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Predict the direction in which the equilibrium will shift...?
Consider the following reaction:
C(s) + H20(g)-->CO(s) +H2(g) Kp-9.7x10^-17 at 290degreesK triangleH>0
Will the equilibrium shift left, right, or not at all for each of the following?
a) addition of H2O(g)
b) increase in reactor volume
c)addition of CO(g)
d)removal ofC(s)
e)increase in temperature
This question is on a practice test and I'm study for an upcoming test. Please only answer if you know your chem because I dont want to study wrong info. A short explanation would be nice. Thanks in advance
2 Answers
- 5 years agoFavorite Answer
C(s) + H20(g)-->CO(s) +H2(g)
Kp= 9.7x10^-17 at 290K
🔺H > 0
a.) if you add anything to a reaction it shifts AWAY because the reaction is able to produce more of the opposite side of the reaction. So if H20 is a reactant, then it shifts RIGHT
b.) Sorry, i dont know this one.
c.) Again, if you add anything to a reaction it shifts AWAY because the reaction is trying to distrivute what was just added. So if CO is a reactant, then it shifts LEFT
d.) Right, so this one is like the opposite of a and c. When you remove anything from a reaction, it shifts back TORWARD it because the reaction attempts to replace what was taken out. So if you are removing C, a recatant, it will shift LEFT.
e.) Okay so the most important thing in this question is that the "triangle H" is greater than 0. Triangle H means change in heat. if the change in heat is positive, that means the reaction is endothermic, it loses heat. So heat is a reactant. So acoarding to le chantleirs (i probably spelt that wrong) principle, you the reaction shifts AWAY from the stress (heat). So it shifts RIGHT.
Hope this is helpful :) Good luck with Chem (I'm sure we will all need it!)
