3) (4 pts) Given the reaction and dissociation constant below, write the corresponding formation reaction and...
2. For the acid dissociation reaction below, the equilibrium concentrations are given as [H'] = 0.0060 M, [C2H302] =0.0060 M and the equilibrium constant, K is given as 1.8 x10-5. HC2H3O2 (aq) + (aq) + C2H:O2 (aq) a) Write the equilibrium constant expression for the reaction b) Calculate the concentration of HC2H302 at equilibrium
a) Write the dissociation reaction and corresponding K, expression for CH3NHs in water 8. b) Write the reaction with water and corresponding Ko expression for aniline (CGHsNH2) 9 A typical sample of vinegar has pH of 3.0. Assuming the vinegar in only an aqueous solution of acetic acid (Ka 1.8 x 105), calculate the concentration of acetic acid in vinegar? 10. Calculate the pH of a solution that contains 1.0 M HF (K-7.2x10) and 1.0 M CHsOH (K-1.6x1010). Calculate the...
Answer the following questions on this sheet or in your laboratory notebook. The reaction for the formation of diamminesilver ion is as follows: Ag + (aq) + 2 NH3 (aq) Ag(NH3)2 + (2 points). 1. Write the equilibrium constant expression for the reaction 2. An experiment was carried out to determine the value of the equilibrium constant, Kc for the reaction. Total moles of Ag+ present= 3.6 x 10 -3 moles Total moles of NH3 present =...
The reaction for the formation of ammonia is shown as: N2(g) + 3 H2(g) ⇄ 2 NH3(g) Kc=? Write the equilibrium constant expression (Kc) for this reaction. Calculate the value of Kc at 500. K for the formation of ammonia in part a) using the following measured concentrations for the equilibrium mixture: [N2] = 3.0 x 10-‐2 M; [H2] = 3.7 x 10-‐2 M; [NH3] = 1.6 x 10-‐2 M. [1.7 x 102] Now, calculate the value of Kc for the formation of...
The formation constant for [Cu(NH3)4]2+ is 5.00 × 1012. What is the equilibrium expression for this value? Group of answer choices Kf = 1/[[Cu(NH3)4]2+] Kf = [Cu2+][NH3]4/[[Cu(NH3)4]2+] Kf = [Cu2+][NH3]/[[Cu(NH3)4]2+] Kf = [[Cu(NH3)4]2+]/[Cu2+][NH3]4 Kf = [[Cu(NH3)4]2+]/[Cu2+][NH3] Kf = [[Cu(NH3)4]2+]
Question 19 5 pts Write the equilibrium constant expression for the reaction: 2 Hg(1) + O2(9) 2 2 HgO(s) K = (490) (H912 H90] (Hg)[02] OK = [H0]?[02] ка (H9012 (Hg)?[021
equilibrium help!! What is the equilibrium constant for the reaction CO(g) + 3 H2(g) - CH4(g) + H2O(g) if at 20 °C the equilibrium molar concentrations are [CO] -0.613, [H2] = 1.839, (CH4) = 0.387, and [H20) - 0.387? Format Β Ι Ο The reaction for the formation of the diamine-silver ion is as follows: Ag (aq) + 2NH3(aq) + Ag(NH3)2(aq) a. Write the equilibrium constant expression for this reaction. for the above b. An experiment was carried out to...
3. For the dissociation of gaseous PCls, the value of K, 2.00. The equilibrium reaction is PCMs) + Cl2(g) pressure of a sample of PCl, is kept constant at 5.00 atm during PCI(g) If the initial total the reaction, what would be the partial pressures of reactant and products when equilibrium is reached? - Write the K,equilibrium constant expression - Write expression of Dalton's law for the partial pressure for this reaction - Tabulate the changes of partial pressures -...
a. Using the Ksp value for Cu(OH)2 (1.6 x 10-19) and the overall formation constant for Cu(NH3)42+ (1.0 x 1013), calculate the value for the equilibrium constant for the following reaction: Cu(OH)2 (s) + 4NH3 (aq) ⇌ Cu(NH3)42+(aq) + 2OH -(aq) b. Use the value of the equilibrium constant you calculated in part a to calculate the solubility (in mol/L) of Cu(OH)2 in 5.0 M NH3. In 5.0 M NH3 the concentration of OH - is 0.0095 M.
4. Write an expression for the equilibrium constant for the formation of two moles of ammonia gas (NH3) from nitrogen and hydrogen in their standard states. N2(g) + 3H2() 52 NH,(8)