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Hydrogen cyanide is produced industrially from ammonia and methane at 1000ºC utilizing a platinum-rhodium catalyst by...

Hydrogen cyanide is produced industrially from ammonia and methane at 1000ºC utilizing a platinum-rhodium catalyst by the following reaction: 2 NH3(g) + 3 O2(g) + 2 CH4(g) → 2 HCN(g) + 6 H2O(g)

a) Calculate ΔGº, ΔHº, and ΔSº for this reaction at 25.00ºC. ΔGº ΔHº ΔSº

b) Why is this reaction performed at such a high temperature (1000ºC)? _____________________________________________________________________________ _____________________________________________________________________________

c) Calculate the value of the equilibrium constant for this reaction at 25.00ºC. ___________________________________

d) What is the value of ΔG at 25.00ºC if each of the gases is at a partial pressure of 0.25 atm.? ___________________________________

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Answer #1

2x 135-1 ナ6x-241. -(2x -4S- t2xHW o6 241 2X 201 f + 6x Iff, f)-( 2x112f ナ3x205. + 2X 186:3 AS - IS364 13チ3, f 08 = 162.6피K

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