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Transcription of this question: 2.The thermal decomposition of dinitrogen monoxide occurs according to the equation:2NP(g) 2N2(g) + 02(g)The reaction can be followed by measuring the change in total pressure, at constanttemperature, with time.The x-axis and y-axis are shown with arbitrary units.35030025020015010050O246810Time12141618(a)Explain why, as the reaction proceeds, the pressure increases by the amount shown.20[2](b) Outline, in terms of collision theory, how a decrease in pressure would affect the rate ofreaction.[2](c)This decomposition obeys the rate expression:0)(ii)d[N20]= k[N20]Deduce how the rate of reaction at t = 2 would compare to the initial rate.It has been suggested that the reaction occurs as a two-step process:Step 1:N20(g) N2(g) + O(g)step 2:N20(g) 02(g)Explain how this could support the observed rate expression.[2](d)The experiment is repeated using the same amount of dinitrogen monoxide in thesame apparatus, but at a lower temperature.Sketch, on the axes in question 2, the graph that you would expect.The experiment gave an error in the rate because the pressure gauge was inaccurate.Outline whether repeating the experiment, using the same apparatus, and averagingthe results would reduce the error.[2](f)The graph below shows the Maxwell—Boltzmann distribution of molecular energies at aparticular temperature.Kinetic energyThe rate at which dinitrogen monoxide decomposes is significantly increased by ametal oxide catalyst.Annotate and use the graph to outline why a catalyst has this effect.[2]Determine the standard entropy change, in JK-I, for the decomposition ofdinitrogen monoxide.2NP(g) 2N2(g) + 02(g)[2]SpeciesN 2002SO/ J morw220193205(ii)Dinitrogen monoxide has a positive standard enthalpy of formation, AHreDeduce, giving reasons, whether altering the temperature would change thespontaneity of the decomposition reaction.

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