a. Calculate Ea if k1 = 4.62 x 10 -7 1/Ms at 315 oC and k2...
a. Calculate Ea if k1 = 4.62 x 10 -7 1/Ms at 315 oC and k2 is 2.31 x 10 -4 1/Ms at 678 oC. b. Based on your answer to a, what’s k at 400 oC?
Homework Answers
(10) 1. The diprotic acid, H2A, has Kai i.e. (K1) = 1.00 X 10 and K2...
(10) 1. The diprotic acid, H2A, has Kai i.e. (K1) = 1.00 X 10 and K2 = 1.00 X 108. a) Consider a solution of 0.100 M H2A. Calculate the pH, and calculate the following concentrations: (H2A), (HA) and (A2). b) Consider a solution of 0.100 M NaHA. Calculate the pH, and calculate the following concentrations: (H2A), CHA') and (AP).
The diprotic acid, H2A, has Ka1 i.e. (K1) = 1.00 X 10-4 and K2 = 1.00...
The diprotic acid, H2A, has Ka1 i.e. (K1) = 1.00 X 10-4 and K2 = 1.00 X 10-8. a) Consider a solution of 0.100 M H2A. Calculate the pH, and calculate the following concentrations: [H2A], [HA- ] and [A2- ]. b) Consider a solution of 0.100 M NaHA. Calculate the pH, and calculate the following concentrations: [H2A], [HA- ] and [A2- ].
The following questions is based on ionization of carbonic acid. [H2CO3 = H+ + HCO3- K1 = 4.7 X 10-7, pK1 = 6.34 ] [HCO3- = H+ CO3-2 K2 = 4.4 X 10-11, pK2 = 10.36] Calculate the pH ofthe solution form...
The following questions is based on ionization of carbonic acid. [H2CO3 = H+ + HCO3- K1 = 4.7 X 10-7, pK1 = 6.34 ] [HCO3- = H+ CO3-2 K2 = 4.4 X 10-11, pK2 = 10.36] Calculate the pH ofthe solution form by mixing the following: a)50.0ml of 0.100 M H2CO3 with 50.0ml of 0.050 M NaOH . b)50.0ml of 0.100 M H2CO3 with 50.0ml of 0.150 M NaOH . c)50.0ml of 0.100 M H2CO3 with 50.0ml of 0.100 M...
[Rh(Cl)5(OH2)]2- undergoes dissociative ligand exchange. Ratios of k-1/k2 were obtained as shown ...
[Rh(Cl)5(OH2)]2- undergoes
dissociative ligand exchange. Ratios of k-1/k2 were obtained as
shown below/
I don't know the part C. Can you explain part C?
10) (10 marks) [Rh(ClI)s(OH2)]2- undergoes dissociative ligand exchange. Ratios of k-1/k2 were obtained as shown below. [Rh(Cl)5(OH2)]2. + X. Cl- N3- k-1/k2 62 7 (a) Do you expect kı and k-1 to change when X changes from Cl to N3? No (b) Provide a reasonable explanation for your answer in part (a). k1 k2 [Rh(Cl)512, +...
Learning Goal: To use the Arrhenius equation to calculate the activation energy. As temperature rises, the...
Learning Goal: To use the Arrhenius equation to calculate the activation energy. As temperature rises, the average kinetic energy of molecules increases. In a chemical reaction, this means that a higher percentage of the molecules possess the required activation energy, and the reaction goes faster. This relationship is shown by the Arrhenius equation k=Ae−Ea/RT where k is the rate constant, A is the frequency factor, Ea is the activation energy, R = 8.3145 J/(K⋅mol) is the gas constant, and T...
part 1 is wrong Calculate the pH of each solution. A solution containing 0.0243 M maleic...
part 1 is wrong
Calculate the pH of each solution. A solution containing 0.0243 M maleic acid and 0.034 M disodium maleate. The K, values for maleic acid are 1.20 x 10-?(K) and 5.37 x 10 (K2). pH = 2.00 A solution containing 0.0360 M succinic acid and 0.023 M potassium hydrogen succinate. The K, values for succinic acid are 6.21 x 10" (K1) and 2.31 x 10 "(K), pH = 4.01
1) Given the two reactions: a) H2S<--> HS- + H+, K1=9.13 x 10-8 b) HS-<--> S2-...
