Ok so I have a couple question I need help answered QUESTION 1 - in lab you and

Question

Ok so I have a couple question I need help answered

QUESTION 1 - in lab you and your partner study the reaction of N2 + 2O2 in equilibrium with N2O4. Kc = 27.5. After 15 seconds, your lab partner reports the following concentrations

[N2] = 0.004 M

[O2] = 0.027 M

[N2O4] = 0.0012 M

Determine the value of Q (the reaction quotient) at 15 seconds...

ANSWER: I got Qc = [products]/[reactants] = (.0012)/(.004)(.0027)^2 = 4.11e-12 which Kc< Kq

QUESTION 2- using the Q you calculated in problem 1, is this reaction at equilibirum?

ANSWER: I got no due to Kc<Kq, reaction is only at equilibrium when Kc=Kq

QUESTION 3 - after 30 seconds, your lab partner records the following equilibrium concentrations.

[N2] = 0.137 M

[O2] = 0.462 M

Given that the Kc = 27.5, determine the equilibrium concentration of N2O4

ANSWER: I don't know what to do for this problem

QUESTION 4 - Your partner now increases the temperature of the reaction.  Assuming that the dHrxn = 2.9 kJ/mol, which way will the reaction proceed?

A. to the reactants

b. no change

c. to the products

I don't know the answer to this one as well

PLEASE HELP!!

Explanation / Answer

first and second parts are correct

third part is Kc = [N2O4]/[NO2][O2]^2

[N2O4] = 27.5*0.137*(0.462)^2 = 0.804M

the fourth part is as temperature is increased the system wil try to go in the direction where some heat is released as reaction in foraward direction ha positive enthalpy = 2.9KJ/mol it will g0 in foraward direction so more products will be formed

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