Consider the following reaction between oxides of nitrogen: NO_2(g) + N_2 O(g) r

Question

Consider the following reaction between oxides of nitrogen: NO_2(g) + N_2 O(g) rightarrow 3NO(g) Use data in Appendix C in the textbook to predict how AG degree for the reaction varies with increasing temperature. increases decreases Calculate delta G degree at 800 K, assuming that delta H and delta S degree do not change with temperature. Express your answer using two significant figures. delta G degree = kJ Under standard conditions is the reaction spontaneous at 800 K? yes no Calculate delta G degree at 1000 K. Is the reaction spontaneous under standard conditions at this temperature? yes

Explanation / Answer

B)

Ho(NO2) = 33.18 KJ/mol

Ho(N2O) = 82.05 KJ/mol

Ho(NO) = 90.2 KJ/mol

delta Ho = 3*Ho(NO) - Ho(NO2) - Ho(N2O)

= 3*90.2 - 33.18 - 82.05

= 155.37 KJ/mol

= 155370 J/mol

So(NO2) = 240.1 J/mol-K

So(N2O) = 219.9 J/mol-K

So(NO) = 210.7 J/mol-K

delta So = 3*So(NO) - So(NO2) - So(N2O)

= 3*210.7 - 240.1 - 219.9

= 172.1 J/mol-K

delta Go = delta Ho - T*delta So

= 155370 - 800*172.1

= 17690 J

= 17.6 KJ

D)

delta Go = delta Ho - T*delta So

= 155370 - 1000*172.1

= -16730 J

= -16.73 KJ

E)

yes

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