A flask is charged with 1.500 atm of N2O4(g) and 0.94 atm NO2(g) at 25°C. The...

Question

Question

A flask is charged with 1.500 atm of N2O4(g) and 0.94 atm NO2(g) at 25°C. The equilibrium reaction is given in the equation below.

N2O4(g) 2NO2(g)

After equilibrium is reached, the partial pressure of NO2 is 0.512 atm.

(a) What is the equilibrium partial pressure of N2O4? ______ atm

(b) Calculate the value of Kp for the reaction. ______

(c) Is there sufficient information to calculate Kcfor the reaction?

-Yes, because the temperature is specified.

-No, because the value of Kc can be determined experimentally only.

-Yes, because the partial pressures of all the reactants and products are specified.

(d) If Kc can be calculated, find the value of Kc. ____ Otherwise, enter 0.

Answer 1

Answer #1

Answer 2

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