Let's write the equations for Kn, Ka, Kb and Kw.
Therefore, by substituting each of the above terms into our equation for Kn, we can get the following.
The equilibrium constant, K. for a neutralization reaction can be symbolized as K_n. Using K_w, and...
Consider the following reaction which is at equilibrium at 25 degree C: NH_4(NH_2CO_2)(s) 2 NH_3(g) + CO_2(g), delta H degree = 152.2 kJ In which direction will the reaction shift if? *(a) the pressure is increased (b) the pressure decreased (c) the temperature is increased (d) the temperature is decreased (e) some CO_2 is added (f) NH_3 is removed (g) a catalyst is added (h) some NH_4(NH_2CO_2) is added (i) some Ne is added; and, (j) the volume is increased
Using the reduction potentials given, calculate the equilibrium constant, K, at 20 degrees C for the reaction Using the reduction potentials given, calculate the equilibrium constant, K, at 25°C for the reaction, 33 3+ Ag (aa) t Fe(a)Ag) Fe (aq) +0.77 V +0.80 V A Ag+(aq) + e- ← a. 1.66 b. 6.4 c. 3.2 d. 6.1 x 10-4 e. 1.6 x 104 Rank the following compounds according to increasing solubility in water. K” is a less than sign) 34...
Predict the direction in which the equilibrium will lie for the following reaction: C_6H_5COO^- + HF C_6H_5COOH + F^- K_a (C_6H_5 COOH) = 6.5 Times 10^ - 5; K_a (HF) = 7.1 Times 10^ - 4 Which of the following yields a basic solution when dissolved in water? NH_3, Na_2O LiOH CO_2 1 and II 1 and III 1, III, and IV 1, II, and III 1, II, III, and IV Calculate the pH of a 6.7 Times 10^-2 M...
Write an equation for the reaction of each of the following with water a) HNO_3 b) HCOOH c) NaOH d) NH_3 (2) Identify the conjugate acid-base pairs in each of the following chemical reactions: a) NH_4^+(aq) + CN^-(aq) NH_3(aq) + HCN(aq) b) CO_3^2-(aq) + HCI(aq) HCO_3^-(aq) + CI^_(aq) c) HCI(aq) + OH^-(aq) H_2O(aq) + CI^-(aq) (3) Classify each of the following as Bronsted acid, Bronsted base, or both in aqueous solution: a) NH_4^+ b) NH_3 c) H_2CO_3 d) HCO_3^- e)...
6) Calculate the equilibrium constant K at 25°C for the following reaction for tant K at 25°C for the following reaction for the standard cell potential (7 points) (nFEⓇ - RT In K, F=96485 C/mol.R=8.31 J/molk) Pb2+ (aq) + Fe(s) 5 Pb(8) + Fe²(aq) 7) Calculate the cell potential of the following cell at 25°C. (7 points) Fe(s) | Fe*(aq) (1.1 M) || Cu?" (aq) (0.50 M) Cu() Ecell - Eºcell = 0.0592/n logQ
6) Calculate the equilibrium constant K at 25°C for the the equilibrium constant K at 25°C for the following reaction for the standard cell potential: (points) (AFE-R7 In K, F-96485 Címol,R-8.37 J/molk) Pb2+ (aq) + Fe(s) S Pb(s) + Fe?*(aq) 7) Calculate the cell potential of the following cell at 25°C. (7 points) Fe(s)| Fe?"(aq) (1.1 M) || Cu?"(aq) (0.50 M) Cu(3) Ecall-E Call - 0.0592/n logo
Calculate the equilibrium constant K for the following reaction at 25 degrees celcius from standard electrode potentials for the following reaction: Sn^4+(aq) + 2Hg(l) = Sn^2+(aq) + Hg2^2+(aq)
Question 3 35 pts Determine the value of the equilibrium constant (K) for the reaction listed below based on the concentrations provided. Alaq) + 2 B(aq) = 3(aq) + D(aq) Reagent/Product A B C D 0.17 0.69 149 0.87 Concentration (mol/L) Question 4 35 pts Determine the equilibrium molar concentration of C in the following reaction if the initial molar concentration of Ais 0.10 M and Bis 0.25 M. The equilibrium constant for the reaction is 78. A(aq) + B(aq)...
Write the chemical reaction for the autoionization of water (equilibrium constant Kw). Look up the numerical value for Kw at Tinitial (Use the average of Tinitial from both trials) -Its 6.81x10^-15 How is the equation in Question 1 related to the net ionic equation for the strong acid-strong base neutralization shown below? H3O+(aq) + OH-(aq) → H2O(l) + H2O(l) Use the value of Kw and the relationship between the equations in Questions 1 and 3 to find the numerical value...
cell = 0.74 V. Calculate the equilibrium constant, K. For the following redox reaction at 25 °C, E° Cd(s) + Cu 2+ (aq) → Cd 2+ (aq) + Cu(s)