Consider the following reaction which produces phosgene, a toxic gas used in WWI. CO (g) + Cl2 (g) ⇌ COCl2 (g) A vessel at 77°C is filled to the following initial partial pressures: PCO = 1.25 atm PCl2 = 1.65 atm PCOCl2 = 0.50 atm The standard Gibb’s Energies of Formation (ΔGf°) for CO is -137.2 kJ/mol and for phosgene (COCl2) is -304 kJ/mol. Compute the ΔG of this reaction mixture which has not yet reached equilibrium. Enter your answer in units kJ/mol.

Consider the following reaction: 2 CO2 (g) + 2 H, = 2 CO (g) + 2 H20 (g) K= 6.00 At the start of the reaction, the flask contains 0.550 atm CO2, 0.300 atm H2, and 1.20 atm CO, and 1.50 atm H20. a. Calculate the value of the reaction quotient, Q. b. Which direction will the reaction proceed to achieve equilibrium?

For the following reaction, AH = 2816 kJ. 6 CO₂(g) + 6 H₂O(I) ⇒ C6H12O6(s) + 6 O₂(g) Select ONE combination of strategies that when applied to this system at equilibrium will result in an increase in the amount of C6H₁2O6 as equilibrium is re-established? a. Increasing Po₂ by adding more O2; increasing the temperature; decreasing the volume; or removing CO₂ b. Increasing Po₂ by adding more O₂ and decreasing the volume C. Decreasing the volume d. Increasing Po₂ by adding more O₂ e. Increasing the temperature

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 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

The equilibrium constant, Kp, for the following reaction is 1.57 at 600 K.CO(g) + Cl2(g) COCl2(g)If ΔH° for this reaction is -108 kJ, what is the value of Kp at 699 K?Kp =

We start with a sample of pure A(g). The following equilibrium is established 2 A(g) <---> B(g) + C(g) The total pressure is 8.33 atm and the temperature is 25.0oC. The partial pressure of A(g) is 5.26 atm. Calculate the value of the standard free enthalpy change (in kJ) of this reaction at 25.0oC.

For the following reaction: NH4Cl(s) ↔ NH3(g) + HCl(g) ΔH = +42.1 kilocalories Suppose the substances in the reaction above are at equilibrium at 600K in volume V and at pressure P. State whether the partial pressure of NH3(g) will have increased, decreased, or remained the same when equilibrium is reestablished after each of the following disturbances of the original system. Some solid NH4Cl remains in the flask at all times. Justify each answer with a one-or-two sentence explanation. (e) A quantity of gaseous NH3 is added. The answer for e states that the partial pressure of NH3 is increase, which is a bit confusing. The explanation is that some of the the added NH3 reacts with HCl to relieve stress but only part of NH3 reacts. Can you explain how and where this is implied in the reaction or question. Would appreciate a lot of clarification

:Calculate Kp for the following reaction.5 A(g) = 2 B(g) + C(g) 2 .at 400 °C if Kc at 400 °C for this reaction is 0.15 * (R = 8.314 J/mol.K = 0.0821 L.atm/mol.K) %3D 8 0 41 O 30 O 19 O 53 O

Consider the decomposition of calcium carbonate: CaCO3 (s) ⇌ CaO(s) + CO2 (g) Calculate the pressure in atm of CO2 in an equilibrium process at 800oC. Assume that  ΔHo = 177.8 kJ/mol and  ΔSo = 160.5 J/molK under these conditions.