Write the equilibrium-constant expressions and obtain numerical values for each constant in a. the basic dissociation of hydroxylamine, HONH2 (Ka = 1.10 x 10-6).   Expression:        Numerical Value:   b. the acidic dissociation of hypochlorous acid, HClO (Ka = 3.0 x 10-8).   Expression:        Numerical Value:

Consider the system 4NH3(g)+3O2(g)2N2(g)+6H2O(l)H=1530.4kJ (a) How will the amount of ammonia at equilibrium be affected by 1. removing O2(g)? 2. adding N2(g)? 3. adding water? 4. expanding the container at constant pressure? 5. increasing the temperature? (b) Which of the above factors will increase the value of K? Which will decrease it?

2. Write the dissociation equation and equilibrium constant expression for the dissociation of the following weak bases a. Methylamine, CH3NH2, Kb = 4.4 x 104 b. Aniline, C6H5NH2 Kb = 4.2 x 10-10

1

Given a solution of acetic acid, with equilibrium net ionic equation (so only showing the ions in the reaction and not the spectator ions): CH3COOH (aq) + H20 () CH3COO (aq) + H3O* (aq) Have 4 beakers with acetic acid. Each beaker gets one of the following four things added to it. Match each thing with how the equilibrium responds when the thing is added. Prompts Submitted Answers sodium acetate Choose a match calcium acetate nothing sodium chloride shifts left to make more reactants acetic acid shifts right then left then right then left... shifts right to make more products

Part A Consider the reaction: N2(9) +3 H2 (g) =2 NH3(g) Complete the table. Assume that all partial pressures are equilibrium values and in bar. Complete the first row. T(K) PN, PH, PNH, K NV ΑΣφ 350 0.121 0.105 0.565 415 0.108 0.134 13.2 515 0.130 0.138 0.0512 K = Submit Request Answer Part B Complete the second row. Hνα ΑΣφ ? bar PH, = Submit Request Answer Part C Complete the third row. να ΑΣφ ? bar PNH, = Submit Request Answer

Determine the Ka for a weak acid by constructing an ICE table and using this information to construct and solve the equilibrium constant expression. Complete Parts 1-2 before submitting your answer. 2 NEXT > 0.030 moles of a weak acid, HA, was dissolved in 2.0 L of water to form a solution. At equilibrium, the concentration of HA was found to be 0.013 M. Fill in the ICE table with the appropriate value for each involved species to determine the unknown concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) HA(aq) H₂O(I) = HO(a) A(aq)

What is the value of the equilibrium constant (K) for the following neutralization reaction:   ?3?++??−⟶2?2?H3O++OH−⟶2H2O Remember: if you want to express an answer in scientific notation, use the letter "E". For example "4.32 x 104" should be entered as "4.32E4". Hint: To answer this question, you may need to use the value of Kw stated in the lab manual.

Use the References to access important values if needed for this question. In an aqueous solution of a weak acid, HA, the assumption is often made that [HA]equilibrium = [HA]nitial: This approximation is reasonable if the initial concentration of the acid is sufficiently large compared to Ka. What multiple of K, must the initial concentration of a weak acid exceed, for the initial concentration and the equilibrium concentration to be within 9.98 percent of each other?

Could I have detailed work on how to solve this equilibrium problem