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If the volume of the reaction vessel is decreased will the yield of ammonia increase or decrease and why?
If you decrease the volume of the of the reaction vessel, you will get a higher yield of ammonia. This is because, decreasing the volume means the particles are more crammed in together and they will collide successfully more often and frequently. This causes a shift in the direction that produces more gas molecules. And since the balances equation for ammonia production is: N2 + 3H2 ----> 2NH3 4 particles on the left, 2 on the right, meaning it will shift to the right, i.e. to the production of ammonia. Hope this helps!
What does Le Châteliers principle state?
Le Chatelier's principle essentially states that if a stress is imposed on a system at equilibrium, the equilibrium will shift to minimize the stress. These stresses include: -Change in temperature -Change in pressure/volume (for gases) -Change in concentration A simple example of this: N2(g) + 3 H2(g) ⇌ 2 NH3(g) ΔH = −92kJ/mol -If you add N2(g) or 3 H2(g) the equilibrium will shift to the right (to the products), and more NH3(g) will be created so as to minimize the stress. - If you add NH3(g), the equilibrium will shift to the left (to the reactants), and more N2(g) and H2(g) will be created. -If you increase the temperature, the equilibrium will shift to the left (to the reactants). The reason for this is that the above reaction is exothermic, and releases heat. Consequently, the heat is on the side of the products, and thus if you add heat, the equilibrium will shift to the reactants and more N2(g) and H2(g) will be created. - If you increased the pressure, which is the same as decreasing the volume, the reaction will shift to the side with fewer moles, which, in this case, is the products. Thus, more NH3(g) will be created. -Conversely, if you decrease the pressure (increase the volume), the reaction will shift to the side with a greater number of moles, which, in this case, is the reactants. Thus, more N2(g) and H2(g) will be created. *It is important to note that changing pressure and volume only effects the equilibrium in gaseous reactions!
How does temperature affect the Keq of a reaction?
Changing the temperature will change Keq. (apex.)
What Will Happen To The Equilibrium Concentration Of Carbonic Acid If The Pressure Of Carbon Dioxide Is Increased In The Container?
The equilibrium concentration of carbonic acid will increase because the system will shift to the right to relieve the increase in pressure by consuming more of the carbon dioxide to produce more carbonic acid. This shift helps maintain the equilibrium constant for the reaction.
What does Le Chtelier's principle say about upsetting a system at equilibrium?
Le Chatelier principle says, if a restriction is applied to a system in equilibrium, the system adjusts to a new equilibrium that tends to counteract the restriction. When equilibrium is under stress it will shift to relieve that stress. or all concentrations would change.
If the volume of the reaction vessel is decreased will the yield of ammonia increase or decrease and why?
If you decrease the volume of the of the reaction vessel, you will get a higher yield of ammonia. This is because, decreasing the volume means the particles are more crammed in together and they will collide successfully more often and frequently. This causes a shift in the direction that produces more gas molecules. And since the balances equation for ammonia production is: N2 + 3H2 ----> 2NH3 4 particles on the left, 2 on the right, meaning it will shift to the right, i.e. to the production of ammonia. Hope this helps!
What does Le Châteliers principle state?
Le Chatelier's principle essentially states that if a stress is imposed on a system at equilibrium, the equilibrium will shift to minimize the stress. These stresses include: -Change in temperature -Change in pressure/volume (for gases) -Change in concentration A simple example of this: N2(g) + 3 H2(g) ⇌ 2 NH3(g) ΔH = −92kJ/mol -If you add N2(g) or 3 H2(g) the equilibrium will shift to the right (to the products), and more NH3(g) will be created so as to minimize the stress. - If you add NH3(g), the equilibrium will shift to the left (to the reactants), and more N2(g) and H2(g) will be created. -If you increase the temperature, the equilibrium will shift to the left (to the reactants). The reason for this is that the above reaction is exothermic, and releases heat. Consequently, the heat is on the side of the products, and thus if you add heat, the equilibrium will shift to the reactants and more N2(g) and H2(g) will be created. - If you increased the pressure, which is the same as decreasing the volume, the reaction will shift to the side with fewer moles, which, in this case, is the products. Thus, more NH3(g) will be created. -Conversely, if you decrease the pressure (increase the volume), the reaction will shift to the side with a greater number of moles, which, in this case, is the reactants. Thus, more N2(g) and H2(g) will be created. *It is important to note that changing pressure and volume only effects the equilibrium in gaseous reactions!
Increasing the volume of a closed system at equilibrium will?
cause a shift in the equilibrium towards the side with more gas molecules, according to Le Chatelier's principle. This is because increasing the volume decreases the pressure, and the system will shift to relieve the pressure by favoring the side with more gas molecules.
How does temperature affect the Keq of a reaction?
Changing the temperature will change Keq. (apex.)
What Will Happen To The Equilibrium Concentration Of Carbonic Acid If The Pressure Of Carbon Dioxide Is Increased In The Container?
The equilibrium concentration of carbonic acid will increase because the system will shift to the right to relieve the increase in pressure by consuming more of the carbon dioxide to produce more carbonic acid. This shift helps maintain the equilibrium constant for the reaction.
What does Le Chtelier's principle say about upsetting a system at equilibrium?
Le Chatelier principle says, if a restriction is applied to a system in equilibrium, the system adjusts to a new equilibrium that tends to counteract the restriction. When equilibrium is under stress it will shift to relieve that stress. or all concentrations would change.
What would happen to the equilibrium price and quantity exchanged if an increase in income and a decreasing price of complement for a normal good?
the equilibrium price and quantity exchanged will go up because thr curve of demand shift rightward in both situations.
What happens to the equilibrium concentration of reactants when the volume of the reaction system is decreased and why?
When the volume of the reaction system is decreased, the equilibrium will shift towards the side of the reaction with fewer moles of gas to relieve the pressure. This causes the concentration of reactants to increase in order to establish a new equilibrium.
Which way will equilibrium reaction shift if keg is large or small?
If the equilibrium constant (K_eq) is large, it means the products are favored at equilibrium. The reaction will shift toward the products to establish equilibrium. If K_eq is small, it means the reactants are favored at equilibrium. The reaction will shift toward the reactants to establish equilibrium.
How are the terms stress and shift used when discussing systems at equilibrium?
In equilibrium, stress means the manner in which equilibrium is altered, and shift represents which direction the equilibrium will move to compensate for the stress.
If a chemical reaction has reached equilibrium and you lower the pressure of the system while keeping the temperature constant what happens to the equilibrium of the reaction?
If all the reactants occupy more volume than all of the products, the reverse reaction will be favored. If all the reactants occupy less volume than all of the products, the forward reaction will be favored. If the products and reagents have the same volume, the equilibrium will not change.
How does the amount on this system affect the amount of N2O4 formed?
The amount of reactants in a system directly affects the amount of products formed. In the case of the reaction forming N2O4, increasing the amount of reactants (NO2) will shift the equilibrium towards forming more N2O4. Conversely, decreasing the amount of reactants will shift the equilibrium towards forming more NO2.
