Given the following equation,
N2O(g)+NO2(g) ---> 3NO(g) deltaG° rxn=-23.0 kj
Calculating deltaG° rxn for the following reaction.
18 NO(g) ---> 6N2O(g)+6NO2(g)
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Given the following equation, N2O(g)+NO2(g) ---> 3NO(g) deltaG° rxn=-23.0 kj Calculating deltaG° rxn for the following...
Given the following equation, N2O(g) + NO2(g) → 3 NO(g) ΔG°rxn = -23.0 kJ Calculate ΔG°rxn for the following reaction. 18 NO(g) → 6 N2O(g) + 6 NO2(g) -3.83 kJ -23.0 kJ 138 kJ -138 kJ 23.0 kJ
Given the following equation, N2O(g) + NO2(g) → 3 NO(g) ΔG°rxn = -23.0 kJ Calculate ΔG°rxn for the following reaction. 18 NO(g) → 6 N2O(g) + 6 NO2(g) -3.83 kJ -138 kJ 23.0 kJ -23.0 kJ 138 kJ
Given the following equation, N2O(g) + NO2(g) → 3 NO(g) AG°/x = -23.0 kJ Calculate AGºrxn for the following reaction. CHO COURO 3 NO(g) + N2O(g) + NO2(g) 153 ou te ato O bbou n esto bancabies A) -23.0 kJSOU nude au CODE B) 69.0 kJ e je bom su se 159 Hou e ab C) -69.0 kJ D) -7.67 kJ ost adapun E) 23.0 kj
Question 14 Given the following equation, 0/1 point N2O(g) + NO2 + 3 NO() AG --23.0k) Calculate AG xn for the following reaction. 21 NO) - 7 N206) 7 NO2 x-161 23.0 kJ 161 kJ -23.0 kJ -3.29
Find the value of the equilibrium constant, Kp, for the following reaction N2O(g) + NO2(g) → 3NO(g) at 900 K given the following data: N2O(g): AGfº=149.2 kJ/mol; NO2(g): AGfº=89.4 kJ/mol; NO(g): AGfº=79.0 kJ/mol. 0.192 1.21 1.00 0.826 O 1.43
Question 23 15 pts Consider the following reaction: N2O(g) + NO2(g) 3NO(g) AH = 155.7 kJ In which direction will the equilibrium be shifted by the following changes? 1. Adding N20 (Select] 2. Removing some N20 (Select] 3. Adding a catalyst (Select] 4. Adding NO [Select] 5. Increasing the temperature of the reaction mixture [ Select) 6. Decreasing the volume of the reaction vessel [Select] Question 24 10 pts A reaction vessel is charged with HI, which partially decomposes to...
8) The rate law for the following reaction N2O(g) + NO2(g) → 3NO(g) is Rate = k [N2O][NO2]2. Fill in the blank in the table below. Experiment [N2O], M [NO2], M Initial Rate, MS-1 1 0.100 0.100 2.0x10-3 2 0.300 0.100 6.0x10-3 3 0.100 0.200 ? a) 2.0x10−3 Ms−1 b) 4.0x10−3 Ms−1 c) 8.0x10−3 Ms−1 d) 6.0x10-3 Ms-1 e) 1.0x10−2 Ms−1
Using the Rxs below determine the value of AG° (in kJ) for this reaction. Rx: N2O(g) + NO2(g) → 3NO(g) + Rx1: 2NO(g) + O2(g) 2NO2(g) AG°= -71.2 kJ Rx2: N2(g) + O2(g) + 2NO(g) AG° = + 175.2 kJ Rx3: 2N2(e) + O2(g) 2N2O(g) AG° = + 207.4 kJ
3. Calculate AH for the reaction Ato AL120103 N2O(g) + NO2(g) → 3 NO(g) from the following enthalpies of reaction: NO(g) + O2(g) + NO2() N2O(g) + N2O) + O2(8) 1 N2(g) + O2(g) → NO(g) AH = -56.6 kJ AH = -81.6 kJ AH = +90.4 k]
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