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1. Pease (1932) studied the gas phase hydrogenation of ethene to form ethane at normal pressure and across the temperature range 202 to 272 °C. (a) C₂H₂ + H₂ → C₂H6 Pressure was not varied as part of this experimental study, but would pressure have any influence on this reaction? Justify your answer. A series of different mixtures of the two reagent components was generated and an initial reaction rate was determined, shown in Table 1.1. Table 1.1: Initial reaction rate for the hydrogenation of ethene at 232 °C. [H₂] [mol m²] [mol m³s¹] [C₂H₂] [mol m 0.0005 0.0005 1.720E-23 1.376E-23 1.032E-23 6.878E-24 3.439E-24 0.0004 0.0003 0.0002 0.0001 0.0005 0.0005 0.0005 0.0005 0.0005 0.0005 0.0005 0.0005 Temp ["C] 202 212 222 232 242 252 262 272 0.0004 0.0003 0.0002 0.0001 (b) From the rate data provided in Table 1, determine the reaction order. The rate constant for the reaction was evaluated over a range of temperatures and is provided in Table 1.2. 1.376E-23 1.032E-23 Table 1.2: Rate constant values determined for the hydrogenation of ethene at atmospheric pressure. k [not stated] 4.587E-18 1.174E-17 2.893E-17 6.878E-17 1.581E-16 6.878E-24 3.439E-24 3.522E-16 7.613E-16 1.600E-15/n(c) (d) (e) Based on the information provided in Table 1.2, if the reaction rate constant follows an Arrhenius type expression, determine the constants within the Arrhenius equation stating units. Comment on your answer to part c, are the values determined sensible? Write out the full rate equation for this reaction.

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