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Please show how to solve it. Given the thermochemical equation: 2NO2 (g)2N0(g) 02(g) ΔΗ-=114 k what...
Question 16 5 pts The thermochemical equation for the reaction of oxygen and nitrogen monoxide to form nitrogen dioxide is 2NO(g) + O2(g) 2NO2(g) AH = -114 kJ What is AH for the reaction re-written in the form NO2(g) -> NO(g) + KO2(g) AH = ? 228 kJ 114 kJ -57 kJ - 114 kJ 57 kJ
uations, calculate AH°rxn for the reaction: (3 marks) LFrom the following thermochemical eq So2(g)+NO2(8) SO3(8)+NO(g) 2 SO28)+02(8)-2SO3(8) 2N0(g) + O2(g. 2 NO2(g) A rxn--197.8 kJ Δ//orxn®-114, 14 kJ -SMB, eus e ,
what is Δ?ΔH for this reaction? Given the reactions X(s)02(g) ΔΗ-924.3 k XO(s) XCO3 (s)XO(s) + CO2 (g) ΔΗ+110.3 kJ what is AH for this reaction? X(s) 02(g)CO2(g) XCO,(s) ΔΗ= 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
(a) For the reaction 2NO2 (g) 2NO (g) + 02 (g) K # 0.50. Predict the direction in which the system will move to reach equilibrium if the initial gas pressures are NO: 0.20 atm . NO2: 0.20 atm (answer: to the right because Q< K) .NO2: 0.0961 atm 02: 0.0589 atm NO: 0.280 atm (answer: the system is already at equilibrium because Q -K) O2: 0.20 atm NO: 0.56 atm NO2: 0.20 atm (answer: to the left because Q>...
Given the following reactions Question 1 Given the following reactions AH 66.4 k N2 (g)+202 (g)2NO2 (g) 2NO (g)+02 (g) 2NO2 (g) AH=-114.2 k the enthalpy of the reaction of the nitrogen to produce nitric oxide 2NO (g) N2 (g)+02 (g) KJ. is 90.3 180.6 -180.6 47.8 47.8
Given: NO (g) + O2 (g) → 2 NO2 (g) ΔΗ = -114.2 kCalculate AH for this equation: NO2 (g)→½NO (g) + ½O2 (g)
[tot] 2NO2(g) + V2O2(g) - N,05(s) ΔΗ(tot) = [1] NOS(S) + 2NO(g) + (3/2002(g). ΔΗ, = 223.7 kg [2] NO(g) + V2O2(g) + NO2(g) ΔΗ, = = -57.1 kJ [tot] =X[1] [2]: ΔΗ(tot) = _XΔΗ, _XΔΗ, = k]
2NO(g)02(g)2NO2(g) AH° =-114.2 kJ and AS° =-146.5 J/K The equilibrium constant for this reaction at 321.0 K is Assume that AH° and AS° are independent of temperature
please answer all parts neatly thank you Given the thermochemical equation: N219) + 3H2(g) + 2NH3 (9) AH° = -92 at 298 K Is this reaction spontaneous or nonspontaneous ? Show Two ways Calculate the internal energy of the reaction.