Experiments show that each of the following redox reactions is second-order overall: (1) no2(g) + co(g) → no(g) + co2(g) (2) no(g) + o3(g) → no2(g) + o2(g) (a) when [no2] in reaction 1 is doubled, the rate quadruples. determine the rate law for this reaction. rate = k[no2][co] k[no2]2 k[no2]3[co]−1 k[no2]4[co]−2 (b) when [no] in reaction 2 is doubled, the rate doubles. determine the rate law for this reaction.

a) rate law1 = k[NO2]²

b) rate law2 = k[NO][O3]

Explanation:

NO2(g) + CO(g) → NO(g) + CO2(g)

NO(g) + O3(g) → NO2(g) + O2(g)

When [NO2] in reaction 1 is doubled, the reaction quadruples

Rxn is second order.

rate law1= [NO2]^a [CO]^b

rate law1= [NO2]² [CO]^0

rate law1 = k[NO2]²

When [NO] in reaction 2 is doubled, the rate doubles.

Rxn is first order

The ratio is 1:1

this makes the rate law2 = k[NO][O3]

the answer is: they rebelled against saddam hussein’s rule.

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answer: the rate of diffusion increases with increase in temperature.

increase in temperature, increases the molecular/particles speed (kinetic energy. diffusion means movement of particles through the material.

generally, the heavier the particle the more it interacts with the environment and more the temperature matters. so higher temperature results in higher diffusion.