Using the reactions below, determine the ∆Hº for 2 N2(g) + 5 O2(g) --> 2 N2O5(g)
N2(g) + 3 O2(g) + H2(g) --> 2 HNO3(aq) ∆Hº = -415 kJ/mol
N2O5(g) + H2O(l) --> 2 HNO3(aq) ∆Hº = -140 kJ/mol
2 H2(g) + O2(g) --> 2 H2O(l) ∆Hº = -572 kJ/mol
Ans :
The desired reaction can be obtained by adding :
= (double of reaction 1) + (double of reverse reaction 2 ) + (reverse of reaction 3)
So using Hess's law , the enthalpy change of the desired reaction will be given as :
= 2(-415) + 2(140) + 572
= 22 KJ/mol
Using the reactions below, determine the ∆Hº for 2 N2(g) + 5 O2(g) --> 2 N2O5(g)...
Consider the following data. 2 H2(g) + O2(g) 2 H2O(l) ΔH = -571.7 kJ N2O5(g) + H2O(l) 2 HNO3(l) ΔH = -92.0 kJ N2(g) + 3 O2(g) + H2(g) 2 HNO3O(l) ΔH = -348.2 kJ Use Hess's law to calculate ΔH for the reaction below. 2 N2O5(g) 2 N2(g) + 5 O2(g) ΔH = _____kJ
72. Determine AHº for this reaction from the data below. N2H4(1) + 2 H2O2(1) -→ N2(g) + 4H2O(1) N2H4(1) + O2(g) →→ N2(g) + 2 H2O(1) A Hº = -622.2 kJ mol-1 H2(g) + + O2(g) →→ H2O(1) A Hº = -285.8 kJ mol-1 H2(g) + O2(g) —> H2O2(1) A,Hº = -187.8 kJ mol-1
Given the following equations and Ho values given below, determine the heat of reaction at 298 K for the reaction: 2 N2(g) + 5 O2(g) 2 N2O5(g) 2 H2(g) + O2(g) 2 H2O(l) Ho/kJ = -571.6 N2O5(g) + H2O(l) 2 HNO3(l) Ho/kJ = -73.7 N2(g) + 3 O2(g) + H2(g) 2 HNO3(l) Ho/kJ = -348.2
5. Given the following data: (2 H2 (g) + O2 (g) → 2 H2O (1) ro in each AH° = -571.6 kJ N20s (g) + H2O (1) 2 HNO3 (1) AH° = -76.6 kJ N2 (g) + 3 O2 (g) + H2 (g) → 2 HNO3 (1) AH° = -348.2 kJ a. Calculate the AHⓇ for the reaction: 2 N2 (g) + 5 O2 (g) → 2 N2O5 (g)
Calculate the standard enthalpy of formation of liquid water
(H2O) using the following thermochemical
information:
2 HNO3(l)
N2O5(g) +
H2O(l)
H = +92.0 kJ
2 N2(g) + 5
O2(g) 2 N2O5(g)
H = +59.3 kJ
N2(g) + 3
O2(g) + H2(g) 2 HNO3(l)
H = -348.2 kJ
Calculate the Delta H formation of N2O5 (g) given the below reactions: 2NO (g) + O2 (g) -> 2NO2 (g), ΔHrxn = -114.1 kJ/mol 4NO2(g) + O2 (g) -> 2N2O5 (g), ΔHrxn = -110.2 kJ/mol N2 (g) + O2 (g) -> 2 NO (g), ΔHrxn = +180.5 kJ/mol
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
Determine ΔrH° for the following reaction, 2 NH3(g) + 5/2 O2(g) → 2 NO(g) + 3 H2O(g) given the thermochemical equations below. N2(g) + O2(g) → 2 NO(g) ΔrH° = +180.8 kJ/mol-rxn N2(g) + 3 H2(g) → 2 NH3(g) ΔrH° = –91.8 kJ/mol-rxn2 2H2(g) + O2(g) → 2 H2O(g) ΔrH° = –483.6 kJ/mol-rxn a. –1178.2 kJ/mol-rxn b. –452.8 kJ/mol-rxn c. –394.6 kJ/mol-rxn d. –211.0 kJ/mol-rxn e. +1178.2 kJ/mol-rxn
Calculate ΔG0 for the following reactions at 25oC. (a) N2(g) + O2(g) → 2NO(g) ΔG0 = kJ/mol (b) H2O(l) → H2O(g) ΔG0 = kJ/mol (c) 2C2H2(g) + 5O2(g) → 4CO2(g) + 2H2O(l) ΔG0 = kJ/mol
For the reaction C2H4(8) + Cl2(g) — C2H4C12(1), determine A,Hº, given that 4 HCl(g) + O2(g) — 2012(g) + 2 H2O(1) AH° = –202.4 kJ mol-1 2 HCl(g) + C2H4(8) + + O2(g) — C2H4Cl2(1) + H2O(1) ArHº = -318.7 kJ mol-1