9.
Given for,
4NO2 + O2 --> 2N2O5 dHb = -110.2 kJ
Divide this equation by 2, and invert the reaction,
fo reverse reaction,
N2O5 <==> 2NO2 + 1/2O2
dH = 110.2/2 = +55.1 kJ
11. moles of C = 49.97/12 = 4.16 mol
moles of H = 10.51/1 = 10.51 mol
moles of F = 39.52/19 = 2.08 mol
divide by smallest number
C = 4.16/2.08 = 2
H = 10.51/2.08 = 5
F = 2.08/2.08 = 1
Empirical formula = C2H5F
Given: 4 NO_2(g) + O_2(g) rightarrow 2 N_2O_5(g) delta H degree = -110.2 kJ find delta...
Given: 4 NO_2(g) + O_2 (g) rightarrow 2N_2O_5(g) DeltaH degree = - 110.2 kJ find Delta Hdegree for N_2O_5(g) rightarrow 2 NO_2 (g) + 1/2 O_2(g) 55.1 kJ 220.4 kJ -55.1 kJ -220.4 kJ
Using the following reactions: N_2(g) + O_2(g) rightarrow 2 NO(g) Delta H = 181 kJ times 2 NO(g) + O_2 rightarrow 2 NO_2(g) Delta H = -113 kJ times 2 N_2O(g) rightarrow 2 N_2(g) + O_2(g) Delta H = -163 kJ times Determine the enthalpy change for the reaction: N_2O(g) + NO_2(g) rightarrow 3 NO(g) Delta H =
For the reaction N_2(g) + 3 H_2(g) rightarrow 2 NH_3(g) Delta G degree = -23.6 kJ and Delta S degree = -198.7 J/K at 345 K and 1 atm. This reaction is (reactant, product) favored under standard conditions at 345 K. The standard enthalpy change for the reaction of 2.30 moles of N_2(g) at this temperature would be kJ. For the reaction 2 H_2O_2(l) rightarrow 2 H_2O(l) + O_2(g) Delta G degree = -236.9 kJ and Delta H degree =...