At -9.76 °C the concentration equilibrium constant K = 5.3 × 10 for a certain reaction. Here are some facts about the reaction: • If the reaction is run at constant pressure, the volume increases by 11.%. • If the reaction is run at constant pressure, 64.0 kJ/mol of heat are released. • The net change in moles of gases is - 1. Using these facts, can you calculate Kat 15. °C? If you said yes, then enter your answer at right. Round it to 2 significant digits. If you said no, can you at least decide whether K at 15. °C will be bigger or smaller than K at -9.76 °C? O Yes. O No. 0 Yes, and K will be bigger. Yes, and K will be smaller. No.

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.

For the reaction below, what is the effect of raising the temperature? 4A(g) + B(g) 3C(g) AH = - 405 kJ Equilibrium shifts to the right; the reaction makes more products. O The reaction makes more of both products and reactants, so equilibrium is unaffected O Equilibrium re-establishes Equilibrium shifts to the left; the reaction makes more reactants.

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.

Please answer ALL parts of the question and show your work. Consider this reaction: 2H2S(g) + 3O2(g)  <-----> 2H2O(g) + 2SO2(g)       H= -1036 kJ Predict whether the forward or reverse reaction will reestablish equilibrium is disturbed by (a) expanding the container (b) removing SO2 (c) rasing the temperature (d) water vapor is added

Consider the following equilibrium: N₂ (g) + 3H₂(g)2NH₂ (g) AG = -34. KJ 2 Now suppose a reaction vessel is filled with 3.70 atm of hydrogen (H₂) and 8.46 atm of ammonia (NH3) at 1099. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of H ₂ tend to rise or fall? x10 fall Is it possible to reverse this tendency by adding N₂? x Ś ? In other words, if you said the pressure of H₂ will tend to rise, can that be changed to a tendency to fall by adding N₂? Similarly, if you said the yes no pressure of H₂ will tend to fall, can that be changed to a tendency to rise 2 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. atm Round your answer to 2 significant digits. ● O

Consider the following system: 4 NH3(g) + 3 O2(g) -> 2 N2(g) + 6 H2O(l) AH = -1530.4 kJ (a) How will the amount of ammonia at equilibrium be affected by      (1) removing O2(g)?      (2) adding N,(g)?      (3) adding water?      (4) expanding the container at constant pressure?      (5) increasing the temperature? (b) Which of the above factors will increase the value of K? Which will decrease it?

Consider the system below at equilibrium at 200°C: 2C12 (g) + 2H20 (g) - 98.6KJ = 4HCI (g) + 02 (g) The change listed below would cause more reactants to form when equilibrium is re- established. Write A if true and B if false (Note: Answer is case sensitive) Decreasing the volume at constant temperature

9. What is the equilibrium constant for reaction below at 25 °C? (R=8.314 J/K-mol) 2 NO(g) + O2(g) 2 NO2(g) given AG° [NO(g)] =+86.6 kJ/mol and AG° [NO2(g)] =+51.2 kJ/mol. a. 3.9 x 10-13 b. 1.0 c. 2.6 x 1012 d. 1.6 x 106 е. 3.8 х 1028 of silver bromide is 5.4 x 10-13 at 298 K.

What is true about the following reaction at 25°C? H₂(g) + 2BrF(g) = 2HBr(g) + F₂(g) \Delta Hr\ deg = 115 kJ mol-¹ \Delta Sr\deg = 11.55 J mol-¹ K-¹ \Delta Gr\deg = 111 kJ mol-¹ i. The reaction is endothermic. ii. As the reaction proceeds heat is transferred from the surroundings to the system.