[Joel]

I have this reaction: 2H₂(g) + 2NO(g) --> N₂(g) + 2H₂O(g)

and the observed rate law is: Rate = k[NO]²[H₂ ]

Now, would a increase of the partial pressure of hydrogen gas affect the rate constant k and/or the reaction rate? And if, how can it be explained?

I've been trying to find some leads in my textbook, but no luck so far =/

[sdekivit]

ideal gas law. When partial pressure p rises, concentration rises and thus k would increase:

p = nRT/V

[mike]

ideal gas law. When partial pressure p rises, concentration rises and thus k would increase:

p = nRT/V

I would have thought that the rate would increase but the rate constant would stay the same

[Borek]

would a increase of the partial pressure of hydrogen gas affect the rate constant k and/or the reaction rate?

Rate constant - no. Reaction rate - yes.

Partial pressure and concentration are effectively the same thing.

[mike]

Temperature will affect the rate constant though.

[kkrizka]

The constant depends on the temperature only, so unless you change the temperature it stays the same. Now for the second part, try plugging in numbers.
What would the rate be if the partial pressure of N) is 1atm and of H2 is 3.5 atm? Now try doulbing H2, what is the new rate and how does it compare with the old one?

[Joel]

Thx guys, I think i know how it works now!