# Chemistry: Equilibrium

What is the significance of a very large Kp value on the equilibrium concentration of H2 in the reaction: 2H2(g) + O2(g) ->2H2O(g)?
<-

There is very little H2 at equilibrium.

The amount of H2 is always equal to the amount of O2 at equilibrium.

The amount of H2 does not depend on the value of Kp.

There is a significant amount of H2 at equilibrium.

1. 👍
2. 👎
3. 👁
1. So Kp = p(H2O)^2/p(H2)^2*p(O2)
A large Kp means high p for H2O and low p for H2 and O2. If you have low p for H2 there isn't much there.

1. 👍
2. 👎
2. Oh Robert, you amaze me with your words

1. 👍
2. 👎
3. There is very little H2 at equilibrium.

1. 👍
2. 👎

## Similar Questions

1. ### Chemistry

Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of SO2(g). 2SO2(g)+O2(g)=2SO3(g) Kc=1.7*10^8 [SO3]aq=0.0034 M [O2]aq=0.0018

2. ### Chemistry

At equilibrium, the concentrations in this system were found to be [N2] = [O2] = 0.100 M and [NO] = 0.500 M. N2(g) + O2(g) 2NO(g) If more NO is added, bringing its concentration to 0.800 M, what will the final concentration of NO

3. ### Chemistry

SO2(g) + NO2(g) SO3(g) + NO (g) At a given temperature, analysis of an equilibrium mixture found [SO2] = 4.00 M, [NO2] = 0.500 M, [SO3] = 3.00 M, and [NO] = 2.00 M. (a) What is the new equilibrium concentration of NO when 1.50

4. ### chemistry

NaCl(s) + H2O(l) Na(aq) + Cl(aq) If you added chloride ions to the above equilibrium, what would happen to the concentration of the products, and the concentration of the reactants? I know the equilibrium would shift to the left,

1. ### chemistry

Concerning the following reaction at equilibrium: 3Fe(s) + 4H2O(g) Fe3O4(s) + 4H2(g), increasing the concentration of the Fe(s) would: Answer A. Shift the equilibrium to the right B. Shift the equilibrium to the left C. No change

2. ### chemistry

The question below, i was wondering if it decrease because the N2 is on the right and so to add to left it would be too much so it gets rid of it by decreases and doing to the right? because the left side is (+) endothermic? sorry

3. ### Chemistry

EQUILIBRIUM: Given the equation 2 PbS(s) + 3 O2(g) 2 PbO(s) + 2 SO2(g) What direction will the reaction proceed if additional SO2 was added to the system at equilibrium? Forward Reverse Nothing Happens Difficult to determine You

4. ### Chemistry

A sample of ammonia gas was allowed to come to equilibrium at 400 K. 2NH3(g) --> N2(g) + 3H2(g) At equilibrium, it was found that the concentration of H2 was 0.0584 M, the concentration of N2 was 0.0195 M, and the concentration of

1. ### Chemistry

For the reaction: 2NO(g) + H2(g) N2O(g) + H2O(g) + energy Write the equilibrium constant expression for the reaction. I wrote: [N2O][H2O] / [NO]2 [H2] This reaction takes place at 25°C. At this temperature the concentration of NO

2. ### Chemistry

C6H12O6 (aq) = 602 (g) - 6CO2 (g) = 6H20 (l) H -2837 A)Exo or endothermic? B)write an expression for the equilibrium constant C)Give the value of the equilibrium constant is very large, would this reaction be fast or slow?

3. ### Chemistry

For the reaction I2 + Br2 2IBr Kc=280 at 150C . Suppose that 0.500 mol IBr in a 1.00-L flask is allowed to reach equilibrium at 150C. What is the equilibrium concentration of IBr What is the equilibrium concentration of I2 What is

4. ### chemistry

what is the equilibrium concentration of acetate ion if the equilibrium concentration of acetic acid is .40 M, the pH is 3.85, and Ka is 1.8E-05?