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The reaction below was studied by performing two experiments.
NO(g) + O3(g) → NO2(g) + O2(g)
In the first experiment (results shown in left table) the rate of disappearance of NO was followed in a large excess of O3. (The [O3] remains effectively constant at 1.0x1014 molecules/cm3.)
In the second experiment [NO] was held constant at 2.0x1014 molecules/cm3. The data for the disappearance of O3 are in the right table.
The rate of reaction is given by Rate = k[NO]x[O3]y
Determine x and y. (Both need to be correct for credit.)
Alrighty kiddos I'm gonna be real all this stuff is gonna be hard, but its okay because I went through the struggle for ya.
So we need to figure out how the molarity of NO and O3 increases throughout the experiment.
In the gas phase the production of phosgene from chlorine and carbon monoxide proceeds by the mechanism given below. The rate of reaction is
Rate = k[CO]x[Cl2]y
Determine x and y.