Achiever Gen Chem help.

[kponenation]

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Hi,

I don't quite understand this problems and I was wondering if someone could explain it to me. Thanks in advance.

2 CO2 What is the equilibrium constant, K, at 400K if 3.00 moles of CO2(g) introduced into a 2 liter container are 20.0% dissociated at equilibrium? 2 CO2(g) « 2CO(g) + O2(g)

 

[Sublimation]

Hi,

I don't quite understand this problems and I was wondering if someone could explain it to me. Thanks in advance.

2 CO2 What is the equilibrium constant, K, at 400K if 3.00 moles of CO2(g) introduced into a 2 liter container are 20.0% dissociated at equilibrium? 2 CO2(g) « 2CO(g) + O2(g)

first u need to figure out how many moles of each is made. Now do it this way take 20% of 3 and 1.5 (these are the theoretical moles that we expect to produce). so just solve 3*.2=moles of CO. 1.5*.2=moles ofO2. now since its 20%dissociation 80%didnt form product. So .8*3=moles of reactant.

so now we have 2.4CO2 and .6CO and .2O2

use P=nrt/v to get total pressure then multiply that by the mole fraction of each and then u will have the partial pressures and then set up the equation for K.

Im sorry but iam horrible at explaining things

 

[kponenation]

Thank you!