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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 ???
 11 months ago
 11 months 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 ???
 11 months ago
 11 months ago

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

SBest ResponseYou've already chosen the best response.0
I was actually confused how to make ice chart
 11 months ago

abb0tBest ResponseYou've already chosen the best response.0
I don't think yoiu need an ICE table for this.
 11 months ago

.Sam.Best ResponseYou've already chosen the best response.3
ok, 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  \[K_p=\frac{p(NO_2)^2}{p(N_2O_4)} \\ \\ 0.15=\frac{(0.752x)^2}{0.6+x} \\ \\ x=0.20162~~~and~~~0.585\]
 11 months ago

abb0tBest ResponseYou've already chosen the best response.0
I don't remember ICE tables at all. Lol i just remember they were long and tedious :p
 11 months ago

SBest ResponseYou've already chosen the best response.0
Also , how do I determine where is  x and where is + x ?
 11 months ago

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

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

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

SBest ResponseYou've already chosen the best response.0
Got it! Thank you for your help a lot !!
 11 months ago
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