrium.
- Boek & Voordeelbundel
- College aantekeningen
- • 14 pagina's •
Physical chemistry is the study of macroscopic, and particulate phenomena in chemical systems in terms of the principles, practices, and concepts of physics such as motion, energy, force, time, thermodynamics, quantum chemistry, statistical mechanics, analytical dynamics and chemical equilibrium.
Chemical kinetics
rate (kinetics) Kinetics: Rate. Chemical Kinetics - The study of the rates of chemical reactions. Rate of a Reaction - The change in concentration of one of the reactants (DX), during a given period of time (Dt) The reaction rate gradually decreases as reactants are consumed.
- Boek & Voordeelbundel
- College aantekeningen
- • 16 pagina's •
rate (kinetics) Kinetics: Rate. Chemical Kinetics - The study of the rates of chemical reactions. Rate of a Reaction - The change in concentration of one of the reactants (DX), during a given period of time (Dt) The reaction rate gradually decreases as reactants are consumed.
Reaction rate(average rates and Instantenous rates)
Reaction rate, in chemistry, the speed at which a chemical reaction proceeds. It is often expressed in terms of either the concentration (amount per unit volume) of a product that is formed in a unit of time or the concentration of a reactant that is consumed in a unit of time.
- Boek & Voordeelbundel
- College aantekeningen
- • 12 pagina's •
Reaction rate, in chemistry, the speed at which a chemical reaction proceeds. It is often expressed in terms of either the concentration (amount per unit volume) of a product that is formed in a unit of time or the concentration of a reactant that is consumed in a unit of time.
Rate laws
Because the rate of a reaction has dimensions of concentration per unit time, the dimensions of the rate constant k depend on the exponents of the concentration terms in the rate law. If p is the sum of the exponents of the concentration terms in the rate law, p=a b
- Boek & Voordeelbundel
- College aantekeningen
- • 17 pagina's •
Because the rate of a reaction has dimensions of concentration per unit time, the dimensions of the rate constant k depend on the exponents of the concentration terms in the rate law. If p is the sum of the exponents of the concentration terms in the rate law, p=a b
Activation energy calculations
Step 1: Convert temperatures from degrees Celsius to Kelvin. T = degrees Celsius 273.15. T1 = 3 273.15. ... Step 2 - Find Ea ln(k2/k1) = Ea/R x (1/T1 - 1/T2) ln(7.1 x 10-2/8.9 x 10-3) = Ea/8.3145 J/K·mol x (1/276.15 K - 1/308.15 K) ... Answer: The activation energy for this reaction is 4.59 x 104 J/mol or 45.9 kJ/mol.
- Boek & Voordeelbundel
- College aantekeningen
- • 10 pagina's •
Step 1: Convert temperatures from degrees Celsius to Kelvin. T = degrees Celsius 273.15. T1 = 3 273.15. ... Step 2 - Find Ea ln(k2/k1) = Ea/R x (1/T1 - 1/T2) ln(7.1 x 10-2/8.9 x 10-3) = Ea/8.3145 J/K·mol x (1/276.15 K - 1/308.15 K) ... Answer: The activation energy for this reaction is 4.59 x 104 J/mol or 45.9 kJ/mol.
Intergrated rate laws
The rate law is a differential equation, meaning that it describes the change in concentration of reactant(s) per change in time. Using calculus, the rate law can be integrated to obtain an integrated rate equation that links concentrations of reactants or products with time directly.
- Boek & Voordeelbundel
- College aantekeningen
- • 9 pagina's •
The rate law is a differential equation, meaning that it describes the change in concentration of reactant(s) per change in time. Using calculus, the rate law can be integrated to obtain an integrated rate equation that links concentrations of reactants or products with time directly.
Half life reactions
The half-life of a reaction, t1/2, is the amount of time needed for a reactant concentration to decrease by half compared to its initial concentration. Its application is used in chemistry and medicine to predict the concentration of a substance over time.
- Boek & Voordeelbundel
- College aantekeningen
- • 23 pagina's •
The half-life of a reaction, t1/2, is the amount of time needed for a reactant concentration to decrease by half compared to its initial concentration. Its application is used in chemistry and medicine to predict the concentration of a substance over time.
Rate constants and Order of reactions
k is the first-order rate constant, which has units of 1/s. The method of determining the order of a reaction is known as the method of initial rates. The overall order of a reaction is the sum of all the exponents of the concentration terms in the rate equation.
- Boek & Voordeelbundel
- College aantekeningen
- • 39 pagina's •
k is the first-order rate constant, which has units of 1/s. The method of determining the order of a reaction is known as the method of initial rates. The overall order of a reaction is the sum of all the exponents of the concentration terms in the rate equation.
Activation energy
Activation energy, in chemistry, the minimum amount of energy that is required to activate atoms or molecules to a condition in which they can undergo chemical transformation or physical transport.The role of activation energy in a chemical reaction is to start the reaction by arranging the reactants appropriately and breaking their existing...
- Boek & Voordeelbundel
- College aantekeningen
- • 16 pagina's •
Activation energy, in chemistry, the minimum amount of energy that is required to activate atoms or molecules to a condition in which they can undergo chemical transformation or physical transport.The role of activation energy in a chemical reaction is to start the reaction by arranging the reactants appropriately and breaking their existing...