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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 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
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 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 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
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 is the balanced equation of nitrogen monoxide with oxygen to poduce nitrogen dioxide at an equilibrium constant?
The balanced equation for this reaction is: 2NO(g) + O2(g) ⇌ 2NO2(g) At equilibrium, the equilibrium constant, Kc, would be equal to [NO2]^2 / ([NO]^2 * [O2]).
Is the equation 2NO O2 - NO2 balanced why or why not?
2NO + O2 --> NO2 is not balanced. There are two nitrogen atoms on the left and only one on the right. There are four oxygen atoms on the left and only one on the right. The correct balanced equation is 2NO + O2 --> 2NO2.
