At a certain temperature the reaction CO_2(g) + H_2(g) CO(g) + H_2O(g) has K_c =

Question

At a certain temperature the reaction CO_2(g) + H_2(g) CO(g) + H_2O(g) has K_c = 2.50. If 2.00 mol. of carbon dioxide and 1.50 mol. of hydrogen are placed in a 5.00-L vessel and equilibrium is established, what will be the concentration of carbon monoxide? Which of the following is the correct unit for a second order rate constant? Ms^-1 s^-1 M^-2s^-1 M^-1s^-1 Ms A container was charged with hydrogen. nitrogen, and ammonia gases at 120 degree C and the system was allowed to reach equilibrium. What will happen if the volume of the container is increased at constant temperature? 3H_2 (g) + N_2(g) 2NH_3(g) Hydrogen's and nitrogen will be produced at the expense of ammonia. The equilibrium constant will increase. More ammonia will be produced at the expense of hydrogen and nitrogen. The equilibrium constant will decrease. There will be no effect. Which is the correct equilibrium constant expression for the following reaction? FeO(s) + H_2(g) Fe(s) + H_2O(g) K_c = [Fe_2O_3][H_2]/[Fe][H_2O] K_c = [Fe][H_2O]/[Fe_2O_3] K_c = [Fe][H_2O]/[Fe_2O_3][H_2] K_c = [H_2O]/[H_2] K_c = [H_2]/[H_2O] For the reaction H_2(g) + Br_2(g) 2HBr(g), K_c = 81.4 at 385 degree C. If [H_2] = [Br_2] = [HBr] = 2.4 times 10^-4 M at 385 degree C, which one of the following is correct? [HBr] increases as the system approaches equilibrium. The system is at equilibrium. (HBr J and [Br_2] increase as the system approaches equilibrium. (H_2) and [HBr] decrease as the system moves toward equilibrium. (H_2) and [Br_2] increase as the system approaches equilibrium.

Explanation / Answer

11. CO2 + H2 ----> CO + H2O

Kc = 2.50

moles of CO2 = 2.00

Volume of vessel = 5.00 L

[CO2] = moles/volume = 2.00/5.00 = 0.40 M

moles of H2 = 1.50

Volume of vessel = 5.00 L

[H2] = moles/volume = 1.50/5.00 = 0.30 M

ICE table:

_________________________[CO2]________________[H2]______________[CO]_____________[H2O]

Initial____________________0.40_________________0.30_______________0_________________0

Equilibrium_____________0.40-x________________0.30-x_______________x__________________x

Kc = [CO][H2O]/([CO2][H2])

2.50 = x.x/[(0.40-x)(0.30-x)]

x2 = 2.50 [(0.40-x)(0.30-x)]

x2 = 2.50 (0.12-0.70x+x2)

x2 = (0.30-1.75x+2.50x2)

1.50x2-1.75x+0.30 = 0

After solving this quadratic equation, x = 0.21

At equilibrium, [CO] = x = 0.21 M

12. The units for the second order rate constant is M-1s-1. Correct answer is d.

13. The volume of container is increased, this means that the pressure of the container decreased. The total number of moles of gases on reactants side is 4 and on products side is 2. The reaction will shift towards the direction of more moles of gases. So, reaction shifts towards left. More hydrogen and nitrogen will be formed. Answer is a.

14. The equilibrium constant is ratio of product of concentration of products and product of concentration of reactants.

So, Kc = [Fe][H2O]/[FeO]H2]

Correct option is c.

15. H2 + Br2 ----> 2HBr

Kc = 81.4

ICE table:

__________________[H2]________________[Br2]____________________[HBr]

Initial____________2.4*10-4________________2.4*10-4________________2.4*10-4

Change___________-x______________________-x___________________+2x

Equilibrium_______2.4*10-4-x_____________2.4*10-4-x______________2.4*10-4+2x

So, this shows that H2 and Br2 are consumed and HBr is formed till it reaches eqilibrium.

Correct option is a.

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