Use the equation AS In(K) = R For K at two temperatures T₁ and T₂, the equation can be manipulated to give: K2 AHⓇ 1 1-K-AR (-) In = K₁ In -AHⓇ RT 3.25 x 10-² 8.94 In(8.94) - 5.62 = (5.80 × 10-5 mol/J)(AH°) -9.69 × 10¹ J/mol AH° = For K= 8.94 at T = 25°C: + = = AHⓇ 8.3145 J/K mol 298 K 1 (K-3K) 348 K AS 8.3145 AS = -307 J/K . mol We get the same value for AS using K = 3.25 × 10-² at T = 348 K. - 36.9 -(-9.69 × 10¹ J/mol) ASⓇ (8.3145 J/K-mol) (298 K) 8.3145 J/K - mol Estimate the temperature where K = 1.00 for this reaction. Temperature K

Ammonia (NH3) decomposes to form nitrogen gas and hydrogen gas with an enthalpy of 89.4kJ/mol. Aclosed container is charged with 6.0 atm ammonia and heated to 25.0°C. At equilibrium the pressure of H2 is3.60atm. a. Write the balanced reaction.

What is AG for the reaction l2(g) → 2 1(g) at 25.0 °C if K = 6.1 x 10-2²? (R = 8.314 J/mol.K)

Calculate AGO at 600. K for using the following data: AGO = H₂O(g) + 1/2O₂(g) → H₂O2(g) H₂(g) + O₂(g) → H₂O2(g) K = 1.8 × 10³7 at 600. K 2H2(g) + O₂(g) → 2H₂O(g) K = 2.3 × 106 at 600. K kJ/mol

8. Given: 2 HI (g) H2 (g) + 12 (g) AH < 0 This reaction is placed in a closed vessel and allowed to reach equilibrium. If H2 is removed, would the vessel feel cold or warm? Explain.

Consider the reaction: PbCl2(s) → Pb2*(aq) + 2 Cl (aq) AH° = 23.30 kJ/mol and AS° = -12.5 J/K-mol a) When solid PbCl2 is dissolved in water at 25°C, what are the concentrations of Pb2* and Cl at equilibrium? (Hint: Do your ICE chart and Law of Mass Action.) Concentration of Pb2+: mol/L and Concentration of Cl = mol/L (Do not use superscripts, subscripts, or carets. Write 1.2 x 10-3 as 1.2x10-3 or 1.2e-3.) b) At 25°C, This reaction is (reactant or product) favored. Justify your answer with the appropriate calculation on the separate sheet of paper. c) The Gibbs free energy at 25°C, when both the concentrations of the lead ion and chloride ion are 1.2 x 10-³M is kJ/mol. Show your calculations on the separate sheet of paper.

[Review Topics] [References] Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH° = -111 kJ/mol, and K. = 0.159 , at 723 K. N2 (g) + 3 H, (g)=2 NH3 (g) When 0.21 moles of NH, (g) are added to the equilibrium system at constant temperature: The value of K The value of Qe K. The reaction must O run in the forward direction to restablish cquilibrium. O run in the reverse direction to restablish coquilibrium. O remain the same. It is already at cquilibrium. The concentration of H, will Submit Answer Retry Entire Group 1 more group attempt remaining

Kk.239.

What is AGxn (in kJ) at 1932 K for the following reaction? 2POCI3(g) → 2PC13(g) + O₂(g) POCI3(g): AH = -592.7 kJ/mol and Sº = 324.6 J/K mol) PC13(g): AH = -287.0 kJ/mol and So = 311.7 J/K mol) O₂(g): AH = ? kJ/mol and Sº = 205.0 J/K mol)

Consider the reaction in the Haber process 3H2 (g) + N2 (g) → 2NH3 (g)where delta H° = -91.8 kJ/mol and delta S° = -197 J/(mol*K). What is the value of the equilibrium constant (K) at a temperature of 125°C?