Consider the following reaction: NO(g) + NO3(g) --> 2NO2(g)which has an observed rate law of rate = k[NO][NO3].
a. Describe what would happen to the rate if the concentrationof NO was cut in half with NO3 held constant.
b. What does this mean on the particle level in terms ofdistance between NO and NO3 particles?
c. Describe what would happen to the rate if the concentrationof NO was doubled with NO3 held constant.
d. What does this mean on the particle level in terms ofdistance between NO and NO3 particles?
e. What if the concentration of NO was very high and NO3 wasvery low -- what would happen to the rate of the reaction (and whatwould affect the rate the most, a slighter increase to [NO] or[NO3])?
** Would love to fully understand this, not just get an answer!Thank you.
