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What would happen if NO were added to N2(g) plus O2(g) 2NO(g) at equilibrium?
Adding NO would shift the equilibrium position to the left, favoring the formation of N2 and O2. This occurs to compensate for the increase in product concentration, restoring equilibrium. The concentrations of N2 and O2 would increase, while the concentration of NO would decrease.
What would happen if O2 were added to N2(g) plus O2(g) 2NO(g) at equilibrium?
More N2 and O2 would form
What would happen if N2 were added to N2(g) O2(g) 2NO(g) at equilibrium?
If N2 were added to the equilibrium mixture, the reaction would shift to the right to consume some of the additional N2. This would lead to an increase in the concentration of NO and a decrease in the concentrations of N2 and O2 until a new equilibrium is established.
What is the equilibrium constant for the reaction N2(g) O2(g) 2NO(g)?
More NO would form
What is the balanced equation of nitrogen gas with oxygen gas to produce nitrogen monoxide at an equilibrium constant?
The balanced equation for the reaction between nitrogen gas and oxygen gas to produce nitrogen monoxide is: 2N2(g) + O2(g) ⇌ 2NO(g) The equilibrium constant for this reaction would be expressed as K = [NO]^2 / [N2]^2[O2].
What would happen if N2 were added N2(g) O2(g) 2NO(g) at equilibrium?
More NO would form
What would happen if NO were added to N2(g) O2(g) 2NO(g) at equilibrium?
More N2 and O2 would form
What wpuld happen if NO were added to N2(g) O2(g) 2NO(g) at equilibrium?
If NO were added to the equilibrium reaction N₂(g) + O₂(g) ⇌ 2NO(g), the system would respond by shifting to the left to counteract the change, according to Le Chatelier's principle. This shift would result in the conversion of some NO back into N₂ and O₂, thus partially restoring the equilibrium. Consequently, the concentrations of N₂ and O₂ would increase while the concentration of NO would decrease until a new equilibrium is established.
What would happen if NO were added to N2 g O2 g equals 2NO g at equilibrium?
If NO is added to the equilibrium of the reaction ( N_2(g) + O_2(g) \rightleftharpoons 2NO(g) ), the equilibrium will shift to the left according to Le Chatelier's principle. This shift will result in the consumption of some NO, leading to an increase in the concentrations of ( N_2 ) and ( O_2 ) until a new equilibrium is established. The overall effect will be a decrease in the concentration of NO in the system as it reacts with the available ( N_2 ) and ( O_2 ).
What would happen if NO were added to N2(g) plus O2(g) at equilibrium?
N2(g) + O2(g) 2NO(g)Adding NO would push the reaction to the left, toward the reactants. This is according to Le Chatelier.
What would happen if NO were added to N2(g) plus O2(g) 2NO(g) at equilibrium?
Adding NO would shift the equilibrium position to the left, favoring the formation of N2 and O2. This occurs to compensate for the increase in product concentration, restoring equilibrium. The concentrations of N2 and O2 would increase, while the concentration of NO would decrease.
What would happend if NO were added to n2(g) o2(g) 2no(g) at equilibrium?
If NO is added to the equilibrium mixture of N₂(g), O₂(g), and 2NO(g), the system will respond according to Le Chatelier's principle. The equilibrium will shift to the left, favoring the formation of reactants (N₂ and O₂) to counteract the increase in NO concentration. This shift will result in a decrease in the concentration of NO and an increase in the concentrations of N₂ and O₂ until a new equilibrium is established.
What would happen if NO were added to N2(g) plus O2(g) 2NO(g) at equilibruim?
more N2 and O2 would form
What would happen if O2 were added to N2 plus O2 gives 2NO at equilibrium?
N2(g) + O2 (g)--> 2NO(g)The arrow should of course be the reversible sign.Le Chatelier's principle states that a system at equilibrium will move to undo any change imposed upon it, so adding oxygen will make the equilibrium move to the right, increasing the amount of nitric oxide.
What would happen if N2 were added to N2(g) O2(g) 2NO(g) at equilibrium?
If N2 were added to the equilibrium mixture, the reaction would shift to the right to consume some of the additional N2. This would lead to an increase in the concentration of NO and a decrease in the concentrations of N2 and O2 until a new equilibrium is established.
What would happen if O2 were added to N2(g) plus O2(g) 2NO(g) at equilibrium?
More N2 and O2 would form
What is the equilibrium constant for the reaction N2(g) O2(g) 2NO(g)?
More NO would form
