Question 1 1 Consider the following reaction: Ce2(g) + 2NO(g) = 2NOC{(g) 1.1 Determine the estimated value of the equilibrium constant for this reaction at 158 °C by making use of the following data: kj at 25°C mol Substance at 25°C 4,H° ()a \mol. K. Cl2(g) 221.3 NO(g) 210.8 90.29 NOC? (g) 261.7 51.71 1.2 Based on your final answer in question 1.1, is the reaction reactant- or product favoured at this temperature? Use a short sentence to explain your answer. 1.3 Calculate the value of A,G for this reaction at this temperature, if Cł2 , NO and NOC? are present at 0.600 atm, 0.700 atm and 0.500 atm, respectively.

MISSED THIS? Read Section 19.10 (Pages 881 - 884); Watch IWE 19.11. Use AG values from Appendix IIB to calculate the equilibrium constants at 25°C for each of the following reactions. - Part B Br₂(g) + Cl₂ (g) = 2BrCl(g) AG (BrCl(g)) = -1.0 kJ/mol Express your answer to two significant figures. ► View Available Hint(s) K = —| ΑΣΦ C ?

Phosphoryl chloride, POCl3(g), is used in the manufacturing of flame retardants. It is manufactured in an equilibrium process in which phosphorus trichloride reacts with nitrogen dioxide to form POCl3(g)and NO(g) according to the following equation: PCI3 (g) + NO₂ (g) POCI3 (g) + NO (g) + 228.93kJ At 298K, the equilibrium concentration of POCI3 was 0.68 mol/L, the concentration of NO was 0.72mol/L, the concentration of PC13 was 0.62 mol/L, and the concentration of NO₂ was 0.56 mol/L. a. 6.25 moles of POCI3 (g) is added to the 5.0 L reaction chamber. What is the new concentration of POCI 3 (g) when equilibrium is re-established? PCI 3 (g) NO2 (g) E' - C E + 11 POCI 3 (g) + NO(g)

6. Given the thermodynamic data below, what is the equilibrium constant Kea of the following popular science fair reaction at 25°C: H'(aq) + HCO3(aq) + CO2(g) + H₂O(g) Species AG% (kJ/mol) H* (aq) 0 HCOs aq) -587.1 CO2(g) -394.4 H₂O(g) -228.6 A. 7.1 x 10¹0 B. 2.0 x 106 C. 89 D. 1.0 E. 4.3 x 10-8 I

[Review Topics] [References] Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH=-108 kJ, and K. 77.5, at 600 K. CO(g) + C,(g) COCI,(g) When 0.22 moles of Cl,(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 cquilibrium. O remain the same. It is already at cquilibrium. The concentration of CO will Submit Answer Retry Entire Group 1 more group attempt remaining

Consider the following equilibrium: 2NO₂ (g) N₂O₂(g) AG=-5.4 kJ Now suppose a reaction vessel is filled with 0.316 atm of nitrogen dioxide (NO₂) at 708. "C. Answer the following questions about this system: Under these conditions, will the pressure of NO₂ tend to rise or fall? Is it possible to reverse this tendency by adding N₂O₂? In other words, if you said the pressure of NO₂ will tend to rise, can that be changed to a tendency to fall by adding N₂O? Similarly, if you said the pressure of NO₂ will tend to fall, can that be changed to a tendency to rise by adding N₂O? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂O₂ needed to reverse it. Round your answer to 2 significant digits. rise O fall O yes O no atm 0.8 X

O ENTROPY AND FREE ENERGY Using reaction free energy to predict equilibrium composition D 3/5 Consider the following equilibrium: 2NOC1 (g) - 2NO (g)+ Cl, (g) AG" =41. kJ Now suppose a reaction vessel is filled with 2.68 atm of nitrosyl chloride (NOCI) and 3.74 atm of chlorine (Cl,) at 227. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of Cl, tend to rise or fall? fall Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of Cl, will tend to rise, can that yes be changed to a tendency to fall by adding NO? Similarly, if you said the no pressure of Cl, will tend to fall, can that be changed to a tendency to rise by adding NO? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO needed to reverse it. | atm Round your answer to 2 significant digits. II

Determine the value of AG for the reaction at 309 K. Assume standard concentration 2NH;(g) = N,H,(g) + H, (g) Given AH (kJ/mol) S°J/{mol · K)) Substance NH3(3) -46.1 192.5 95.35 N2H4(g) H2(3) 238.5 0.0 130.6 O-87.0 kJ -182.5 kJ O -192.6 kJ O 87.0 kJ O 192.6 kJ

Use the data below to calculate the value of the equilibrium constant for the following reaction at 298 K. Please give your answer with 2 significant figures. 3 NO2(g) + H2O(e) → 2 HNO3(e) + NO(g) AfG [H2O(l)] = -237.2 kJ mol-1 ; AFG°[HNO3(e)] = -79.9 kJ mol-1 ; AfG [NO(g)] = 86.7 kJ mol-1; AfG°[NO2(g)] = 51.8kJ mol-1

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