Wednesday
April 1, 2015

Homework Help: AP Chem

Posted by Bill on Sunday, January 8, 2012 at 6:29pm.

At a particular temperature, Kp = 0.25 for the following reaction.
N2O4(g) 2 NO2(g)

(a) A flask containing only N2O4 at an initial pressure of 5.3 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases.

(b) A flask containing only NO2 at an initial pressure of 7.0 atm is allowed to reach equilibrium. Calculate the equilibrium partial pressures of the gases.

Answer this Question

First Name:
School Subject:
Answer:

Related Questions

chem - A flask is charged with 1.596 atm of N2O4(g) and 1.008 atm of NO2(g) at ...
Chemistry - Dinitrogen tetroxide decomposes to nitrogen dioxide: N2O4 (g) --->...
CHM - Given the initial concentrations of 0.10 atm NO2 and 0.10 atm N2O4 in a 1....
chemistry - The half-life for the first-order decomposition of is 1.3*10^-5. ...
Chemistry - 92.01 grams of N2O4 (g) is placed in a container and allowed to ...
Chem 2 - The following system is at equilibrium with [N2O4] = 0.55 M and [NO2...
chemistry - A 1.00 mol sample of N2O4 (g) is placed in a 10.0 L vessel and ...
chemistry - Liquid Nitrogen tetroxide, N2O4(l), was used as a fuel in Apollo ...
Chemistry - Nitrogen dioxide, NO2, dimerizes easily to form dinitrogen tetroxide...
chemistry - The following system is at equilibrium with [N2O4] = 0.55 M and [NO2...

Members