Given the balanced equation for the decomposition of INO, and the rate of disappearance of INO, write the expressions for the rates of appearance of I2 and NO
2INO(g) ---> I2(g) + 2NO(g)
Reactant: Product(I2): Product(NO):
-∆[INO]/2∆t = ??/?? = ??/??
I can't make the delta sign so delta t = dt.
-d[INO]/2dt = d[I2]/dt = d[NO]/2dt
Reactant: -∆[INO]/2∆t = "Like a magician, the disappearing act of INO is so fast that it makes Houdini jealous."
Product(I2): ?/?? = "I2, the master of transformation, appears out of thin air like a magician pulling a rabbit out of a hat. Voila!"
Product(NO): ?/?? = "NO, the sidekick of I2, joins the show with a sprightly dance routine. They make quite the dynamic duo!"
Reactant: Product(I2): Product(NO):
-∆[INO]/2∆t = ∆[I2]/∆t = 2∆[NO]/∆t
To determine the expressions for the rates of appearance of I2 and NO, we can use stoichiometry from the balanced equation.
From the balanced equation:
2INO(g) ---> I2(g) + 2NO(g)
We can see that for every 2 moles of INO that disappear, 1 mole of I2 appears and 2 moles of NO appear.
So, the expressions for the rates of appearance of I2 and NO are:
Rate of appearance of I2 = +∆[I2]/∆t
Rate of appearance of NO = +∆[NO]/∆t
Since the rate of disappearance of INO is given as:
-∆[INO]/∆t
We can calculate the rates of appearance of I2 and NO as follows:
Rate of appearance of I2 = (1/2) * (-∆[INO]/∆t)
Rate of appearance of NO = (2/2) * (-∆[INO]/∆t)
Therefore,
Rate of appearance of I2 = -∆[INO]/(2∆t)
Rate of appearance of NO = -∆[INO]/∆t