Be sure to answer all parts. Take all the thermodynamic data from your textbook. Assume the data do not vary with temperature.

(a) Calculate ΔSuniv for the reaction H2O2(l) → H2O2(g) at 171.0°C. Enter your answer in the box provided. J/K · mol

(b) Is the reaction spontaneous, nonspontaneous, or an equilibrium process? Select the best single answer. spontaneous nonspontaneous an equilibrium process

(c) The reaction NH3(g) + HCl(g) → NH4Cl(s) is spontaneous in the forward direction at room temperature. Determine the temperature at which it is no longer spontaneous in the forward direction.

(d) Determine the boiling point of Br2, in degrees C

b. atoms in metallic solids are not arranged in a regular pattern

explanation:

n2(g) + 3h2-> 2nh3(g)   this is the balanced equation

note the mole ratio between n2, h2 and nh3.   it is 1 : 3 : 2   this will be important.

moles n2 present = 28.0 g n2 x 1 mole n2/28 g = 1 mole n2 present

moles h2 present = 25.0 g h2 x 1 mole h2/2 g = 12.5 moles h2 present

based on mole ratio, n2 is limiting in this situation because there is more than enough h2 but not enough n2.

moles nh3 that can be produced = 1 mole n2 x 2 moles nh3/mole n2 = 2 moles nh3 can be produced

grams of nh3 that can be produced = 2 moles nh3 x 17 g/mole = 34 grams of nh3 can be produced

note:   the key to this problem is recognizing that n2 is limiting, and therefore limits how much nh3 can be produced.