Question

For the reaction below, describe the temperature and pressure conditions that would produce the highest yield for the forward reaction. Explain your answer in terms of Le Châtelier’s principle.

N2 (g) + 3 H2 (g) Two arrows stacked on top of each other. The top arrow points to the right. The bottom arrow points to the left. 2 NH3 (g) deltaH = -92 kJ/mol



Can anyone please guide me through this question and help me? @iPwnBunnies

Answer 1

@Compassionate

Answer 2

@nincompoop @zepdrix

Answer 3

@abb0t

Answer 4

can u plz help? @Jesstho.-.

Answer 5

i don't know this o-o

Answer 6

can u plz tag anyone that does?

Answer 7

Since the reaction is exothermic as delta H is -ve so temperature condition should be low whereas the pressure would be high as increasing the pressure shifts the direction of reaction towards that side where no. Of moles are less and as you can see that in forward reaction which is of 2NH3 no.of moles are 2 compared to backward reaction where no, of moles are 4

Answer 8

asalamualaikum sister, is that all I have to write ? is that the answer to the question? @asra_saleem

Answer 9

Yeah but in terms of Le Chateliers principle for temp u have to explain this that as delta H is negative the reaction is exothermic so equilibrium will shift towards forward reaction and for pressure I have already written above

Answer 10

so i just add this to it?

Answer 11

Yeah