Question

In: Chemistry

What is ΔG° at 298 K for the following reaction? HCN( g )+N H 3 (...

What is ΔG° at 298 K for the following reaction? HCN( g )+N H 3 ( g )→C H 4 ( g )+ N 2 ( g ) ;   ΔH°=−164.1kJ;    ΔS°=−17J/K   at   298 K?

Solutions

Expert Solution

We know the equation

G0 =H0 -TS0  

Now from given values

G0 = -164.1 kJ - 298 K ( -17 x 10-3 kJ/K) ................ make J to kJ for S0 values

= -164.1 kJ + 5.066 kJ

= -159.034 kJ

So

Answer is

-159.034 kJ

queen_honey_blossom answered 1 year ago
Next > < Previous

Related Solutions

Estimate ΔG°rxn for the following reaction at 407 K. HCN(g) + 2 H2(g) → CH3NH2(g) ΔH°=...
Estimate ΔG°rxn for the following reaction at 407 K. HCN(g) + 2 H2(g) → CH3NH2(g) ΔH°= -158.0 kJ; ΔS°= -219.9 J/K answer choices -68.5 kJ +247 kJ -247 kJ +68.5 kJ +61.9 kJ
Consider the reaction: 2 NO2(g) → N2O4(g) Calculate ΔG (in kJ/mol) at 298°K if the equilibrium...
Consider the reaction: 2 NO2(g) → N2O4(g) Calculate ΔG (in kJ/mol) at 298°K if the equilibrium partial pressures of NO2 and N2O4 are 1.337 atm and 0.657 atm, respectively.
Calculate ΔG for the following reaction at 1200 K and 3.29 × 10^-3 atm of Cl2(g)....
Calculate ΔG for the following reaction at 1200 K and 3.29 × 10^-3 atm of Cl2(g). 2AgCl(s) ⇄ 2Ag(s) + Cl2(g)   ΔG° = 220 kJ
Consider the following reaction occurring at 298 K: N2O(g)+NO2(g)⇌3NO(g) Part A Show that the reaction is...
Consider the following reaction occurring at 298 K: N2O(g)+NO2(g)⇌3NO(g) Part A Show that the reaction is not spontaneous under standard conditions by calculating ΔG∘rxn. Part B If a reaction mixture contains only N2O and NO2 at partial pressures of 1.0 atm each, the reaction will be spontaneous until some NO forms in the mixture. What maximum partial pressure of NO builds up before the reaction ceases to be spontaneous? Part C What temperature is required to make the reaction spontaneous...
Consider the following reaction at 298 K: 4Al(s) + 3O2(g) ==> 2Al2O3(s) Delta H= -3351.4 kJ/mol...
Consider the following reaction at 298 K: 4Al(s) + 3O2(g) ==> 2Al2O3(s) Delta H= -3351.4 kJ/mol Calculate: a. Delta Ssystem = _______J/mol*K b. Delta Ssurroundings = _______J/mol*K c. Delta S universe = _________J/mol*K
Consider the following reaction where Kc = 6.50×10-3 at 298 K 2 NOBr (g)-> 2 NO...
Consider the following reaction where Kc = 6.50×10-3 at 298 K 2 NOBr (g)-> 2 NO (g) + Br2 (g) A reaction mixture was found to contain 8.52×10-2 moles of NOBr (g), 2.31×10-2 moles of NO (g), and 4.58×10-2 moles of Br2 (g), in a 1.00 liter container. Indicate True (T) or False (F) for each of the following: 1. In order to reach equilibrium NOBr(g) must be consumed . 2. In order to reach equilibrium Kc must increase ....
Determine the equilibrium constant for the following reaction at 655 K. HCN(g) + 2 H2(g) →...
Determine the equilibrium constant for the following reaction at 655 K. HCN(g) + 2 H2(g) → CH3NH2(g) ΔH° = -158 kJ; ΔS°= -219.9 J/K. Determine the equilibrium constant for the following reaction at 655 K. HCN(g) + 2 H2(g) → CH3NH2(g) ΔH° = -158 kJ; ΔS°= -219.9 J/K A. 3.07 × 1011 B.13.0 C. 3.26 × 10-12 D. 3.99 × 1012 E. 2.51 × 10-13
Determine the equilibrium constant for the following reaction at 655 K. HCN(g) + 2 H2(g) ?...
Determine the equilibrium constant for the following reaction at 655 K. HCN(g) + 2 H2(g) ? CH3NH2(g); ?H
Determine the equilibrium constant for the following reaction at 655 K. HCN(g) + 2 H2(g) →...
Determine the equilibrium constant for the following reaction at 655 K. HCN(g) + 2 H2(g) → CH3NH2(g) ΔH° = -158 kJ; ΔS°= -219.9 J/K
A reaction has and △H°298 = 151 kJ/mol and △S°298 = 286 J /mol K at...
A reaction has and △H°298 = 151 kJ/mol and △S°298 = 286 J /mol K at 298 K. Calculate △G in kJ/mol.
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT