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11 Nov 2019
Please help a-f! Thank you!
reduce it. Adding more reactant or product, will shift the equilsbrium to . Taking away reactant or produet, will shift the equilibrium to replace it Treat heat as if it was a product (for exothermie reactions) or a reactant (for endothermic reactions) when increasing or decreasing the temperature the change . with the least number of moles of gas.[Decreasing pressure will have the opposite affeet, the reaction shifts to the side wsth the most moles of gas.] . Inereasing pressure (hy decreasing volume) will shift the equilibrium to the side of the reaction Solve the following problems. . Consider a set of simple reactions Where Ratesnn kA) and Ratepre koB 30 90 0.20 0.40 50 0.60 60 60 0.20 0.60 a. What is the distinetion between [Al, and [AJey in the column heading? b. For Trial M2, calculate the rate of the forward reaction (A âB) at equilibrium and the rate of the reverse reaction (BâA) at equilibrunn. How do these values compare? For Trial P2, calculate the rate of the forward reaction (A âB) at equilibrium and the rate of the reverse reaction (BâA) at equilibrium. How do these values compare? c. d. Examine the table above: i. If k k, what are the relative values of the equilibrium concentrations of A and B? Explain. B) at equilibrium compare to the rate of the reverse reaction (BâA) at equilibrium? LB) f. Show that is a constant for trial 1 and 2 for each set.
Please help a-f! Thank you!
reduce it. Adding more reactant or product, will shift the equilsbrium to . Taking away reactant or produet, will shift the equilibrium to replace it Treat heat as if it was a product (for exothermie reactions) or a reactant (for endothermic reactions) when increasing or decreasing the temperature the change . with the least number of moles of gas.[Decreasing pressure will have the opposite affeet, the reaction shifts to the side wsth the most moles of gas.] . Inereasing pressure (hy decreasing volume) will shift the equilibrium to the side of the reaction Solve the following problems. . Consider a set of simple reactions Where Ratesnn kA) and Ratepre koB 30 90 0.20 0.40 50 0.60 60 60 0.20 0.60 a. What is the distinetion between [Al, and [AJey in the column heading? b. For Trial M2, calculate the rate of the forward reaction (A âB) at equilibrium and the rate of the reverse reaction (BâA) at equilibrunn. How do these values compare? For Trial P2, calculate the rate of the forward reaction (A âB) at equilibrium and the rate of the reverse reaction (BâA) at equilibrium. How do these values compare? c. d. Examine the table above: i. If k k, what are the relative values of the equilibrium concentrations of A and B? Explain. B) at equilibrium compare to the rate of the reverse reaction (BâA) at equilibrium? LB) f. Show that is a constant for trial 1 and 2 for each set.
Deanna HettingerLv2
25 Mar 2019