Week 9 Chem 14A Learning Session Number 8 & 1
Posted: Sat Dec 09, 2017 1:10 pm
In number 8, it says, will the equilibrium constant K increase, decrease, or remain constant after the following changes to the exothermic reaction 4A(g) + 3B(g) ⇌ 2C(g)?
When the stoichiometric coefficients are doubled, it says increase or decrease, but I thought that it would definitely decrease? Why could it increase or decrease? Wouldn't it decrease no matter the equilibrium concentrations? Also, if the temperature is doubled, does the K decrease because the equilibrium shifts left because it's exothermic? Why does this change the actual K?
Also, in number 1, since it said X was the equilibrium concentration for SO2, I thought that meant that 2x was equal to x, but then it said O2 also had a concentration of 2x, which doesn't really make sense to me. Can someone explain how to solve?
Thanks!
When the stoichiometric coefficients are doubled, it says increase or decrease, but I thought that it would definitely decrease? Why could it increase or decrease? Wouldn't it decrease no matter the equilibrium concentrations? Also, if the temperature is doubled, does the K decrease because the equilibrium shifts left because it's exothermic? Why does this change the actual K?
Also, in number 1, since it said X was the equilibrium concentration for SO2, I thought that meant that 2x was equal to x, but then it said O2 also had a concentration of 2x, which doesn't really make sense to me. Can someone explain how to solve?
Thanks!