What is the G°rxn for the reaction in question?
NO(g) + O(g) -> NO2(g) Grxn= -676.0kJ
2O3(g) -> 3O2(g) Grxn= +489.6kJ
O2(g) -> 2O(g) Grxn = ??
NO(g) + O3(g) -> NO2(g) + O2(g) Grxn=-199.5kJ
What is the G°rxn for the reaction in question? NO(g) + O(g) -> NO2(g) Grxn= -676.0kJ...
Given the following data: 2O3(g) 3O2(g) -427 kJ O2(g) 2O(g) 495 kJ NO(g) + O3(g) NO2(g) + O2 -199kJ Calculate (in kJ) for the reaction: NO(g) + O(g) NO2(g)
Calculate the enthalpy change for the reaction NO(g) + O(g) → NO2(g) from the following data NO(g) + O3(9) → NO2(g) + O2(g) ΔH=-198.9 kJ/mol O3(g) → 1.5O26(g) ΔH=-142.3 kJ/mol O2(g) → 2O(g) ΔH = 495.0 kJ/mol A. 153.8 kJ B. 190.9 kJ C.-551.6 kJ D.-304.1 kJ E. 438.4 kJ
Question 62 Calculate the enthalpy change for the following reaction: NO(g) + O(g) - NO2(g) from the following data: NO(g) + O3(g) – NO2(g) + O2(g) O3(g) – 1.502(g) O2(g) - 20(g) AH = -198.9 kJ AH = -142.3 kJ AH = 495.0 kJ 0-304.1kJ 438.4 kJ 190.9 kJ 153.8 kJ O -551.6 kJ
NO + O3--->NO2+O3 find delta rxn H, delta rxn S, and delta rxn G. for this reaction A=7.9x10^11cm^3/mole-s and Ea =10.5 KJ/mol. find delta H,delta S, delta G++ for this reaction. draw a reaction coordinate diagram for this reaction scaled correctly. Temperature of 293.13
What is the role of NO(g) in the reaction mechanism below? NO(g) + O3(g) --> NO2(g) + O2(g) O(g) + NO2(g) --> NO(g) + O2(g)
from rxn mechanism 03+ no2 ->no3 +o2 (slow) no3+no2->n2o5 (fast) rate=k [o3]1 [no2]1 so here, I see that order is 1 for [o3] and [no2] because o3 + no2 has 1 coefficient in front. but my question is I learned that the order of reaction is not equal to the coefficient of species. !! so why coefficient is determined when writing rate of reaction here? this does not make sense to me.
Step 1: 03 (g) + NO (g) = NO2 (g) + O2 (g) Step 2: NO2 (g) + O (9) NO (g) + O2 (g) PE "IM Reaction path What is the overall rate law? Rate = k[O3] Rate = k[O3][0] Rate = k[O3][NO]
Calculate ΔS∘rxn for the reaction 2NO(g)+O2(g)→2NO2(g) Substance S∘ (J/mol⋅K) NO2 240.0 O2 205.2 NO 210.8
24. A mixture of O2(g) and O3(g) is present at equilibrium in a rigid container at 152 torr and 125° C. The density of the gaseous mixture is 0.228 g/L. Calculate Kp at 125° C for the reaction 3O2(g) 2O3(g)
For the reaction: N2O3(g) → NO(g) + NO2(g) at 298 K AG° = -4.78 kJ/mol RXN. Compute K for this reaction. a) 1.01 Ob) 0.998 O c) 0.948 O d) 6.89 Oe) 10.23