Given:
T1 = 250 oC
=(250+273)K
= 523 K
T2 = 325 oC
=(325+273)K
= 598 K
K2/K1 = 5.6/1
use:
ln(K2/K1) = (Ea/R)*(1/T1 - 1/T2)
ln(5.6/1) = ( Ea/8.314)*(1/523 - 1/598)
1.7228 = (Ea/8.314)*(2.398*10^-4)
Ea = 59728 J/mol
Ea = 59.7 KJ/mol
Answer: 59.7 KJ/mol
Consider the reaction below; (6 points) N2O2(g) + O2(g) + 2NO2(g) When the reaction is performed at 250.0°C and aga...
9. Consider the reaction below; (6 points) N2O2(g) + O2(g) + 2NO2(g) When the reaction is performed at 250.0°C and again at 325.0°C, the rate constant increases by a factor of 5.6. Use the information to calculate the activation en reaction.
Consider the following reaction: 2NO(g)+O2(g)⇌2NO2(g)2NO(g)+O2(g)⇌2NO2(g) The data in the table show the equilibrium constant for this reaction measured at several different temperatures. Temperature K 400 1.9x10^7 425 2.5x10^6 465 1.6x10^5 515 8.8x10^3 600 2.0x10^2 Use the data to find ΔrS∘ΔrS∘ for the reaction. (answer in J K-1 mol-1) The answer is NOT 158
Consider the reaction: 2NO(g) + O2(g)2NO2(g) Using standard thermodynamic data at 298K, calculate the free energy change when 1.710 moles of NO(g) react at standard conditions. G°rxn = kJ
For the reaction 2 NO (g) + O2 (g) → 2 NO2 (g) it is found that the rate doubles when the O2 concentration is doubled, but the rate increases by a factor of 4 when the NO concentration is doubled. Which of the following mechanisms is/are consistent with this? 1. (i) NO + O2 ⇋ NO3 (fast) (ii) NO + NO3 → 2 NO2 (slow) 2. (i) 2 NO → N2O2 (slow) (ii) O2 + N2O2 → N2O4 (fast)...
10. Consider the reaction A + 2B → C ne rate law for this reaction is on der in and and order in B if the rate constant at 25°C is 1.25x 105 , find the rate of reaction when the concentration of A is 0.27M and the concentration of B is 0.32 M UMA 21 11. Consider the reaction A +2B C + D. The rate law for this reaction is first order in A and zeroth order in...
2. (10 pts) Consider the following second-order reaction: 2NO2(g) + 2NO(g)+O2(g) The rate constant is 0.54 M-15-1, at 300 °C. How long would it take for the concentration of NO2 to decrease from 0.62M to 0.28M?
Question 6: Reaction Mechanisms (9 points) For the reaction: 2NO2 → 2NO + O2 Suppose there are two possible mechanisms to define a particular reaction. These two mechanisms are proposed below: 1. NO2 → NO + O (slow) O + NO2 → O2 + NO (fast) 2. 2NO2 → NO3 + NO (slow) NO3 → NO + O2 (fast) a) Identify the rate for each reaction and the order of each reaction. (4 points) b.) Identify the intermediate for each...
The reaction 2NO(g)+O2(g)→2NO2(g) is second order in NO and first order in O2. When [NO]= 4.5×10−2 M and [O2]= 3.7×10−2 M , the observed rate of disappearance of NO is 9.9×10−5 M/s . What is the rate of disappearance of O2 at this moment?
13. Consider the reactions below; H2S(g) + H2O(1) H2S(g) + 2H2O(l) H30'(aq) + HS (ag); K1 - 2.5 x 10 + 2H30 (aq) + (aq); K3 = 6.8 x 10-16 Use the information above to calculate the K for the reaction given below (6 points); HS (aq) + H2O(0) H:0 (aq) + (aq); K = ? 14. Consider the reaction below; 2NO2(g) + 2Cl2 2NOCl2(g) + O2(g) If the equilibrium constant Kat 100°C is 1.5 x 10, calculate its k....
The rate law for the reaction 2NO2 + O3 → N2O5 + O2 is rate = k[NO2][O3]. Which one of the following mechanisms is consistent with this rate law? A) NO2 + NO2 → N2O4 (fast) N2O4 + O3 → N2O5 + O2 (slow) B) NO2 + O3 → NO5 (fast) NO5 + NO5 → N2O5 + 5/2O2 (slow) C) NO2 + O3 → NO3 + O2 (slow) NO3 + NO2 → N2O5 (fast) D) NO2 + NO2 → N2O2...