Equilibrium

which reaction is favored when we let the syringe cool down to room temperature again?

2 NO2(g) -> N2O4(g)

what color did you predict for the syringe inside the liquid nitrogen tank? have a look at the graphs on the screen to answer the question

transparent

anything else that might favor the forward reaction

yes, you should constantly remove NH3 from the system

what happens after pulling the plunger back up?

The color becomes pale immediately and then darker again

what happens immediately after you press the plunger? Explore to retry the experiment

The concentration of both gases increases

looking at the screen, how do the concentrations of reactants and products change over time at equilibrium?

The concentrations of NO2 and N2O4 stay the same

now I think about the opposite case to our experiment, and exothermic reaction. Chatelier's principle can help here again. How do you think the equilibrium is affected by an increase in temperature?

The equilibrium is shifted to the left

what happens when you put the syringe into boiling water? Cook explore to try the experiment and generate new data on the screen if you wish

most of the N2O4 is converted to NO2

what happens when you put the syringe into liquid nitrogen? Explore to retry the experiment

most of the NO2 is converted to N2O4

which statement below is true of Kc's value at -196C? click on view image to use the cheat sheet

Kc << 1

what is the value of Kc in boiling water?

Kc >> 1

what happens when we let the mixture heat up to room temperature again

N2O4 is converted back to NO2

at the beginning of the experiment there are no NH3 in the system so it's concentration is zero. If you assume that the value of Kc in our reaction is 9.6, which of the following statements is correct.

Q<Kc

equilibrium

Q=Kc

directly after increasing the pressure, what is the relationship between Q and Kc?

Q>Kc

The Haber process as exothermic. Recalling from what we have learned in the first mission: in which direction will the equilibrium be shifted by hearing the reaction chamber with the Bunsen burner

To the left

for our equilibrium, Kc was calculated to be 4.6×10^-3 how did the current conditions. What does this imply for the concentrations of NO2 and N2O4? if you click on view image you can have a look at the cheat sheet containing the relevant equations.

[N2O4]>[NO2]

why does the color get paler again after the pressure increases?

all the answers are correct

which statement about a chemical equilibrium is correct?

forward and reverse reactions happen at equal rates

which of the following reactions is not reversible?

frying an egg

despite these improvements my yields are still low. Do you have any new insights about how I could improve the production of ammonia? How can I increase the yields?

increase the pressure, keep the temperature as low as possible

how does a catalyst influence chemical chemical equilibrium?

it speeds up the rate of the forward and back reactions

our system has to operate at high temperatures. according to Le Chatelier, how could we nevertheless shift the equilibrium towards the product side? Have a look at balanced reaction again in the cheat sheet

it speeds up the rate of the forward and back reactions

what happens to Kc when the pressure is increased?

it stays the same