Reaction Reversibility Read 14.2 (pg. 553) 1.Colourless N2O4gas breaks down into brown NO2gas. Write the equilibrium equation for this reaction. 2.How is the existence of equilibrium indicated in a chemical equation? 3.Because the two gasses in this equilibrium are different colours, their concentrations can be determined using a spectrophotometer. The following chart indicates what happens over time following the addition of 1 mol N2O4to an empty 1 L vessel. Plot the data (include title and label axes). Time (min) 0 1 2 3 4 5 6 7 8 9 10 11 12 [N2O4] 1.00 0.70 0.45 0.350.300.2184.108.40.206 0.21 0.200.200.20[NO2] 0 0.60 1.10 1.301.401.461.501.541.56 1.58 1.601.601.604.Was all of the N2O4used up in the reaction? How does the graph show this? 5.According to the graph, how many moles of NO2were produced? 6.How many moles of NO2would have been produced if all of the N2O4was used up? 7.Use the collision theory to explain why all of the N2O4is not used up and why equilibrium is eventually established (think about forward versus reverse reactions, and how concentration affects reaction rate).
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