If at 400°C the equilibrium constant for the reaction NO2(g) + H2(g) = NO(g) + H₂O(g) has Kp = 7.28 x 10-6, what is AG for this reaction at 400°C? (1) 66.2 kJ/mol O (3) 654 kJ/mol O (4) 388 kJ/mol O (2) 39.3 kJ/mol Question 2 of

BaCl, · H,O(s) loses water when it is heated in an oven: BaCl, · H,O(s) = BaCl, (s) + H,O(g) AH° = 63.11 kJ/mol at 25 °C AS +148 J/(K · mol) at 25 °C Write the equilibrium constant for this reaction. Find the vapor pressure of H,O (PH,0) above BaCl, · H,O(s) at 298 K. PH,0 bar = If AH° and AS° are not temperature dependent (a poor assumption), estimate the temperature at which PH,0 above BaCl, · H, O(s) will be 1 bar. T = °C

The reaction N204(g) 2NO2(g) has a K, = 0.140 at 25 °C. In a reaction vessel containing the gases in equilibrium at that temperature, the partial pressure of N204 was 0.127 atm. (a) What was the partial pressure of NO2 in the reaction mixture? pressure of NO2 = i atm (b) What was the total pressure of the mixture of gases? total pressure = i atm

The equilibrium system shown below was analyzed and the concentrations of H2(g), I2(g) and HI(g), were found, in mol/L, to be 4.2, 3.8, 1.6 respectively. The equilibrium constant must be? H2(g) + I2(g) <=====> 2HI(g) + 65 kJ

The equilibrium constant for the following reaction is 260 at -1 °C. 2 NO(g) + Br₂(g) 2 NOBr(g) K 260 at -1 °C - Calculate the equilibrium constant for the following reactions at -1 °C. (a) 2 NOBr(g) (b) NOBr(g) ? 2 NO(g) + Br₂(g) NO(g) + 1/2 Br₂(g) K = K =

10 Determine the structure of an alcohol with the molecular formula CH₁O that exhibits the following 13C NMR spectra. Broadband-decoupled 100 90 80 70 DEPT-90 100 60 60 50 50 40 30 30 20 20 90 80 60 70 60 50 50 40 40 DEPT-135 100 90 80 80 50 30 30 10 10 0 20 10 0 40 30 20 20 Chemical Shift (ppm) 70 60 10 0

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?

(b) At 100° C, the Keq for the Haber process is 4,51 X 10-5: N₂ + 3 H₂ 2 NH3 Consider the following reaction conditions and determine if the system is at equilibrium. If not, indicate the direction in which the reaction must proceed to establish equilibrium (i) PNH3 105 atm, PN2 = 35 atm and PH2 = 495 atm (ii) PNH3 35 atm, PN2 = 0 atm and PH2 = 595 atm (iii) PNH3 = 26 atm, PN2 = 202 atm and PH2 = 42 atm (iv) PNH3 105 atm, PN2 = 5 atm and PH2 = 55 atm