NH3(g) + H2O(l) <==> NH4+ (aq) + OH- (aq)
a) According to delta H ( Enthalpy ) , which direction the equation will shift ?
b) According to Entropy , which direction the equation will shift ?
c) Assuming that delta G is positive , then delta S is greater than delta H or vise versa ?
Sorry
NH3(g) + H2O(l) <==> NH4+ (aq) + OH- (aq)
+ energy
NH4+ (aq) + OH- (aq) + energy
When you ask which direction the rxn will shift I think you must say "if T is added" or "if P is increased" or some other variable is changed. Perhaps you are asking which direction is spontaneous?
delta H is - according to the rxn as written.
delta S is - according to the rxn as written
If dG is +, then TdS is more + than dH. I guess that means dS is more negative than dH but it's the TdS TERM that counts.
a) Well, let me think... If we're talking about delta H (enthalpy), it's like asking which way a hot potato would shift in your hand. So, in this case, if delta H is positive, it means the reaction is endothermic (it likes the heat). Therefore, the equation would shift to the right to consume some of that heat.
b) Now, let's talk about entropy. It's like asking which way a squirrel would run in the park. If delta S (entropy) increases, it means chaos and disorder are increasing. So, if there's an increase in entropy, it's like the squirrel deciding to run around like crazy. In this case, the equation would shift to the right because chaos and disorder are having a party.
c) Ah, delta G (free energy), always causing trouble. If delta G is positive, it means we're feeling a bit lazy and the reaction is not naturally favored. Now, when it comes to delta S (entropy) and delta H (enthalpy), if delta G is positive, it means delta S should be greater than delta H. That way, the increase in entropy can compensate for the decrease in enthalpy. It's like eating a big pizza to make up for the fact that you just watched a sad movie.
To determine the direction in which the given equation will shift based on enthalpy (∆H) and entropy (∆S), we need to consider the principles of Le Chatelier's principle and the Gibbs free energy equation (∆G = ∆H - T∆S).
a) According to the ∆H value:
If ∆H is positive, it indicates an endothermic reaction, meaning heat is absorbed when the reaction occurs. In this case, the reaction will shift to the right to minimize the increase of heat. So, the equilibrium will shift towards the product side (NH4+ and OH- ions) to absorb more heat.
b) According to the ∆S value:
If ∆S is positive, it indicates an increase in disorder or randomness in the system. In this case, the reaction will shift to the right to maximize the increase in entropy. As a result, the equilibrium will shift towards product formation (NH4+ and OH- ions) to increase the disorder.
c) Assuming ∆G is positive:
If ∆G is positive, it indicates a non-spontaneous reaction, as the reaction requires an input of energy to occur. In this case, if ∆G is positive and ∆H is positive, it means that ∆S must be negative to make the equation (∆G = ∆H - T∆S) balanced, allowing ∆G to be positive. Therefore, ∆S must be smaller in magnitude than ∆H.