Calorimetry Of A Chemical Reaction Lab Report

1. Ozone (O3) in the atmosphere can react with nitric oxide (NO): O3(g) + NO(g) ( NO2(g) + O2(g), with (H( = -199 kJ/mol, (S( = -4.1 J/K·mol. Calculate the (G( for this reaction at 25(C. A. 1020 kJ/mol B. -1.22 ( 103 kJ/mol C. 2.00 ( 103 kJ/mol D. -1.42 ( 103 kJ/mol E. -198 kJ/mol

2. For the reaction H2(g) + S(s) ( H2S(g), (H( = -20.2 kJ/mol and (S( = +43.1 J/K·mol. Which of these statements is true? A. The reaction is only spontaneous at low temperatures. B. The reaction is spontaneous at all temperatures. C. (G( becomes less favorable as temperature increases. D. The reaction is spontaneous only at high temperatures. E. The reaction is at equilibrium
The equilibrium constant for the reaction AgBr(s) ℜ Ag+(aq) + Br- (aq) is Ksp = 7.7 ( 10-13 at 25(C. Calculate (G for the reaction when [Ag+] = 1.0 ( 10-2 M and [Br-] = 1.0 ( 10-3 M. Is the reaction spontaneous or nonspontaneous at these concentrations? A. (G = 69.1 kJ/mol, nonspontaneous B. (G = -69.1 kJ/mol, spontaneous C. (G = 97.5 kJ/mol, spontaneous D. (G = 40.6 kJ/mol, nonspontaneous E. (G = -97.5 kJ/mol, nonspontaneous

6. The element oxygen was prepared by Joseph Priestley in 1774 by heating mercury(II) oxide: HgO(s) ( Hg(l) + ½ O2(g) (H( = 90.84 kJ/mol.
Estimate the temperature at which this reaction becomes spontaneous under standard state conditions.
[S(( Hg) = 76.02 J/K mol, S(( O2) = 205.0 J/K mol, S(( HgO) = 70.29 J/K
108 K B. 430 K C. 620 K D. 775 K E. 840 K

7. The normal freezing point of ammonia is -78(C. Predict the signs of (H, (S, and (G for ammonia when it freezes at -80(C and 1 atm: NH3(l) ( NH3(s) [pic]

8. Find the temperature at which the reaction N2O4(g) ℜ 2NO2(g) will be in equilibrium when both gases are present at partial pressures of 1.00 atm. A. 300(C B. 28(C C. 55(C D. 32(C E. 562(C

9. Predict the normal boiling point of triethylborane (C6H15B) using thermodynamic data. A. 92(C B. -21(C C. 21(C D. 365(C E. 256(C

10. A sample of solid naphthalene is introduced into an evacuated flask. Calculate the equilibrium vapor pressure of naphthalene (C10H8) in the flask at 35(C. A. 890. mmHg B. 0.21 mmHg C. 696 mmHg D. 0.086 mmHg E. 833 mmHg

11. Find the temperature at which Kp = 4.00 for the reaction N2O4(g) ℜ 2NO2(g). [Assume that (H( and (S( are independent of temperature.] A.