help please The equilibrium constant Kcfor the reaction below is is 5.355x10-5 2nd attempt jal See...
The equilibrium constant K, for the reaction below is is 7.755x10 CD+E 1st attempt See Periodic Table Part 1 (1point) The initial composition of the reaction mixture is (C] ID]-[E]-1.1110x10 M What is the equilibrium concentration of C? Part 2 (1 point) What is the equilibrium concentration of D? Part 3 (1 point) Feedback See Hint What is the equilibrium concentration of E? O 1.978 x10M
I got the first one correct but not the last 2. The equilibrium constant K for the reaction below is is 7.755x105. CODE 4th attempt Part 1 (1 point) W See Periodic Table The initial composition of the reaction mixture is [C] = [D] – [E] = 1.7110x103 M. What is the equilibrium concentration of C? 0.00303 M Part 2 (1 point) What is the equilibrium concentration of D? 0.000386 M Part 3 (1 point) See Hint What is the...
07 Question (6 points) The equilibrium constant Ke for the reaction below is is 6.755x105 1st attempt Part 1 (2 points) The initial composition of the reaction mixture is [C] [D]- [E]- 1.7110x103 M What is the equilibrium concentration of C? Part 2 (2 points) What is the equilibrium concentration of D? Part 3 (2 points) What is the equilibrium concentration of E?
2nd attempt See Periodic Table See Hint Feedback Write a chemical equation for the hydrolysis reaction that explains why an aqueous solution of CH3NH3Cl is acidic. [Please include the states of matter with each chemical species. Remember, it is an equilibrium reaction.] xx. He (aq).
12 Question ( point) a See page 749 One millimole of Ni(NO3)2 dissolves in 260.0 mL of a solution that is 0.300 M in ammonia. The formation constant of Ni(NH3)62+is 5.5x108. 5th attempt Part1 (0.5 point) Feeback Feedback see Periodic Table See Hint What is the initial concentration of Ni(NO3)2 in the solution? 0.003846M Part 2 (0.5 point) Feedback What is the equilibrium concentration of Ni2 (aq) in the solution? x 10-0 M 7.00
23 Question (1 point) See page 330 2nd attempt See Periodic Table See Hint Feedback Balance the neutralization reaction of phosphoric acid with magnesium hydroxide. States of matter are not needed. х. Не X х) Mg(он), — н,о H2PO43 23/27 C TRY AGAIN VIEW SOLUTION 20 OF 27 QUESTIONS COMPLETED
Question (1 point) 2nd attempt Feedback It See Periodic Table O See Hint In a 8.00 M nitrous acid (HNO,) solution, calculate (H). Nitrous acid is a weak acid with K - 4,00 x 104 at 25°C. 1.789 x 10- M > 1st attempt
the equilibrium constant Kc for the reaction below is is 5.877×10-5 . c->d+e The initial composition of the reaction mixture is [C] = [D] = [E] = 1.995×10-3 M. What is the equilibrium concentration of C?
Iul See Periodic Table See Hint Calculate the equilibrium concentration of Ag (aq) in a solution that is initially 0.120 M AgNO, and 0.840 MNH3, and in which the following reaction takes place: Ag (aq) + 2NH, (aq) (NH)2(aq) (K - 1.70.10) M Ag One millimole of Ni(NO3)2 dissolves in 270.0 mL of a solution that is 0.500 M in ammonia The formation constant of Ni(NH3)2 is 5,5x10% 1st attempt Part 1 (1 point) i See Periodic Table See Hint...
There is a rather lengthy video animation about free energy located in the hint. 2nd attempt Part 1 (2 points)See HintSee Periodic Table Determine the value of ΔGº for a reaction at 25°C which has an equilibrium constant of 21.2 . kJ/mol Part 2 (3 points)See Hint Calculate ΔG for the reaction below at 25°C when 5.00 bar of A and 9.20 bar of B are present. ΔGº = +5.44 kJ/mol for this reaction. $$A(g) 2B(g) kJ/mol