Adding NO to the system at equilibrium would increase the concentration of the NO product. According to Le Chatelier's principle, the system will counteract this change by producing more of the reactants, N2 and O2.
N2(g) + O2(g) 2NO(g)Adding NO would push the reaction to the left, toward the reactants. This is according to Le Chatelier.
More N2 and O2 would form
2HCN(g) N2(g) + C2H2(g)-1.The reverse reaction rate suddenly increases. 2.C2H2 is consumed.
N2 + O2 --> 2NO
More NO would form
More NO would form
More N2 and O2 would form
N2(g) + O2(g) 2NO(g)Adding NO would push the reaction to the left, toward the reactants. This is according to Le Chatelier.
N2(g) + O2(g) 2NO(g)Adding NO would push the reaction to the left, toward the reactants. This is according to Le Chatelier.
more N2 and O2 would form
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.
More N2 and O2 would form
2HCN(g) N2(g) + C2H2(g)-1.The reverse reaction rate suddenly increases. 2.C2H2 is consumed.
N2 + O2 --> 2NO
More NO would form
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.
N2 + o2 ----> 2no