Lecture 5
... o Again, ν is the stoichiometric coefficient (by convention negative for reactants, positive for products) and the sum is over all compounds in the reaction. ...
... o Again, ν is the stoichiometric coefficient (by convention negative for reactants, positive for products) and the sum is over all compounds in the reaction. ...
2 Chemical equilibrium occurs when a reaction and its reverse
... The ratio of [NO2]2 to [N2O4] remains constant (within error) at this temperature no matter what the initial concentrations of NO2 and N2O4 are. ...
... The ratio of [NO2]2 to [N2O4] remains constant (within error) at this temperature no matter what the initial concentrations of NO2 and N2O4 are. ...
Ch 17 Equilibrium Notes
... • The state where the concentrations of all reactants and products remain constant with them. • All reactions are reversible. • Forward and reverse rates are equal at equilibrium. • Any chemical reaction carried out in a close vessel reaches equilibrium. • On the molecular level, there is frantic ac ...
... • The state where the concentrations of all reactants and products remain constant with them. • All reactions are reversible. • Forward and reverse rates are equal at equilibrium. • Any chemical reaction carried out in a close vessel reaches equilibrium. • On the molecular level, there is frantic ac ...
Chemistry and the material world
... The sign of ΔG tells us the direction in which a reaction will proceed to reach an equilibrium and the magnitude of ΔG tells us how far from equilibrium the reaction still is (ΔG = 0 means equilibrium). Thus, as the reaction progresses, the magnitude of ΔG will become smaller and smaller until an eq ...
... The sign of ΔG tells us the direction in which a reaction will proceed to reach an equilibrium and the magnitude of ΔG tells us how far from equilibrium the reaction still is (ΔG = 0 means equilibrium). Thus, as the reaction progresses, the magnitude of ΔG will become smaller and smaller until an eq ...
Equilibrium 4 Noteform - IndustrialProcesses
... The overall rate of the process depends on the STEP 2. We can apply Le Chatelier’s Principle to this reaction to find the conditions that most favour the formation of the product. ...
... The overall rate of the process depends on the STEP 2. We can apply Le Chatelier’s Principle to this reaction to find the conditions that most favour the formation of the product. ...
CH 17 Study Guide with answer Key
... equilibrium to the (14) ________________________ because the forward reaction liberates heat and removes the (15) ________________________. A (16) ________________________ speeds up a reaction by lowering the (17) ____________________ requirements for the reaction, but it does so equally in both the ...
... equilibrium to the (14) ________________________ because the forward reaction liberates heat and removes the (15) ________________________. A (16) ________________________ speeds up a reaction by lowering the (17) ____________________ requirements for the reaction, but it does so equally in both the ...
AP Chemistry: Chapter 13 Gaseous Equilibrium Section 1: Multiple
... (d) Calculate the partial pressure of S2(g) in the container at equilibrium at 483 K. (e) For the reaction H2(g) + S2(g) H2S(g) at 483 K, calculate the value of the equilibrium constant, Kc. ...
... (d) Calculate the partial pressure of S2(g) in the container at equilibrium at 483 K. (e) For the reaction H2(g) + S2(g) H2S(g) at 483 K, calculate the value of the equilibrium constant, Kc. ...
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.