For any reaction
Standard enthalpy change of reaction = sum of heat of formation of products- sum of heat of formation of reactants
For the reaction 3NO2(g)+ H2O(l)----->2HNO3(aq)+ NO(g)
Standard enthalpy change= 2* heat of formation of HNO3 (aq)+ Heat of formation of NO- { 3* heat of formation of NO2+ heat of formation of H2O(l)
2*(-207)+91.3- {3*33.2+(-187.8}=-234.5 Kj/mole
1. Calculate ΔHnn for the following reaction. 3NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g) Given....
Calculate the ΔG°rxn using the following information. 2 HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l) ΔG°rxn = ? ΔH°f (kJ/mol) -207.0 91.3 33.2 -285.8 S°(J/mol∙K 146.0 210.8 240.1 70.0 -151 kJ +50.8 kJ -186 kJ +222 kJ -85.5 kJ
Calculate the ΔG°rxn at 298 K using the following information. 2 HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l) ΔG°rxn = ? ΔH°f (kJ/mol) -207.0 91.3 33.2 -285.8 S°(J/mol∙K 146.0 210.8 240.1 70.0
Calculate the DGorxn using the following information. 2 HNO3(aq) + NO(g) à 3 NO2(g) + H2O(l) DHof (kJ/mol) -207 91.3 33.2 -285.8 So (J/mol . K) 146 210.8 240.1 70.0
Consider the following chemical reaction. NH3(g) + 2 O2(g) → HNO3(aq) + H2O(l) Calculate the change in enthalpy (ΔH) for this reaction, using Hess' law and the enthalpy changes for the reactions given below. (1a) 4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(l); ΔH = −1166.0 kJ/mol (2a) 2 NO(g) + O2(g) → 2 NO2(g); ΔH = −116.2 kJ/mol (3a) 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g); ΔH = −137.3 kJ/mol
Calculate ΔG°(in kJ/mol) for the reaction NO2(g) + H2O(l) --> HNO3(l) + NO(g). (unbalanced) Question 7 Calculate AG°(in kJ/mol) for the reaction NO2(g) + H2O(0) --> HNO3(1) + NO(g). (unbalanced) Substance AGF(kj/mol) NO2(g) 51.8 NO(g) 86.7 HNO3(0) -79.9 H2O(l) -237.2 Write answer to two significant figures and correct sign.
only worth 1 point. 1. (6) 15.0 g of ice cubes at 0.0°C are combined with 150.g of liquid water at 70.0°C in a coffee cup calorimeter. Calculate the final temperature reached, assuming no heat loss or gain from the calorimeter. (Data: specific heat capacity of H2O(l). C4.18 1/8 'C) H2O(s) → H2O(1) AH = 6.02 kJ/mol) 2. (6) Calculate A s for the reaction: 5C(s) + 6H2(g) → CsHuz10 Use the following reactions and given AH's. CsHua(l) + 802()...
Calculate the ΔG°rxn using the following information. 2 HNO3(aq) + NO(g) → 3 NO2(g) + H2O(l) ΔG°rxn = ? ΔG°f (kJ/mol) -110.9 87.6 51.3 -237.1
For 3NO2(g)+H2O(l)→2HNO3(aq)+NO(g), the first part of the question asks me to find the mass of HNO3 made from 293 g of NO2 (found to be 267.55). How do i find the volume of NO gas formed in the reaction with those 293 grams? Air temp is 284.5K and pressure is 714/760atm
Calculate ΔG°(in kJ/mol) for the reaction NO2(g) + H2O(l) --> HNO3(l) + NO(g). ( unbalanced) Substance ΔGfo(kJ/mol) NO2(g) 51.8 NO(g) 86.7 HNO3(l) -79.9 H2O(l) -237.2 Write answer to two significant figures and correct sign.
Which is the anode in the following oxidation reduction reaction? 3NO2−(aq) + 2MnO4−(aq) +H2O(l) →3NO3−(aq) + 2MnO2(aq) +2OH−(aq) a) There is no anode in this reaction b) H2O(l) c) MnO4−(aq) d) NO2−(aq)