Acetonitrile (CH3CN) isomerizes to methylisonitrile (CH3NC) at high temperatures. Use the data below to determine the energy of activation (in kJ) of this reaction. Use the graphical method to complete this problem and sketch a rough drawing of the graph you use in the box provided, being sure to label the axes. Slope of the line =         Ea =

Which of the following is not an example of heterogeneous catalysis?     a) 2O3(g) → 3O2(g) has a catalyst of Cl(g) b) CO(g) + 3H2(g) → CH4(g)+H2O(g) has a catalyst of Co(s) c) C2H4(g) + H2(g) → C2H6(g) has a catalyst of Ni(s) d) 2CO(g) + 2NO(g) → 2CO2(g)+N2(g) has a catalyst Rh(s)

14.70 b A reaction has a rate constant of 1.26×10−4 s−1s−1 at 27  ∘C ∘C and 0.226 s−1s−1 at 77  ∘C ∘C .

In the reaction N2  +3 H2  à 2NH3  if the Δ[H2]/t  is   -1.5 x 10-3 M/s,  What is the Δ[NH3] at the same point? (How fast is the NH3 being produced)?

Consider these three reactions as the elementary steps in the mechanism for a chemical reaction.(i) Cl2 (g) + Pt (s) à 2Cl (g) + Pt (s) Ea = 1550 kJ ∆H = – 950 kJ(ii) Cl (g)+ CO (g) + Pt (s) à ClCO (g) + Pt (s) Ea = 2240 kJ ∆H = 575 kJ(iii) Cl (g) + ClCO (g) à Cl2CO (g) Ea = 2350 kJ ∆H = – 825 kJ e. Which reaction intermediate would be considered a catalyst (if any) and why?f. If you were to add 2700kJ of activation energy to the reaction, would you be able to make thereaction reverse itself (i.e. have the products become reactants)? Justify your answer.g. If you were to added a positive catalyst to step (iii) what would the end result be? Justify yourprediction.h. Your friend is looking at your graph and states that she believes that step (ii) is the ratedetermining step. Do you agree with her? Justify your reasoning.

Label the components of an energy diagram for a spontaneous reaction. 4 Energy- Reaction progress- Answer Bank activation energy catalyzed reaction reactants products uncatalyzed reaction

The Scenario Professor Ndekele asks you to test a new low temperature catalyst for the decomposition of ammonia, NH3. With previously existing catalysts decomposing ammonia requires a temperature of 450 ºC, but this new catalyst is said to be effective at a temperature of 100  ºC!   You plan to heat ammonia gas with the catalyst in a flask connected to a manometer and track the reaction by the change in pressure, which should increase as the temperature increases and as the reaction progresses and the number of moles of gas increases via the balanced chemical equation: 2 NH3 (g) → N2 (g) + 3 H2 (g) You make the following observations.   Observations Vflask = 1.00 L Patm = 630.5 mmHg TRoom = 23.2  ºC Before heating h = 0.00 As you heat the flask, the mercury falls on the flask side of the manometer and rises on the open end.  At 100.0  ºC, the height difference in the flask is 65.5 cm.   Analysis **convert all T-values to K for gas law calculations! Use the ideal gas equation to…