a)
T = 298.15 K
deltaG = -16.5 KJ/mol
deltaG = -16500 J/mol
we have below equation to be used:
deltaG = -R*T*ln Kc
-16500 = - 8.314*298.15* ln(Kc)
ln Kc = 6.6564
Kc = 778
Answer: 778
b)
This reaction is 2 times of above reaction
So,
Kc2 = Kc1^2
= (778)^2
= 6.05*10^5
Answer: 6.05*10^5
5. Given ΔG =-16.5 kJ/mol for the reaction ½ N2 + 3/2 H2 → NH3, find...
Consider the Haber synthesis of gaseous NH3 (ΔH∘f = -46.1 kJ/mol; ΔG∘f = -16.5 kJ/mol): N2(g)+3H2(g)→2NH3(g) What are the equilibrium constants Kp and Kc for the reaction at 350 K ? You may assume that ΔH∘ and ΔS∘ are independent of temperature.
Info from ALEKS data lab: Gf[N2] = 0 kj/mol Gf[H2] = 0 kj/mol Gf[NH3] = -26.50 kj/mol A chemist fills a reaction vessel with 0.520 atm nitrogen (N2) gas, 7.66 atm hydrogen (H) gas, and 5.02 atm ammonia (NH3) gas at a temperature of 25.0°C. Under these conditions, calculate the reaction free energy AG for the following chemical reaction: N2(g) + 3H2(g) + 2NH3(g) Use the thermodynamic information in the ALEKS Data tab. Round your answer to the nearest kilojoule....
5. The following equilbrium partial pressures were measured at some temperature: NH3 N2 H2 0.240 atm 0.290 atm 0.330 atm Determine the value of the equilibrium constant at the temperature of the reaction for the following reaction. Your are given values to 3 significant figures, so make sure you answer to three significant figures to avoid rounding errors in WebAssign. N2 + 3H2 2NH3 K = In a different experiment at the same temperture, the equilibrium pressure of N2 was...
Consider the reaction: N2(g) + 3 H2(g) « 2 NH3(g) a. Write the expression for the equilibrium constant, K, for this reaction. b. An equilibrium misture of N2, H2, and NH3 at 300°C is analyzed, and it is found that: [N2] = 0.25 mol/L, [H2] = 0.15 mo/L, and [NH3] = 0.090 mol/L. Find K at 300°C for this reaction.
Find ΔrG for the following (in kJ mol-1) N2 (g) + 3 H2 (g) ⇌ 2 NH3 (g) The conditions for this reaction are: Temp: 298k P - NH3 = 0.95 bar P - H2 = 1.95 bar P - N2 = 1.25 bar NH3(g) ?H ∙(kJ mol-1) = -45.9 ?G ∙(kJ mol-1) = -16.4 S ∙(J K-1 mol-1)192.8 N2(g) ?H ∙(kJ mol-1) = 0 ?G ∙(kJ mol-1) = 0 S ∙(J K-1 mol-1)191.6 H2(g) ?H ∙(kJ mol-1) = 0...
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
For the following reaction at equilibrium with a given AHºrxn = -207 kJ/mol: N2(g) + 3H2(g) <=> 2NH3(g) What will be the response of the system at equilibrium if the temperature is decreased? More reactants will be formed. More products will be formed. There will be no change in the amount of products formed. There will be no change in the amount of reactants being consumed More reactants and products will be formed.
1. Consider the reaction: 2NH3(g) → N2(g) + 3 H2 (8) AG = +33.3 kJ a. Is this reaction spontaneous? Explain. b. Predict the sign of AS. Explain. C. Based on your answer to part b, is this reaction exothermic or endothermic? Explain. For the reaction N2(g) + 3H2(g) 2NH3 (8) a. Using values in Appendix Cin your book, calculate AHⓇ and AS. b. Assuming that AHºand ASº don't change with temperature, calculate the value for AG at 400K Is...
uton containing 110 5. Determine the equilibrium constant Kp at 25°C for the reaction N2(g) + 3H2(g) [AG°f (NH3(g)) = -16.6 kJ/mol]. (show your calculation steps) de 2NH3(g)
At equilibrium, there is 0.823 mol of NH3 present. Determine the number of mol of N2 and H2 that are present when the reaction is at equilibrium. At a certain temperature, 0.885 mol of N2, and 2.654 mol of H2 are placed in a container N2g) + 3H2 At equilibrium, there is 0.823 mol of NH3 present. Determine the number of mol of N2 and H2 that are present when the reaction is at equilibrium. Moles of N2 at equilibrium...