The Reaction below has an equilibrium constant of Kp = 2.26 x 104 at 298 K. For Reactions a, b and c, PREDICT whether REACTANTS or PRODUCTS will be favored at equilibrium. CO(g) + 2 H₂(g) = CH3OH(g) a. CH₂OH(g) = CO(g) + 2 H₂(g) b. CO(g) + H₂(g) = CH3OH(8) c. 2 CH3OH(g) = 2 CO(g) + 4H₂(g) Reaction c Reaction a Reaction b Favors REACTANTS Favors PRODUCTS

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Consider the following equilibrium: N2O4(g) 2NO2 (g) AG = 5.4 kJ Now suppose a reaction vessel is filled with 2.78 atm of dinitrogen tetroxide (N204) at 710. °C. Answer the following questions about this system: rise x10 fall 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. yes no ☐ atm X S

Consider the following equilibrium: 2NOC1 (g) → 2NO(g) + Cl₂ (g) AG = 41. kJ Now suppose a reaction vessel is filled with 8.30 atm of nitrosyl chloride (NOC1) and 5.80 atm of chlorine (C1₂) at 878. °C. Answer the following questions about this system: Under these conditions, will the pressure of Cl₂ tend to rise or fall? Is it possible to reverse this tendency by adding NO? In other words, if you said the pressure of Cl₂ will tend to rise, can that be changed to a tendency to fall by adding NO? Similarly, if you said the pressure of Cl₂ 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. Round your answer to 2 significant digits. оо rise fall yes no 0 atm x10 X Ś

Carbon monoxide reacts with water according to the following equilibrium reaction: CO (g) H2O (g) CO2 (g) + H2 (g) For this reaction, K = 0.810 at a temperature of 1000.°C. Calculate the value of AG for this reaction at 1000.ºC. %3D

You are given the following:   H2 (g) + Br2 (g) 2 HBr (g) Kp = 7.9 x 1011                            H2 (g) 2 H (g) Kp = 4.8 x 10-41                                         Br2 (g) 2 Br (g) Kp = 2.2 x 10-15 What is Kp for the reaction shown below?                                H (g) +  Br (g)   HBr (g) Kp = ?

3. Phosphoryl chloride, POCI3(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 POCI3(8)and NO(g) according to the following equation: PCI3 (g) + NO2 (g) = POCI3 (g) + NO (g) The Keg for this reaction at 800 K is 6.90. If 1.25 mol PCI3 (g) and 1.94 mol NO2 (g) are placed into a 2.0 L container, what is the concentration of each gas at equilibrium at 800 K? PCI3 (g) NO2 (g) POCI3 (g) NO(g) Keq = 6.90 + + E

Nitrogen dioxide reacts to form dinitrogen tetroxide as follows: 2 NO2 N₂04 (g) At 150 °C, Kp = 4.51. If one starts with 10.0 atm NO2 (g), what is the equilibrium pressure (in atm) of N₂O4 (g)?

Consider the following equilibrium: 2NH3(g) = N₂ (g) + 3H₂(g) 2 AG = 34. kJ Now suppose a reaction vessel is filled with 7.87 atm of ammonia (NH3) and 1.17 atm of hydrogen (H₂) at 448. °C. Answer the following questions about this system: Under these conditions, will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding N₂? In other words, if you said the pressure of NH3 will tend to rise, can that be changed to a tendency to fall by adding N₂? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding N₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of N₂ needed to reverse it. Round your answer to 2 significant digits. rise fall yes no atm x10 X 5

Consider the following equilibrium: N2(g) + 2O2(g)⇄2NO2 (g). If Kp = 0.0255 at 500.0 K, calculate Kc.