The rate law for the reaction NO + O2 > NO2 is R=k[NO][O2]. what will be the effect on the reaction rate if the partial pressure of NO is doubled? What will the effect be if the partial pressure of O2 is tripled?
My answer: More NO2 would be produced if NO was doubled. If O2 tripled, then there would be more oxygens in NO2.
See your post above about OH^- and H2PO2^2-.
Same scenario.
So NO will be doubled in the rate and O3 will be tripled.
Doubling NO will double the rate. If you mean rate will be tripled if O2 is tripled, yes, that's right.
Lactose(MWT:342 amu)makes up the vast majority of carbohydrates. calculate the molarity of lactose in butter milk
Lactose (mwt:342amu)makes up the vast carbohydrate.calcilate the lactose in buttermilk
To determine the effect of changing the partial pressure of NO or O2 on the reaction rate, we need to consider the rate law equation R=k[NO][O2], where R represents the reaction rate, k is the rate constant, [NO] represents the concentration of NO, and [O2] represents the concentration of O2.
If the partial pressure of NO is doubled, it means that the concentration of NO will also double (assuming ideal gas behavior). Consequently, the reaction rate will increase because the rate law is directly proportional to the concentration of NO. Therefore, doubling the partial pressure of NO will lead to a proportional increase in the rate of the reaction.
On the other hand, if the partial pressure of O2 is tripled, it indicates that the concentration of O2 will also increase by a factor of three. Since the rate law depends on the concentration of O2, tripling the partial pressure of O2 will result in a threefold increase in the rate of the reaction.
In summary, doubling the partial pressure of NO will lead to a proportional increase in the reaction rate, while tripling the partial pressure of O2 will cause the reaction rate to increase by a factor of three.