#DeltaG = DeltaH - TDeltaS# If #DeltaH = -232 kJ, DeltaS = 138 J/K and T = 273 K,# is this reaction spontaneous? Solve to prove and explain

1 Answer
Junaid Mirza
May 9, 2018

Yes. Reaction is spontaneous.

Explanation:

Given

  • #Δ"H" = -"232 kJ"#
  • #Delta"S = 138 J/K"#
  • #"T = 273 K"#

Calculate #Δ"G"# by using the equation

#"ΔG = ΔH - TΔS"#

#"ΔG" = -"232 kJ" - [273 cancel"K" × 138\ "J"/cancel"K"]#

#"ΔG = -232 kJ - 37674 J"#

#"ΔG = -232 kJ - 37.674 kJ"#

#"ΔG = -269.674 kJ"#

For a reaction to be spontaneous #"ΔG"# value must be negative. Therefore reaction is spontaneous.

#color(white)(...)—————————#

#"ΔG < 0"# - Reaction is spontaneous
#"ΔG = 0"# - Reaction is at equilibrium
#"ΔG > 0"# - Reaction is non-spontaneous

Related questions
Impact of this question
1237 views around the world
You can reuse this answer
Creative Commons License