Understanding Equilibrium Shift in the Haber Process (N2 + 3H2 ⇔ 2NH3)

  • Thread starter Thread starter 24forChromium
  • Start date Start date
  • Tags Tags
    Equilibrium Shift
AI Thread Summary
In the Haber process (N2 + 3H2 ⇔ 2NH3), the system is not in equilibrium if the molar ratios of reactants and products do not match the stoichiometric coefficients. With 2 moles of N2, 3 moles of H2, and 1 mole of NH3, the reaction quotient can be calculated to determine the direction of the shift. If the reaction quotient is less than the equilibrium constant, the system will shift toward the products; if greater, it will shift toward the reactants. Understanding these ratios and the equilibrium constant is essential for predicting the behavior of the system. Proper calculations are necessary to ascertain the equilibrium state.
24forChromium
Messages
155
Reaction score
7
Please post this type of questions in the HW section using the template.
in the Haber process (N2 + 3H2 ⇔ 2NH3),
if there are 2mol of N2, 3mol of H2 and 1mol of NH3, how do I know that the system is not in equilibrium and which direction will it shift?
 
Physics news on Phys.org
Hi man;
The solution is easy. Just look at the number of each element. Nitrogen, for example, have 2 atoms in the left (reactants) and 2 atoms in the right (products) and this true about the Hydrogen atoms.
 
About second part of your question ''which direction will it shift''. You should notice that the reaction is both toward the products and reactants, that's why it called the reaction is on equilibrium.
 
You can't do anything without the equilibrium constant - you need to calculate reaction quotient and compare it with the equilibrium constant.
 
Thread 'Confusion regarding a chemical kinetics problem'

Thread 'Confusion regarding a chemical kinetics problem'

TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
View full post »

Thread 'Prove that evolution is constant (Provide at least two arguments to support your position)'

I don't get how to argue it. i can prove: evolution is the ability to adapt, whether it's progression or regression from some point of view, so if evolution is not constant then animal generations couldn`t stay alive for a big amount of time because when climate is changing this generations die. but they dont. so evolution is constant. but its not an argument, right? how to fing arguments when i only prove it.. analytically, i guess it called that (this is indirectly related to biology, im...
View full post »

Similar threads

Chemistry Calculating Final Composition of Compounds in Haber's Process with 50% Yield
Replies
10
Views
2K
Thermodynamics equilibrium constant problem
Replies
9
Views
2K
Calculate Delta G & Delta H of N2+3H2=>2NH3
Replies
1
Views
4K
2NH3->N2+3H2. Rate=k[NH3]/[H2], what is the mechanism?
Replies
1
Views
13K
Chemistry/The equilibrium number/ I really
Replies
1
Views
2K
Equilibrium constant (K) Question problem
Replies
1
Views
3K
Calculating Maximum Ammonia Mass from Nitrogen and Hydrogen Reaction
Replies
1
Views
2K
How Do Stoichiometric Coefficients Affect Gibbs Free Energy Calculations?
Replies
3
Views
3K
Solving Gas Laws: 3H2 + N2 -> 2NH3 at 110 ATM
Replies
7
Views
2K
Increasing Yield of a System with Le Chatelier's Principle
Replies
5
Views
2K

Hot Threads

Recent Insights

Back
Top