1) Given the two reactions: a) H2S<--> HS- + H+, K1=9.13 x 10-8 b) HS-<--> S2- + H+, K2=1.20 x 10-19 what is the equilibrium constant Kfinal for thefollowing reaction? S2- + 2H+<--> H2S 2) Given the two reactions: a)PbCl2 <--> Pb2+ + 2Cl-,K1= 1.80 x 10-10 b) AgCl<--> Ag+ + Cl-, K2= 1.23 x10-4 what is the equilibrium constant Kfinal for thefollowing reaction? PbCl2 + 2Ag+<--> 2AgCl + Pb2+
Lunes CHEMWORK The Hg2+ ion forms complex ions with I as follows: Hg2+ + HgT+ HgI + 1 =Hg2 K1 = 1.0 108 K2=1.0 x 10...
Lunes CHEMWORK The Hg2+ ion forms complex ions with I as follows: Hg2+ + HgT+ HgI + 1 =Hg2 K1 = 1.0 108 K2=1.0 x 105 K3 -1.0 x 10° K4 = 1.0 * 108 Hgl2 + 1 + HgI3 HgI3 + 1 = Hg142 A solution is prepared by dissolving 0.057 mol Hg(NO3)2 and 5.00 mol Nal in enough water to make 1.0 L of solution. Calculate the equilibrium concentration of [Hg142]. (Hg142) = M Calculate the equilibrium concentration...
7) Calculate the key of a reaction at 315 °K and a AG° = -35.7 kJ/mol....
7) Calculate the key of a reaction at 315 °K and a AG° = -35.7 kJ/mol. Is the reaction favorable? a. Keq = 8.38*10°; exergonic b. Keq = 8.38*10-5; endergonic c. Keg = 3.76*10°; exergonic d. Keq = 3.76*10-4; endergonic
1) Calculate the activation energy (Ea) of a reaction having a rate constant of 1.78 X...
1) Calculate the activation energy (Ea) of a reaction having a rate constant of 1.78 X 10^-3 MS at 34.5C and a rate constant at 52C of 1.40x10^-2 MS. Could you please give step by step. Unsure of what to do after plugging numbers into the equation.
(10) 1. The diprotic acid, H2A, has Kai i.e. (K1) = 1.00 X 10 and K2 = 1.00 X 108. a) Consider a solution of 0.100 M H2A. Calculate the pH, and calculate the following concentrations: (H2A), (HA) and (A2). b) Consider a solution of 0.100 M NaHA. Calculate the pH, and calculate the following concentrations: (H2A), CHA') and (AP).
[Rh(Cl)5(OH2)]2- undergoes
dissociative ligand exchange. Ratios of k-1/k2 were obtained as
shown below/
I don't know the part C. Can you explain part C?
10) (10 marks) [Rh(ClI)s(OH2)]2- undergoes dissociative ligand exchange. Ratios of k-1/k2 were obtained as shown below. [Rh(Cl)5(OH2)]2. + X. Cl- N3- k-1/k2 62 7 (a) Do you expect kı and k-1 to change when X changes from Cl to N3? No (b) Provide a reasonable explanation for your answer in part (a). k1 k2 [Rh(Cl)512, +...
part 1 is wrong
Calculate the pH of each solution. A solution containing 0.0243 M maleic acid and 0.034 M disodium maleate. The K, values for maleic acid are 1.20 x 10-?(K) and 5.37 x 10 (K2). pH = 2.00 A solution containing 0.0360 M succinic acid and 0.023 M potassium hydrogen succinate. The K, values for succinic acid are 6.21 x 10" (K1) and 2.31 x 10 "(K), pH = 4.01
Lunes CHEMWORK The Hg2+ ion forms complex ions with I as follows: Hg2+ + HgT+ HgI + 1 =Hg2 K1 = 1.0 108 K2=1.0 x 105 K3 -1.0 x 10° K4 = 1.0 * 108 Hgl2 + 1 + HgI3 HgI3 + 1 = Hg142 A solution is prepared by dissolving 0.057 mol Hg(NO3)2 and 5.00 mol Nal in enough water to make 1.0 L of solution. Calculate the equilibrium concentration of [Hg142]. (Hg142) = M Calculate the equilibrium concentration...
7) Calculate the key of a reaction at 315 °K and a AG° = -35.7 kJ/mol. Is the reaction favorable? a. Keq = 8.38*10°; exergonic b. Keq = 8.38*10-5; endergonic c. Keg = 3.76*10°; exergonic d. Keq = 3.76*10-4; endergonic
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