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Chemistry Forums for Students => High School Chemistry Forum => Topic started by: cerez05 on January 05, 2005, 10:13:53 PM

Title: Equilibrium
Post by: cerez05 on January 05, 2005, 10:13:53 PM

Does increasing the temperature of the reversible reaction, N2 (g), + 3 H2(g) = 2NH3(g), shift the reaction to the left?  Please Explain.

In attempting to answer this question, I became confused with the concept of the shifting equilibrium.  My first instinct was that it shifts Right but i am not sure about this.

Title: Re:Equilibrium
Post by: Mitch on January 05, 2005, 10:27:52 PM

Are you sure N2 is aqueous?  ;)

Title: Re:Equilibrium
Post by: cerez05 on January 05, 2005, 10:48:23 PM

My mistake, I modified the question.

Title: Re:Equilibrium
Post by: AWK on January 06, 2005, 01:52:04 AM

Still traction is incorrect - NH2(g)

Title: Re:Equilibrium
Post by: cerez05 on January 06, 2005, 06:59:09 AM

gosh u know what i mean....

Title: Re:Equilibrium
Post by: AWK on January 06, 2005, 07:14:24 AM

Formation of ammonia is an exothermic reaction (-46 KJ/mol), hence heating shift the reaction to the left.

Title: Re:Equilibrium
Post by: Donaldson Tan on January 06, 2005, 10:34:02 AM

Le Chaterlier's Principle states that a system in equilibrium will tend to counter the stress acting on the system. if the stress is increasing the pressure, the system will shift such that there will be a reduction in pressure. if the stress is heat, the system will shift in equilibrium such that there will be less heat. hence, an increase in temperature will favour the endothermic reaction, ie. your backward reaction.

Title: Re:Equilibrium
Post by: cerez05 on January 06, 2005, 08:04:03 PM

Alright thank you I understand