Hydrogen Constant
Find Equilibrium constant for a gas reaction?
I have tried for several hours to solve this problem. The answer is supposed to be 1.154. Can someone tell me how to find this?
Just plugging in the numbers for the normal equilibrium constant equation doesn’t work, and I’m not sure what else to do.
2.017 bar of white phosphorous vapor, P4(g), are combined with 6.289 bar of Hydrogen, H2(g), in a 10-L reactor to produce phosphine, PH3(g). The equilibrium reaction is given by:
½ P4(g) + 3 H2(g) ↔ 2 PH3(g)
If 2.941 bar of PH3(g) are produced at equilibrium what is the value of the equilibrium constant? Assume ideal gas behavior and don’t forget the stoichiometry.
Thanks!
i tried the question i found out kp very well but not kc as per asked
i think that if they mentioned temp, it was a plum question to find out
else
here u can try finding the equlibrium moles of each of the reactants and products in terms of v,t,r using p=nrt/v
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