Question

Which of the following would increase the rate of this chemical reaction N2(g) + 3H2(g) arrow 2NH3(g)
Reduce the temperature
Decrease the volume
Introduce a catalyst

I only

I and II

II and III

III only

Answer 1

Is this what you meant? \(N_{2}(g)+3H_{2}(g)\rightarrow2NH_{3}(g)\)

Answer 2

To be able to understand the process, you would need the complete chemical reaction:

\(3H_2+N_2 \leftrightarrow 3NH_3 + 92~kJ~mol^{-1}\)

Apply Le Chatelier's principle:
"If a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change."
( http://www.chemguide.co.uk/physical/equilibria/lechatelier.html)

Equilibrium moves to counteract:
I. reduce temperature - means reaction is likely to generate more heat to counteract the decreased temperature
II decrease volume - means equilibrium is likely to move towards the side that has a bigger volume to counteract the decrease the volume.
III. Introduce a catalyst - unless mentioned otherwise (as a negative catalyst), catalysts increase the rate of the forward reaction.

Answer 3

HEy

Answer 4

2 increases the likelyhood that the molecules or atoms will hit because they are in a more confined space, and 3 lowers the activation energy required for the reaction to take place. So between the 2 of them it will increase the rate of the reaction.

Answer 5

II and III. is correct

Lowering temperature will slow down the reaction rate.
Decreasing volume, increases pressure so more frequent collisions.
Catalysts lowers activation energy, so reaction will occur faster.

Answer 6

Hey thanks.
But the medal goes to mathmate for answering me first (:

Answer 7

@NvidiaIntely
Thank you!