Chemistry term paper

1. The reaction X + X₃ → 2 X₂ is shown to have an activation energy of 35 kJ/mol while the enthalpy of reaction (∆H) is -388 kJ/mol. What is the activation energy of the reverse reaction? 2.What is the activation energy of a reaction if it has the following rate constants? 3 The activation energy Ea for a particular reaction is 42.2 kJ/mol. How much faster is the reaction at 343 K than at 314 K? (R = 8.314 J/mol • K). 4. The activation energy Ea for a particular reaction is 50.0 kJ/mol. How much faster is the reaction at 315 K than at 310.0 K? (R = 8.314 J/mol • K) 5 The activation energy for a particular reaction is 102 kJ/mol. If the rate constant is 1.35 × 10⁻⁴ s⁻¹ at 306 K what is the rate constant at 273 K?. 6. What is the activation energy for the isomerization of methyl isocyanide? 7 The activation energy Ea for a particular reaction is 13.6 kJ/mol. If the rate constant at 754 °C is 24.5/min at what temperature (in °C) will the rate constant be 20.5/min? (R = 8.314 J/mol • K). 8. The activation energy Ea for a particular reaction is 37.8 kJ/mol. If the rate constant at 280 K is 0.178 M/s then what is the value of the rate constant at 425 K? (R = 8.314 J/mol • K) 9.A reaction is determined to have the rate law rate = k[NO]²[H₂]. What is the rate-determining step in the mechanism? A) Step 1 B) Step 2 C) Step 3 D) Cannot be determined from the rate law 10. Identify the molecularity of the elementary reaction below: 2HI(g)→ H₂(g) + I₂(g) A) unimolecular B) bimolecular C) termolecular D) quadmolecular 11. What is the molecularity of the rate-determining step in the proposed mechanism? A) unimolecular B) bimolecular C) termolecular D) Cannot be determined from given mechanism 12. The following reaction 2 NO(g) + O₂(g) → 2 NO₂(g) was found to be first in each of the two reactants and second overall. The rate law is therefore A) rate = k[NO]²[O₂] B) rate = k[NO][O₂] C) rate = k[NO₂]² – [NO]² – [O₂] D) rate = k[NO]²[O₂]² E) rate = k([NO][O₂])⁻² 13. Consider the multistep reaction. What is the best rate law for the overall reaction? A) Rate = k₁[A][B][C] B) Rate = k₂[C] C) Rate = k₁[A]²[B] D) Rate = (k₁[A][B])/(k₂[C]) E) Rate = k₁k₂[A]²[B] 14. Consider the proposed mechanism for the decomposition reaction 2 H₂O₂(aq) → 2 H₂O(l) + O₂(g) in the presence of I⁻(aq). What is the rate law for this reaction? A) rate = k[H₂O₂] B) rate = k[H₂O₂]² C) rate = k[H₂O₂][I⁻] D) rate = k[H₂O₂][IO⁻] E) rate = k[H₂O₂]²[I⁻]/[H₂O] 15. What is the rate law for the proposed mechanism? A) rate = k[H₂][NO] B) rate = k[H₂]²[NO] C) rate = k[H₂][NO]² D) rate = k[H₂]²[NO]² E) rate = k[H₂][N₂O] 16. For the reaction mechanism shown identify the intermediate(s). A) Cl(g) B) Cl₂(g) C) HCl(g) D) CCl₃(g) E) Cl(g) and CCl₃(g) 17. The Haber Process: N₂ + 3H₂ → 2NH₃ is an important industrial route for the production of ammonia. However the reaction does not occur fast enough at room temperature to be useful. What could be done to increase the rate of this reaction the most? A) Decrease the temperature B) Add a catalyst C) Increase the temperature D) Decrease the temperature and add a catalyst E) Add a catalyst and increase the temperature 18. For the following reaction mechanism what is the catalyst? A) O(g) B) O₂(g) C) O₃(g) D) NO(g) E) NO₂(g) 19. Which of the following statements is false about catalysts? A) Enzymes are biological catalysts. B) A catalyst is consumed in a chemical reaction. C) A catalyst increases reaction rate by providing an alternate reaction pathway with a lower activation energy. D) A catalyst may undergo change during a reaction but is unchanged at the end of a reaction. E) Catalysts may be homogeneous or heterogeneous. 20. A certain reaction has an activation energy of 39.5 kJ/mol. As the temperature is increased from 25.0°C to a higher temperature the rate constant increases by a factor of 2.80. Calculate the higher temperature (in °C). 21. The decomposition of ethylene oxide (CH₂)₂O(g) → CH₄(g) + CO(g) is a first reaction with a half-life of 58.0 min at 652 K. The activation energy of the reaction is 218 kJ/mol. Calculate the half-life at 621 K. 22. For homework points solve the rate law for: One proposed mechanism for the decomposition of N2O5 to NO2 involves three elementary steps: Step 1: 2 N2O5 <—–> N4O10 fast and reversible Step 2: N4O10 ⟶ N2O3 + 2 NO2 + O3 slow Step 3: N2O3 + O3 ⟶ 2 NO2 + O2 fast What is the overall reaction and rate law based on the proposed mechanism? Make sure to give me the answers in pdf file.