The gas-phase oxidation of nitrogen monoxide is represented by the overall reaction 2NO(g)+O2(g)→2NO2(g). For the temperature used in a particular experiment, the rate law has been determined to be rate=k[NO]2[O2], where k is a constant for that temperature.
(a) A mixture designated as Trial 1 has initial partial pressures of 0.10atm for both NO and O2. In Trial 2 the initial partial pressure of NO is doubled to 0.20atm while the partial pressure of O2 remains 0.10atm. Calculate the factor by which the initial rate in Trial 2 differs from that in Trial 1.
(b) Explain, without numerical calculation, why changing only the concentration of NO affects the reaction rate even though O2 is also a reactant.
(c) Describe one practical laboratory precaution you would take to ensure that concentration is the only factor influencing the rate difference between the two trials.