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Transcription of this question: 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)(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.The graph below shows the Maxwell—Boltzmann distribution of molecular energies at aparticular temperature.[2]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]

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