An industrial chemist is studying the rate of the haber synthesis: n2 + 3h2 → 2nh3. starting with a closed reactor containing 1.35 mol/l of n2 and 0.35 mol/l of h2, she finds that the h2 concentration has fallen to 0.12 mol/l after 50. seconds. what is the average rate of reaction of h2 over this time? (enter in mol/liter/sec). what is the average rate of nh3 production for this example? (enter in mol/liter/sec)

1) Balanced chemical reaction: 3H₂ + N₂ → 2NH₃.

c₁(H₂) = 0.35 mol/L; initial concentration of hydrogen gas.

c₂(H₂) = 0.12 mol/L; concentration of hydrogen after 50 seconds.

Δt = 50 s.

the average rate of reaction = 1/3 · (Δc(H₂)/Δt).

the average rate of reaction of hydrogen = 1/3 · ((c₂(H₂)-c₁(H₂))/Δt).

the average rate of reaction = 1/3 · (0.12 mol/L - 0.35 mol/L) / 50 s.

the average rate of reaction of hydrogen = -0.00153 mol/Ls, it is negative because it measures the rate of disappearance of the reactants.

2) From chemical reaction: n(H₂) : n(NH₃) = 3 : 2.

c(NH₃) = 2 · 0.23 mol/L / 3.

c(NH₃) = 0.153 mol/L.

the average rate of reaction of ammonia = 1/2 · (0.153 / 50 s).

the average rate of reaction of ammonia = 0.00153 mol/L·s.

c is having 4 valence electrons and is bonded to three hydrogens and one sulphur atom, therefore, the number of bond pair is equal to four. as all the valence electrons are used in forming the bonds so, there is no lone pair left on carbon.

s is having 6 valence electrons and is bonded to one other sulfur atom and one carbon atom, therefore, the number of bond pair is equal to 2. as only two valence electrons are used in forming the bonds so, four electrons are left. therefore, two lone pairs are present on s.