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S
 3 years ago
N2O4(g)<>2NO2 , kp= 0.15
A gaseous mixture contains 0.600 ATM pressure of n2o4 is mixed with 0.75. ATM pressure of no2. Calculate the equillibrium pressures of each gas ???
S
 3 years ago
N2O4(g)<>2NO2 , kp= 0.15 A gaseous mixture contains 0.600 ATM pressure of n2o4 is mixed with 0.75. ATM pressure of no2. Calculate the equillibrium pressures of each gas ???

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.Sam.
 3 years ago
Best ResponseYou've already chosen the best response.3Do we need ICE table for this?

S
 3 years ago
Best ResponseYou've already chosen the best response.0I was actually confused how to make ice chart

abb0t
 3 years ago
Best ResponseYou've already chosen the best response.0I don't think yoiu need an ICE table for this.

.Sam.
 3 years ago
Best ResponseYou've already chosen the best response.3ok, ICE stands for Iinitial Cchange and Eequilibrium, for each reactant and products has these states, N2O4 <> 2NO2 I 0.600 0.75 C +x 2x E 0.6+x 0.752x  \[K_p=\frac{p(NO_2)^2}{p(N_2O_4)} \\ \\ 0.15=\frac{(0.752x)^2}{0.6+x} \\ \\ x=0.20162~~~and~~~0.585\]

abb0t
 3 years ago
Best ResponseYou've already chosen the best response.0I don't remember ICE tables at all. Lol i just remember they were long and tedious :p

S
 3 years ago
Best ResponseYou've already chosen the best response.0Also , how do I determine where is  x and where is + x ?

.Sam.
 3 years ago
Best ResponseYou've already chosen the best response.3Then use x=0.20162 on equilibriums, N2O4=0.6+0.20162=0.80162 N2O2= 0.752(0.20162)=0.34676

.Sam.
 3 years ago
Best ResponseYou've already chosen the best response.3N2O2 started at higher amount than N2O4, so it will be reduced

.Sam.
 3 years ago
Best ResponseYou've already chosen the best response.3thanks @abb0t tried my best :)

S
 3 years ago
Best ResponseYou've already chosen the best response.0Got it! Thank you for your help a lot !!
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