1) 2NH3 ----> N2 + 3H2 , Delta G° = +33.3 KJ
A) Since, Delta G° is positive thus reaction is non spontaneous.
B) Delta S is positive for reaction as product side has more gaseous moles than reactants moles.
C) Reaction is endothermic because Delta H is positive as per below;
Delta G° + T * Delta S = Delta H
Positive + T * positive = positive
2) N2 + 3H2 ---> 2NH3
A) Delta H(rxn) = 2*Delta H(NH3) - 3*Delta H(H2) - Delta H(N2)
Delta H(rxn) = 2*(-46.11) - 3*(0) - 0
Delta H(rxn) = -92.22 KJ/mol = -92220 J ...Answer
Similarly,
Delta S(rxn) = 2*(192.45) - 3*(130.684) - (191.61)
Delta S(rxn) = -198.762 J/K ....Answer
B) Delta G = Delta H - T * Delta S
Delta G = -92220 - 400 * (-198.762)
Delta G = -12715.2 J = -12.72 KJ/mol ....Answer
C) Since, Delta G is negative. Reaction is spontaneous.
D) Delta G = - R * T * ln Kc
-12715.2 = - 8.314 * 298 * ln Kc
Kc = 169.38 ....Answer
E) Delta H = T * Delta S
-92220 = T * (-198.762)
T = 463.973 K ....Answer
Let me know if any doubts/answer is not matching.
1. Consider the reaction: 2NH3(g) → N2(g) + 3 H2 (8) AG = +33.3 kJ a....
8. (3 points) Consider the following reaction: N2 (g) +3H2 (g) 2NH3 (g). Find the desired values given the following conditions: PNH3 2.00 atm, PN2 2.00 atm, and PH2 -2.50 atm. The AGo -33.3 kJ/mol at 25 °C. Calculate the Q value for these conditions. a. b. Calculate the AG value for these conditions. c. Is the reactions more or less spontaneous under these conditions compared to the standard conditions? How do you know?
AGº is -32.7 kJ/mol of N2 for the reaction N2 (g) + 3H2 (g) = 2NH3(g) This calculation was for the reaction under standard conditions—that is, with all gases present at a partial pressure of 1 atm and a temperature of 25°C. Calculate AG for the same reaction under the following nonstandard conditions: . PN2 = 2.00 atm, PH2 = 7.00 atm, PNH3 = 0.021 atm, . and T = 100°C.
In the Haber process, ammonia is synthesized from nitrogen and hydrogen: N2(g) + 3H2(g) → 2NH3(g) ΔG° at 298 K for this reaction is -33.3 kJ/mol. The value of ΔG at 298 K for a reaction mixture that consists of 1.9 atm N2, 1.6 atm H2, and 0.65 atm NH3 is ________. -3.86 × 103 -1.8 -7.25 × 103 -104.5 -40.5
15. The standard Gibbs free energy change (AG%) for the Haber reaction at 298K is -2.83 kJ/mol N2(g) + 3H2(g) + 2NH3(g) If the reaction begins with 2.55 atm N2(g) 0.115 atm Hz(g) and 0.488 atm NH3(9) at 298K what is the free energy change (AG) for the reaction under these conditions AND will the reaction be spontaneous under these conditions? (10 points) 16. For the following reactions, predict whether they will tend to be spontaneous at either high or...
For the reaction CO2(g) + H2(9)—-CO(g) +H30(9) AH° = 41.2 kJ and A Sº = 42.1 JK The equilibrium constant for this reaction at 252.0 K is Assume that AH and AS are independent of temperature. For the reaction N2(g) + 3H2(g) 2NH3(g) AH° = -92.2 kJ and AS™ = -198.7 J/K The equilibrium constant for this reaction at 347.0 K is Assume that AHⓇ and AS are independent of temperature.
Consider the reaction: N2(g) + 3H2(g) <---> 2NH3(g) The Gibbs free energy of formation ((delta)Gfo) for ammonia is -16.5 kJ/mol and the reaction is exothermic. Calculate the (delta)Gorxn and the equilibrium constant for the reaction and clearly state whether K increases or decreases with temperature.
1. Calculate AH° and AG', using data in Appendix C. Determine whether each reaction is endothermic or exothermic, and spontaneous or nonspontaneous. a) 2PbO(s) + N2(g) → 2Pb(s) + 2NO(g) b) CS2(1) + 2H20(1) - CO2(g) + 2H,S(9)
For the reaction N2(g) + 3H2(g) = 2 NH3(g), what is AG (in kJ) at 298 K when the pressures of the gases are: P(N2) = .13 atm P(H2) = 6.2 x 10-5 atm P(NH3) = 1.8 atm? +1.73 +47.0 0 -33.0 0-113 0 -2.49
10. The value of AGº for the Haber reaction, 3H2(g) + N2(g) → 2NH3(g), at 25°C is -32.3 kJ mor! Answer the following: a) Determine the value of Keq for the reaction at 25°C (4 points) b) The value of AH° is-92.2 kJ mor' and the value of AS is -201 J mor' K'Assuming the values of AH° and Asº do not change with temperature, determine agº for the reaction at 475°C. (4 points) c) Determine the value of Key...
For the reaction N2(g) + 3 H2(g) = 2 NH3(g), what is AG (in kJ) at 298 K when the pressures of the gases are: P(N2) .13 atm P(H2) = 6.2 x 10-5 atm P(NH3) = 1.8 atm? O +47.0 O-113 O-2.49 0 -33.0 O +1.73