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) |
Given the following data: 2O3(g) 3O2(g) -427 kJ O2(g) 2O(g) 495 kJ NO(g) + O3(g) NO2(g)...
Given the following data, 2 O3(g) ----> 3 O2(g) ∆rH = -377.00 kJ mol-1 O2(g) ----> 2 O(g) ∆rH = 545.00 kJ mol-1 NO(g) + O3(g) ----> NO2(g) + O2(g) ∆rH = -124.00 kJ mol-1 Determine ∆rH for the reaction, NO(g) + O(g) ----> NO2(g) ∆rH = ? kJ mol-1
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
1. 2O3(g)↔ 3O2(g) ; if 10.0g of O2 is at equilibrium with 7.50g of O3 calculate Kp if the total pressure is 1.10atm. A. 2.94 B. 0.499 C. 0.339 ^ I submitted this question already but the answer was wrong, I worked through it and still couldn't find one of these options. Suggestions? 2. For: N2(g) + O2(g) ↔ 2NO(g) 0.500M O2 and 0.750M N2 is allowed to reach equilibrium. Kc = 1.00 x 10-1. Calculate equilibrium concentration of N2...
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
1. Consider the following thermochemical equation. NO (g) +O3 (g) → NO2 (g) + O2(g) ΔΗ--1 99 kJ a) This reaction is i. endothermic ii. exothermic b) Calculate the amount of energy (kJ) released when 8.50 g of NO (g) is reacted with an excess of ozone, O3
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)
physical chemistry 2. The bond dissociation energy of oxygen gas is 495 kJ/mole, while the enthalpy of formation of ozone gas (O3(g))is 142.3 kJ/mole. For the reaction: NO +O3(g) NO2(g) + O2(g) it is found that AH = -198.9 kJ/mole, Determine the enthalpy change for the reaction: NO(g) + O() NO2(8)
Given the following data: C(s) + O2(g) → CO2(g) ΔH = -393.5 kJ CS2(l) + 3O2(g) → CO2(g) + 2SO2(g) ΔH = -1076.5 kJ C(s) + 2S(s) → CS2(l) ΔH = +89.4 kJ Find the ΔH of the following reaction: SO2(g) → S(s) + O2(g)
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
18. Consider the following data. 2 NO(g) N2(g) + O2(g) H = -180.7 kJ 2 NO(g) + O2(g) 2 NO2(g) H = -113.1 kJ 2 N2(g) + O2(g) 2 N2O(g) H = +163.2 kJ Use Hess's law to calculate H for the reaction below. 3 NO(g) N2O(g) + NO2(g) H = ______________ kJ