Question
For the system CaO(s) + CO2(g) = CaCO3(s), I added 1.00 mol of CaO(s) to 1.00L of 0.500M CO2(g) at 200 oC. At equilibrium the [CO2] = 0.150M. What is the value of Kp for this reaction?
Kp would = CaCO3/(CaO)(CO2)
I do not know what to do with the 0.500M and 1.00mol.
Kp would = CaCO3/(CaO)(CO2)
I do not know what to do with the 0.500M and 1.00mol.
Answers
First you need to work on the Kp expression. SOLIDS aren't used (pure liquids aren't either) so the expression is 1/pCO2 = Kp.
The problem tells you that AT EQUILIBRIUM [CO2] = 0.150M.
I would calculate Kc from Kc = 1/([CO2]
then convert to Kp by Kp = Kc(RT)<sup>Dn</sup>
The problem tells you that AT EQUILIBRIUM [CO2] = 0.150M.
I would calculate Kc from Kc = 1/([CO2]
then convert to Kp by Kp = Kc(RT)<sup>Dn</sup>
So I did 1/0.150 and got 6.66 so now I use this with RT. I am not sure what R is?
R is 0.08206