# Chemistry

posted by .

Consider the reaction: N2O4(g) <--> 2NO2(g)
delta H^o =58.576kJ; Keq =0.87 at 55degrees celsius
What is the effect of each of these changes upon the concentration of N2O4 at equilibrium?
a)increasing the temperature
b)increasing the volume
c) adding more NO2(g) to the system without changing pressure or temperature,
d) adding He gas to the container

• Chemistry -

This is Le Chatelier's Principle and you need to learn how to do these. They are simple but students often get confused. Most books give a very good definition but the problem is that most students don't follow it. My unorthodox definition is this. When a system in equilibrium is subjected to a stress the system will try to undo what we've done to it. That means if we add a reagent or heat it will shift so as to undo what we did.
Note that the reaction is endothermic; ie., we can write heat on the LEFT side. So if we increase T it will try to undo that. How can it do that? It can react more of the reactants to form more products. That's how it can use up the added heat. If we add N2O4 it will shift to the right in order to use up the added N2O4. With increasing pressure the system will shift to the side with the fewer moles of gas.

• Chemistry -

Thank you! :)

## Similar Questions

1. ### chemistry

Can you please check if I came up with the right answer for this please. A 4.30L container had 55.10 moles of N2O4 added to it. When equilibrium was established the concentration of N2O4 was found to be 1.69M.What is the Kc for the …
2. ### Chemistyr 152

Given the following data, what is the value of delta Gf (in kJ) for N2O4 (g) at 25C. N2O4(g)-----2NO2(g) Keq= 0.144 delta Gf: ?
3. ### chemistry

Consider the following equation: N2O4(g)+ 2NO2(g) Kc= 5.8 x 10^-3 If the initial concentration of N2O4(g)= 0.040 M and the initial concentration of NO2(g) is 0 M, what is the equilibrium of concentration of N2O4(g)?
4. ### chemistry

i already posted this question, but im still confused on it. Dinitrogentetraoxide partially decomposes according to the following equilibrium: N2O4 (g) -> 2NO2 (g) <- A 1.00-L flask is charged with 0.400 mol of N2O4. At equilibrium …
5. ### Chemistry

When heated, N2O4 dissociates as follows: N2O4 =2NO2 A flask initially contians .560 M N2O4. at this temperature, Kc is 4.00. what is the equilibrium concentration of NO2?
6. ### Chemistry

The equilibrium system N2O4(g) 2NO2(g) was established in a 1.00-liter vessel. Upon analysis, the following information was found: [NO2] = 0.500 M; [N2O4] = 0.0250 M. What is the value of Keq?
7. ### Chemistry

Dinitrogen tetroxide decomposes to nitrogen dioxide: N2O4 (g) ---> 2NO2 (g) Delta H rxn: 55.3 kJ At 298 K a reaction vessel initially containing .100 atm of N2O4. When equilibrium is reached, 58% of the N2O4 has decomposed to NO2. …
8. ### Chemistry!! Help

Consider the following equilibrium: N2O4 <=> 2NO2 You may assume that delta H and delta S do not vary with temperature. At what temperature will an equilibrium mixture of 1 atm total pressure contain twice as much NO2 as N2O4?
9. ### chemistry

Consider the equation: 2NO2(g) N2O4(g). Using ONLY the information given by the equation which of the following changes would increase the molar concentration at equilibrium of the product N2O4(g)?
10. ### CHEMISTRY

A chemist studying the equilibrium N2O4(g)<----->2NO2(g) controls the temperature so that keq ( equilibrium constant)= 0.028. At one equilibrium position, the concentration of N2O4 is 1.5 times greater than the concentration …

More Similar Questions