Determine the equilibrium constant Kp at 25°C for the reaction: (AG rxn=-69.7 kJ/mol) 00000 2.60 13.4 6.07 x 10-13 8.28 x 10-2 1.65 x 1012 2NO(g) + O₂(g) 2NO₂(g)

ces Large quantities of hydrogen are needed for the synthesis of ammonia. One preparation of hydrogen involves the reaction between carbon monoxide and steam at 3.00 × 102°C in the presence of a copper-zinc catalyst: CO(g) + H₂O(g) CO₂(g) + H₂(g) Using the standard data in the table, calculate the equilibrium constant (Kp) for the reaction at 3.00 × 102°C and the temperature at which the reaction favors the formation of CO and H₂O Species ΔΗ (kJ/mol) s f CO(g) -110.5 H₂O(g) -241.8 CO₂(g) -393.5 H₂(g) Kp = T= 0 K S¯ (J/mol·K) 197.7 188.8 213.8 130.7

The equilibrium constant, Kp, for the following reaction is 6at 698 K.H2(g) + I2(g) 2HI(g)If ΔH° for this reaction is -10.4 kJ, what is the value of Kp at 603 K?Kp =

7. Calculate A,G° for the reaction below at 25.0 °C CHA(g) + H20(g) →3 H2(g) + CO(g) given AG° [CH(g)] =-50.8 kJ/mol, AG° [H2O(g)] =-228.6 kJ/mol, AG° [H2(g)] = 0.0 kJ/mol, and AG° [CO(g)] = -137.2 kJ/mol. a. -416.3 kJ/mol-rxh b. -142.2 kJ/mol-rxn +142.2 kJ/mol-rxn %3D C. d. +315.0 kJ/mol-rxn +416.3 kJ/mol-rxn e.

Calculate AG°ran for the following reaction of white phosphorous with HCl. 2P (s) + 10HC1 (g)→ 2PCI5 (g) + 5H2 (g) AGʻfof P(s) = 0 KJ/mol AG†of HCl (g) = -95.3 KJ/mol AG°fof H2 (g) = 0 KJ/mol AGʻfof PCI5(s) = -305.0 KJ/mol

Consider the following equilibrium: N₂O4 (g) → 2NO₂ (g) AG = 5.4 kJ Now suppose a reaction vessel is filled with 0.399 atm of dinitrogen tetroxide (N₂O4) at 588. °C. Answer the following questions about this system: Under these conditions, will the pressure of N₂O4 tend to rise or fall? Is it possible to reverse this tendency by adding NO₂? In other words, if you said the pressure of N₂O4 will tend to rise, can that be changed to a tendency to fall by adding NO₂? Similarly, if you said the pressure of N₂O4 will tend to fall, can that be changed to a tendency to rise by adding NO₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of NO₂ needed to reverse it. Round your answer to 2 significant digits. O O rise fall yes no atm x10 X 5

Sulfur trioxide decomposes at high temperature in a sealed container.      2SO3 (g)   ==   2SO2(g)  +  O2(g) at  1000 K.  The SO3(g)  concentration that placed in  the container   is  2.4 x 10-3 M.  Calculate the value  of Kc    and Kp  at 1000K

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Calculate the Kp.

Consider the following reaction at 25 °C: 3 NiO(s) + 2 NH,(g) → 3 Ni(s) + N,(g) + 3 H,O(g) If AG° = -18.1 kJ/mol, determine the value of the equilibrium | %3D constant at 25 °C. 3 4 C 7 8. 9. +/- x 100 2. 5