1.Calculate the normality of the solutions containing 5.267g/L K2Cr2O7 (the Cr is reduced to Cr3+). (FW=294.19 g/mol) 2.A and B react as follows: A + B 2C. The equilibrium constant is 5.0 x 106 . If 0.40 mol of A and 0.70 mol of B are mixed in 1L, what are the concentrations of A, B and C after reaction? 3. The following data is given at a certain temperature: (1) 2N2 (g) + O2 (g) 2N2O (g) K1 = 1.2 x 10-35 (2) N2O4 (g) 2NO2 (g) K2 = 4.6 x 10-3 (3) ½N2 (g) + O2 (g) NO2 (g) K3 = 4.1 x 10-9 Calculate the molar equilibrium constant, K for the reaction: 2N2O (g) + 3O2 (g) 2N2O4 (g)
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Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
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1.Calculate the normality of the solutions containing 5.267g/L K2Cr2O7 (the Cr is reduced to Cr3+).
(FW=294.19 g/mol)
2.A and B react as follows: A + B 2C. The equilibrium constant is 5.0 x 106
. If 0.40 mol of A
and 0.70 mol of B are mixed in 1L, what are the concentrations of A, B and C after reaction?
3. The following data is given at a certain temperature:
(1) 2N2 (g) + O2 (g) 2N2O (g) K1 = 1.2 x 10-35
(2) N2O4 (g) 2NO2 (g) K2 = 4.6 x 10-3
(3) ½N2 (g) + O2 (g) NO2 (g) K3 = 4.1 x 10-9
Calculate the molar equilibrium constant, K for the reaction:
2N2O (g) + 3O2 (g) 2N2O4 (g)
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