Question

A flask is charged with 1.500 atm N2O4(g) and 1.00 atm NO2(g) at 25 °C and...

A flask is charged with 1.500 atm N2O4(g) and 1.00 atm NO2(g) at 25 °C and the following equilibrium is achieved: N2O4(g)<-------> 2NO2(g)

After equilibrium is reached, the partial pressure of NO2 is 0.512 atm. What is the equilibrium partial pressure of N2O4?

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Homework Answers

Answer #1

Temperature does not have influence on moles

Consider partial pressures as moles. No. moles is proportional to pressure or volume.

NO2 used = 1 - 0.512 = 0.488 atm

extra N2O4 = 1/2 x 0.488atm = 0.244atm
partial prressure of N2O4 = 1.5 + 0.244 = 1.744atm

ICE table can be written as follows to better understand

Answer: The equilibrium partial pressure of N2O4 = 1.744atm

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