a)
b)
OR,
OR,
For THE REVERSE REACTION THE VALUE OF
hence, for 18 mol it will be = -1102*18 = -19836 kj
5) N2(g) + O2(g) 2 NO(g) ΔΗ' 180.7 kJ ; AS°-24.7 J/K 25°C (a)Calculate the standard...
4) (a) Use the standard entropy values (AS") in the Appendix to solve for ?5° of each reaction at 25°C. (b) Solve for AG° ron for both reactions as well using the standard free energy values. (AG) 2H20(liquid)2H2(g) + O2(g) Al2O3(s) 3 H2(g) 2 Al(s)3 H20(g) 5) AH° 180.7 kJ; AS 24.7 JIK 25°C N2(8) O2(g)-2 NO(g) (a)Calculate the standard free-energy change for the reaction at 25°C. (b) Calculate ?G at 500°C using the ?G° value calculated from part a.
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 N2O(g) 2 N2(g) + O2(g)
H = -163.2 kJ
Use Hess's law to calculate H for the reaction below.
N2O(g) + NO2(g) 3 NO(g)
H =_______ 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
Thermochemical equations 5. Given 2NO → N2 + O2 ∆H= -180.7 determine the enthalpy of the reverse reaction? Is the reverse reaction endothermic or exothermic? 6. Given H2 + F2 → 2HF ∆H= -537 kJ a) How much heat is required to react 9.5 g F2 with H2? b) What mass of H2 is needed to react with F2 with -294 kJ of energy? Hess Law State Hess’s Law 8. Use the standard reaction enthalpies given below to determine ΔH°...
Calculate the standard free energy change at 25°C for the reaction 2 NO(g) + O2(g) → 2 NO2(g). Species ΔH°f, kJ/mol S°, J/(K · mol) NO (g) 91.3 210.7 O2 (g) 0.0 205.0 NO2 (g) 33.2 240.0 A) -157.8 kJ B) -532.6 kJ C) -72.6 kJ D) -4.7 kJ
If there is formation of NO(g) from N. (g) and 0,(g) at 298 K, calculate the standard free energy. The reaction is as follow: N,(g) + O2(g) → 2 NO(g) given that AH° = 180.7 kJ and ASⓇ = 24.7 J/K. Is the reaction spontaneous under these circumstances? A. Write the chemical reaction in which glucose is completely oxidized to CO, and H,O, and nitrate is completely reduced to N, B. What is the Gibbs free energy change and cell...
For the reaction N2(g) + O2(g) –> 2 NO(g) AG° = 172.2 kJ and AS° = 24.9 J/K at 339 K and 1 atm. favored under This reaction is (reactant, product) standard conditions at 339 K. The standard enthalpy change for the reaction of 2.47 moles of N2(g) at this temperature would be kJ. Submit Answer Retry Entire Group 9 more group attempts remaining
Consider the reaction: 12(e) + Cl2(8) 21CI(g) Using standard thermodynamic data at 298K, calculate the free energy change when 2.200 moles of 12(g) react at standard conditions. AG" KJ rea ex rea
For the reaction Fe(s) + 2HCI(aq)FeCl2(s) + H2(g) ΔΗο--7.4 kJ and ΔS°-107.9 J/K The standard free energy change for the reaction of 2.11 moles of Fe(s) at 278 K, 1 atm would be -37.4kJ This reaction is (reactant, product) -78.9 favored under standard conditions at 278 K Assume that Δ Ho and Δ are independent of temperature. For the reaction N2(g) + O2(g)2 NO(g) Δσ 172.7 kJ and ΔS°-24.9 J/K at 318 K and 1 atm. This reaction is (reactant,...
1. Thermodynamic data at 298 K. So (J/K) AHOf (kJ/mol) 205 0 O2 (g) 239 142.7 O3 (g) a) Calculate the standard entropy change for the production of ozone from oxygen at 298 K. Is this an increase or decrease in randomness? Explain briefly. -> 203 (g) 302 (g) b) Calculate the standard free energy change for this reaction. Is this reaction spontaneous under standard conditions? c) Calculate the AG° of formation for ozone.