N2(g) + O2(g) = 2 NO(g). ∆H° = 183 KJ
Reverse the equation
2 NO(g) = N2(g) + O2(g). ∆H° = -183 KJ i
1/2 N2(g) + O2(g) = NO2(g). ∆H° = 33 kJ
Multiply by 2
N2(g) + 2O2(g) = 2 NO2(g). ∆H° = 2*33 = 66 Kj. ii
Add equation i and ii
2 NO(g) + O2(g) = 2 NO2(g)
∆H° = -183 + 66 = -117 KJ
Option E
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What is AHºrxn for the following reaction based on the standard reaction enthalpies given below? AHºrn...
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Determining deltaHrxn using standard reaction
enthalpies.
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Use the standard reaction enthalpies given below and Hess's Law to determine AH°rxn for the following reaction: Input answer in kJ rounded to the ones place with the correct sign. X4(g) + 10 Y2(g) →4XY5(s) AHørxn = ? Given: XY5(s) → XY3(g) + Y2(g) AHºrxn=-157 kJ X4(g) + 6 Y2(g) →4 XY3(g) AH°rxn = 1,363 kJ