Calculate the enthalpy of change for the reactions. NO (g) + O(g) --> NO 2 (g) f

Question

Calculate the enthalpy of change for the reactions. NO (g) + O(g) --> NO2 (g) from the following data: NO (g) + O3 (g) --> NO2 (g) +O2(g)         H= -198.9 kJ O3 (g) --> 1.5 O2(g)                                  H= -142.3 kJ O2 (g) --> 2O(g)                                      H = 495.0 kJ Calculate the enthalpy of change for the reactions. NO (g) + O(g) --> NO2 (g) from the following data: NO (g) + O3 (g) --> NO2 (g) +O2(g)         H= -198.9 kJ O3 (g) --> 1.5 O2(g)                                  H= -142.3 kJ O2 (g) --> 2O(g)                                      H = 495.0 kJ

Explanation / Answer

NO (g) + O(g) --> NO2 (g) from the following data: NO (g) + O3 (g) --> NO2 (g) +O2(g)         H= -198.9 kJ O3 (g) --> 1.5 O2(g)                                  H= -142.3 kJ O2 (g) --> 2O(g)                                      H = 495.0 kJ

so in order to get the answer
er start with
NO (g) + O3 (g) --> NO2 (g) +O2(g)         H= -198.9 kJ
then we need to change the O3
O3 (g) --> 1.5 O2(g)                  H = -142.3 kJ
with this you get
NO (g) --> NO2 (g) + 2.5O2(g)
now to get rid of the 2.5 o2
we do
O2 (g) --> 2O(g)                                      H = 495.0 kJ so is all a matter of adding them
-198.9-142.3+495=153.8
NO (g) + O3 (g) --> NO2 (g) +O2(g)         H= -198.9 kJ
then we need to change the O3
O3 (g) --> 1.5 O2(g)                  H = -142.3 kJ
with this you get
NO (g) --> NO2 (g) + 2.5O2(g)
now to get rid of the 2.5 o2
we do
O2 (g) --> 2O(g)                                      H = 495.0 kJ

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