6. At a certain temperature, K. = 4.0 for the following reaction. [6] 2HF) → H2) A 1.0 L reaction vessel contained 0.045 mol of F2(9) at equilibrium. What was the initial amount of HF in the reaction vessel? (Hint: use two variables -seen in class) %3D + F26)

Picture 1 is A) And  Picture 2 is B)

The equilibrium constant, K., for the following reaction is 1.29×102 at 600 K. CoC,(g) CO(g) + Cl(g) Calculate the equilibrium concentrations of reactant and products when 0.270 moles of COCI,(g) are introduced into a 1.00 L vessel at 600 K. [COC1] = M %3D [CO] M [Cl2] M

Question 41 of 44 Consider the equilibrium system described by the chemical reaction below, which has a value of Kc equal to 7.1 x 10 at a certain temperature. If a solid sample of CaCrO4 dissolves in solution, what will the equilibrium concentration of Ca in the solution be? CaCrO.(s)= Ca (aq) + CrO (aq) NEXT Based on the given values, set up ICE table in order to determine the unknown. CaCrO-(s) Ca-(aq) CrO. (aq) Initial (M) Change (M) +2x +2x Equilibrium (M) 7.1 x 10-2x +2x +2x RESET 7.1 x 10 +2x -2x 7.1 x 10 +* 7.1 x 10-r 7.1x 10+ 2x 7.1x 10-2x

For the reaction 8 H, S(g) = 8 H, (g) + S3 (g) 8. the equilibrium concentrations were found to be [H, S] = 0.250 M, [H,] = 0.560 M, and [S] = 0.750 M. What is the equilibrium constant for this reaction? Ko

3b) please see attached

Give typed solution

The following reaction at a certain temperature has an equilibrium constant value of 0.016.  2 HI (g) ⥂ H2 (g) + I2 (g) For each of the following compositions, decide whether the reaction mixture is at equilibrium. a.) [ HI ] = 0.076 M; [ H2 ] = 0.012 M; [ I2 ] = 0.012 M b.) [ HI ] = 0.140 M; [ H2 ] = 0.031 M; [ I2 ] = 0.010 M

for the reaction 2IBr -- I2(g) + Br2, Kc=.026. Consider that the starting composition is .010 mol IBr in a 2-L vessel at 100 C. Find the moles of all species present at equilibrium. (Hint: Divide moles by volume to get molarities.

At equilibrium, the concentrations in this system were found to be [N,] = [0,] = 0.100 M and [NO] = 0.400 M. N, (g) + 0,(g) = 2 NO(g) If more NO is added, bringing its concentration to 0.700 M, what will the final concentration of NO be after equilibrium is re-established? [NO]final = M