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

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

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

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

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

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

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