Question

Use the set of three reactions shown below to answer the questions that follow.

2NO(g) + O2(g) → 2NO2(g) ΔH = -116 kJ
2N2(g) + 5O2(g) + 2H2O(l) → 4HNO3(aq) ΔH = -256 kJ

N2(g) + O2(g) → 2NO(g) ΔH = +183 kJ

a. If 30.2 g of NO g is reacted with excess oxygen, how much heat energy is produced?

b. What mass of liquid water will be consumed during the production of 31000 J of energy assuming that there is excess nitrogen and oxygen?

c. Determine the heat of reaction in kJ for the reaction below.

3NO2(g) + H2O(l) → 2HNO3(aq) + NO(g) ΔH

Answer 1

2 a) molen og No - mam 30.2 = 1:007 A molar man 30 2 NO + O 2NO, ON= - 116 KJ Imole no producen= -116 KG Imole No will produce = -116 1.007 mole No will produce 116 x 1.007 -58.41 Kg or -56.41K5 b) 2 mole of Ho will poodne= -256 kg or -256000 J 310005 in produced by 2 x 31000 - 0.2422 256000 mont of H₂ O= 0.2422 X 18 = 4.36 gramy c) 2 No e 02 2002 An= -116 KTM Reverse & de multibly by 3 multiply by z 3N02 Not 3 02 on=-3x (116) = 174ks to 2N2 +502 +240 4HNO3 Dno = -256 kg lolot multiply by £ Not O2 + H₂O 2HNO, on=-256 = -126 ks Ng + O2 2 No a DH= 183 renexe the equation No - N2 +02 on = -183 KT Sodd all of the equations 3N0g + H₂O 211NO₃ + No on = 174-1 (-120) + (-183) = -137kg

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