2 (g) + 3H2 (g) 2NH3 (g) ΔrS = - 201 J K−1mol−1 ΔrH = - 99.3 kJ mol-1 a) Calculate the ΔrG for the reaction above at 30 °C. b) As written, is this reaction spontaneous or nonspontaneous and why? At what temperature will this reaction be spontaneous? Briefly justify your answer c) Explain why the value of ΔrS is negative for this chemical reaction. List two circumstances where ΔrS will be negative. d) A gas mixture of total pressure 56 kPa consisting of 1 part N2 to 3 parts H2 was obtained in the reaction above. Calculate the partial pressure of nitrogen and hydrogen gas in the gas mixture e) How much work is done when a piston is compressed from 9.87 L to 2.56 L under constant atmospheric pressure (1.013 × 105 Pa)? f) Which intermolecular forces will be dominant between NH3 molecules? Which has the higher boiling point: NH3 or PH3? Briefly justify your answer g) What intermolecular forces will be dominant between N2 molecules? Briefly justify your answer.
N2 (g) + 3H2 (g) 2NH3 (g)
ΔrS = - 201 J K−1mol−1
ΔrH = - 99.3 kJ mol-1
a) Calculate the ΔrG for the reaction above at 30 °C.
b) As written, is this reaction spontaneous or nonspontaneous and why? At what temperature will this reaction be spontaneous? Briefly justify your answer
c) Explain why the value of ΔrS is negative for this
d) A gas mixture of total pressure 56 kPa consisting of 1 part N2 to 3 parts H2 was obtained in the reaction above. Calculate the partial pressure of nitrogen and hydrogen gas in the gas mixture
e) How much work is done when a piston is compressed from 9.87 L to 2.56 L under constant atmospheric pressure (1.013 × 105 Pa)?
f) Which intermolecular forces will be dominant between NH3 molecules? Which has the higher boiling point: NH3 or PH3? Briefly justify your answer
g) What intermolecular forces will be dominant between N2 molecules? Briefly justify your answer.
The balanced equation is:
N2(g) + 3H2(g) 2NH3(g)
rS = - 201 J.mol-1.K-1 or - 0.201 kJ.mol-1.K-1
rH = - 99.3 kJ.mol-1.
Step by step
Solved in 4 steps
