physics/0010052 PDF
... Pay attention that if P=const and A is the work of expansion then dQ and dA=PdV are exact differentials. Let's consider heat exchange, one introduces the quantity of heat ∆Q in the system (∆V=0): ∆Q=∆U. Now let's suppose ∆V>0. Let's find out, is it necessary to write ∆Q=∆U-P∆V or ∆Q=∆U+P∆V. It is ne ...
... Pay attention that if P=const and A is the work of expansion then dQ and dA=PdV are exact differentials. Let's consider heat exchange, one introduces the quantity of heat ∆Q in the system (∆V=0): ∆Q=∆U. Now let's suppose ∆V>0. Let's find out, is it necessary to write ∆Q=∆U-P∆V or ∆Q=∆U+P∆V. It is ne ...
Ch. 2 The Chemistry of Life
... - Adhesion – an _______________ between molecules of _______________ substances o Ex.) __________ molecules to __________ ...
... - Adhesion – an _______________ between molecules of _______________ substances o Ex.) __________ molecules to __________ ...
I PUC Chemistry Mock Paper
... a) Explain Born- Haber cycle for the formation of one mole of NaCl b) Distinguish between closed and isolated system. ...
... a) Explain Born- Haber cycle for the formation of one mole of NaCl b) Distinguish between closed and isolated system. ...
Equilibrium notes (complete)
... equilibrium with the reactants at one side of the tub and the products at the other. • If you dump some water at one end of the tub the water flows towards the other end of the tub to reestablish equilibrium • If you scoop out some water at one end of the tub the water flows back towards the “hole” ...
... equilibrium with the reactants at one side of the tub and the products at the other. • If you dump some water at one end of the tub the water flows towards the other end of the tub to reestablish equilibrium • If you scoop out some water at one end of the tub the water flows back towards the “hole” ...
quarter 4 final exam guide - District 196 e
... Draw a potential energy diagram representing an endothermic reaction. Label your axes. Label reactants, products, activated complex, activation energy and net energy absorbed. ...
... Draw a potential energy diagram representing an endothermic reaction. Label your axes. Label reactants, products, activated complex, activation energy and net energy absorbed. ...
Chemistry I Final Review
... 52. How many grams of potassium bromide should be added to water to prepare 0.50 L of solution with a molarity of 0.125 M? ...
... 52. How many grams of potassium bromide should be added to water to prepare 0.50 L of solution with a molarity of 0.125 M? ...
CYL110
... When a system is at equilibrium, its state is defined entirely by the state variables, and not by the history of the system. The properties of the system can be described by an equation of state which specifies the relationship between these variables. ...
... When a system is at equilibrium, its state is defined entirely by the state variables, and not by the history of the system. The properties of the system can be described by an equation of state which specifies the relationship between these variables. ...
Equilibrium - Clayton State University
... - Many reactions do not go to completion - Amount of products formed or reactants consumed cannot be predicted from stoichiometry alone - These reactions achieve a condition of equilibrium ...
... - Many reactions do not go to completion - Amount of products formed or reactants consumed cannot be predicted from stoichiometry alone - These reactions achieve a condition of equilibrium ...
Objectives - Dixie State University
... III. Thermodynamics of Reactions What thermodynamics tells you 1. Explain what thermodynamics of a reaction tells us, and why this is important. What equilibrium is 2. Explain what is happening to the rates of the reactions and the concentrations of the reactants in both reactions when the reaction ...
... III. Thermodynamics of Reactions What thermodynamics tells you 1. Explain what thermodynamics of a reaction tells us, and why this is important. What equilibrium is 2. Explain what is happening to the rates of the reactions and the concentrations of the reactants in both reactions when the reaction ...
111 Exam III OUTLINE TRO 1-3-11
... 1. The forward reaction (⇀ ) and reverse (↽ ) reactions are occurring simultaneously. 2. The rate for the forward reaction is equal to the rate of the reverse reaction and a dynamic equilibrium is achieved. 3. The ratio of the concentrations of the products to reactants is constant. B. THE EQUILIBRI ...
... 1. The forward reaction (⇀ ) and reverse (↽ ) reactions are occurring simultaneously. 2. The rate for the forward reaction is equal to the rate of the reverse reaction and a dynamic equilibrium is achieved. 3. The ratio of the concentrations of the products to reactants is constant. B. THE EQUILIBRI ...
Spectrum05
... The rate of the forward reaction is equal to the rate of the reverse reaction. The concentration of products and reactants stays the same, but the reactions are still running. ...
... The rate of the forward reaction is equal to the rate of the reverse reaction. The concentration of products and reactants stays the same, but the reactions are still running. ...
Chapter 15. Chemical Equilibrium
... with constant concentrations of nitrogen, hydrogen, and ammonia. However, if we start with just ammonia and no nitrogen or hydrogen, the reaction will proceed and N2 and H2 will be produced until equilibrium is achieved. No matter what the starting composition of reactants and products is, the equil ...
... with constant concentrations of nitrogen, hydrogen, and ammonia. However, if we start with just ammonia and no nitrogen or hydrogen, the reaction will proceed and N2 and H2 will be produced until equilibrium is achieved. No matter what the starting composition of reactants and products is, the equil ...
Lecture 5 - Thermodynamics II
... which occurs at constant T, P G = U + PV – TS = H – TS (dH = dU + PdV + VdP) • The total differential is: dG = dU + PdV + VdP – TdS – SdT G is therefore the energy that can run a process at constant P, T (though it can be affected by changing P and T) Reactions that have potential energy in a system ...
... which occurs at constant T, P G = U + PV – TS = H – TS (dH = dU + PdV + VdP) • The total differential is: dG = dU + PdV + VdP – TdS – SdT G is therefore the energy that can run a process at constant P, T (though it can be affected by changing P and T) Reactions that have potential energy in a system ...
國立嘉義大學95學年度
... 2NO(g) + Br (g) . After equilibrium was reached, the volume was increased to 2.0 liters, while the temperature was 44. 2NOBr(g) ...
... 2NO(g) + Br (g) . After equilibrium was reached, the volume was increased to 2.0 liters, while the temperature was 44. 2NOBr(g) ...
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.