3. Calculate the molar concentration of Co+ at equilibrium when 0.12 moles Co3+ is mixed with 0.98 moles NHs in 100 mL total volume of solution. Kf Co(NH3).+ = 1.0 x 105 * Co3* + 6NH3 2 Co(NH3)6³* 3.9 x 10-3 M O 3.9 x 10-8 M O 3.0 x 10-11 M O 4.6 x 10- M

Express the equilibrium constant (K) for the chemical equations. (Note the physical states) A. CH3OH (g) ↔ CO (g) + 2 H2 (g) B. C3H8 (g) + 5 O2 (g) ↔ 3 CO 2 (g) + 4 H2O (g) C. SbCl5 (g) ↔ SbCl3 (g) + Cl2 (g)

For the reaction, 2NH3(g)--> <---3H2 (g)+ N2 (g) the equillibrium concentrations were found to be [NH3 ]=0.250 M, [H2 ]=0.540 M, and [N2 ]= 0.750 M. What is the equilibrium constant for this reaction? Kc=?

Consider the cobalt-chloride ion equilibrium shown. Co(H,O)%*(aq)+4Cl (aq) = CoCl (aq) +6H,O) 4 blue pink Determine how the equilibrium will be affected by the addition of each reagent. Adding HCI will shift the equilibrium Adding water will shift the equilibrium -

The reaction below is at equilibrium. Before the reaction began, the concentrations of the reactants were 0.060 M of SO2 and 0.050 M O2.  After the equilibrium is reached, the concentration of SO3 is 0.040 M.  What is the value of K? 2 SO2(g) + O2(g)  <===>  2 SO3(g) 130 2.7 0.0075 8.9 0.38

11. The Kf for [AIF6]³- is 7.0 x 101⁹ and the corresponding equilibrium is shown below. Calculate the concentration of Al³+ ions in a solution that is initially 0.83 M in [AlF6]³-. Al³+ (aq) + 6 F-(aq) [AIF6]³(aq)

Consider the general reaction below. 2A(g) + B₂(g) = 2AB(g) K = 6.4 x 10-6 @ 298 K The reaction was initiated by combining 0.70 mol A and 0.90 mol B2 in a 2.0 L container. Calculate the equilibrium concentrations of the components. What is the equilibrium concentration of AB? 10[? ] [AB] = [?] x 10¹ M

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Heating solid sodium bicarbonate in a closed vessel established this equilibrium: 2NaHCO3(s) → Na₂CO3(s) + H₂O(g) + CO₂ (g) What would happen to the equilibrium position in the following situations (the temperature remains constant)? Part 1 of 3 Some of the solid NaHCO3 was removed from the system. O shift equilibrium to the right O have no effect O shift equilibrium to the left X

At equilibrium, the concentrations in this system were found to be [N,] = [0,] = 0.200 M and [NO] = 0.500 M. %3D %3D %3D N,(g) + 0,(g) =2 NO(g) If more NO is added, bringing its concentration to 0.800 M, what will the final concentration of NO be after equilibrium is re-established? [NOJfinal %3D TOOLS x10 about us privacy policy terms of, use contact us help careers 4:40 A 4/25/20 End Insert 888 F12 Home Pく F7 F9 F10 F11 F4 F5 F6 F8