Consider the synthesis of ammonia: N2(g) + 3H2(g) → 2NH3(g). At 298 K, the equilibrium constant Kp is 6.3×105 and the standard reaction enthalpy is -93.2 kJ/mol. Find the equilibrium constant at 450 K and report it with the precision of <1%.

Consider the reaction NH4+(aq) H+(aq)+NH3(aq) Use G f for NH3(aq) at 25C=26.7 kJ/mol and the appropriate tables to calculate (a) G at 25C (b) Ka at 25C

Suppose you have an endothermic reaction with H = + 15 kJ and a S of 150 J/K. Calculate G and Keq at 10, 100, and 1000 K.

At a certain temperature, K=0.29 for the decomposition of two moles of iodine trichloride, ICl3(s), to chlorine and iodine gases. The partial pressure of chlorine gas at equilibrium is three times that of iodine gas. What are the partial pressures of iodine and chlorine at equilibrium?

For the reaction aA(aq) + bB(1) cC(g) + dD(aq) the equilibrium constant, K, can be written as Pc- [D]d [A]a K= The equilibrium constant is unitless because the units always mathematically cancel when the pressure is expressed in torr and concentration is expressed in molality. each quantity is a dimensionless ratio of the actual concentration or pressure divided by standard state concentration or pressure. pressure and concentration are unitless quantities. taking each pressure or concentration to its coefficient power cancels out the units.

Calculate the value of the reaction quotient Q when the reaction beaker contains 0.13 g Al, 0.33 M CuCl2, 0.42 g Cu, and 0.46 M AlCl3. *doesn’t require units

Ethyl acetate is synthesized in a nonreacting solvent (not water) according to the following reaction: CH; CO,H + C,H OH = CH; CO,C,H; + H20 K = 2.2 Acetic acid Ethanol Ethyl acetate For the following mixtures (a-d), will the concentration of H2 O increase, decrease, or remain the same as equilibrium is established? а. [сH,CO,C, Ны] — 0.22 М, [Н,0] — 0.1о м, [сH,СО, н] — 0.010 м, [C, H, онј — 0.010 M O increase O ecrease O remain the same b. [CH; CO2C,H5] = 0.22 M, [H2O] = 0.0020 M, [CH3 CO,H] = 0.0020 M, [C,H;OH] = 0.10 M O increase O decrease Oremain the same c. [CH; CO2C,H5]= 0.88 M , [H2O] = 0.12 M, [CH; CO,H] = 0.044 M, [C,H; OH] = 6.0 M с. O increase decrease Oremain the same d. [CH3 CO,C,H5]= 4.4 M , [H2O] = 4.4 M, [CH3 CO,H] = 0.88 M , [C,H5 OH] = 10.0 M O increase O decrease Oremain the same e. What must the concentration of water be for a mixture with [CH3CO,C,H5] = 1.0 M, [CH3 CO;H] = 0.10 M , and [C2H; OH] = 6.0 M to be at equilibrium? Concentration м

Solid NH4I ammonium iodide (which is always considered to be in excess) is introduced into an initially empty container at a constant temperature of 427°C. An equilibrium is quickly established and the total pressure (PT) is then 0.9 bar. NHẠI (s) 2 NH3(g) + HI(g) Express the equilibrium constant K' of this reaction as a function of PT a. Express the equilibrium constant K' of this reaction as a function of PT- The answer is PNH, PHI - - ( 2 2 P K' || po2 p°2 2P°, Can you explain why we get (p/2)^2?

The decomposition reaction, C(9) = A(g) + 2B(g) has Ke 26 at 298 K. What is the value of K, for this system at 298 K? K, = | %3!

At 298 K, the equilibrium constant for the reaction Fe,O3(s) + 3 H2(g) 2 2 Fe(s) + 3 H¿O(€) is 4.0 × 10-6, and that for CO2(g) + H2(g) 2 CO(g) + H,O(€) is 3.2 x 10-4. Suppose some solid Fe,O3, solid Fe, and liquid H2O are brought into equilibrium with CO(g) and CO2(g) in a closed container at 298 K. Calculate the ratio of the partial pressure of CO(g) to that of CO2(g) at equilibrium.