What is the equilibrium constant at 25o C for the reaction 2 CO(g) + O2(g) ⇌ 2 CO2(g) given the following data: ΔGfo[CO(g)] = –137.2 kJ/mol ΔGfo[CO2(g)] = –394.4 kJ/mol

Consider the following equilibrium: N2 (g)+3H2(g)2NH3 (g) AG = -34. kJ Now suppose a reaction vessel is filled with 2.15 atm of nitrogen (N2) and 2.19 atm of ammonia (NH3) at 236. °C. Answer the following questions about this system: OO rise ☐ x10 fall OO Under these conditions, will the pressure of NH3 tend to rise or fall? Is it possible to reverse this tendency by adding H₂? 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 H2? Similarly, if you said the pressure of NH3 will tend to fall, can that be changed to a tendency to rise by adding H₂? If you said the tendency can be reversed in the second question, calculate the minimum pressure of H2 needed to reverse it. Round your answer to 2 significant digits. yes no ☐ atm S

Consider the following equilibrium: 2NO, (g) – N,04(g) AG = - 5.4 kJ Now suppose a reaction vessel is filled with 7.26 atm of dinitrogen tetroxide (N,O) at 95. °C. Answer the following questions about this system: rise Under these conditions, will the pressure of N,O, tend to rise or fall? 4 fall Is it possible to reverse this tendency by adding NO,? In other words, if you said the pressure of N,0, will tend to rise, can that yes be changed to a tendency to fall by adding N0,? Similarly, if you said the no pressure of N,0, 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. O O

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.

What is AGxn (in kJ) at 1932 K for the following reaction? 2POCI3(g) → 2PC13(g) + O₂(g) POCI3(g): AH = -592.7 kJ/mol and Sº = 324.6 J/K mol) PC13(g): AH = -287.0 kJ/mol and So = 311.7 J/K mol) O₂(g): AH = ? kJ/mol and Sº = 205.0 J/K mol)

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.

A reaction has an equilibrium constant (K) of 90.9.  If the entropy of this reaction is -69.1 J/mol K at a temperature of 280 K, what is the enthalpy of this reaction in kJ/mol?Report your answer to one decimal place. ΔG = ΔH - T ΔSΔG = -RT ln K

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.