Question

For a reaction for which ΔH = -64.2 kJ/mol and ΔS = +285 J/mol K, which of the following statements is true? A) The reaction is spontaneous only above 225 K. B) The reaction is spontaneous only below 225 K. C) The reaction will never reach equilibrium. D) The reaction is always at equilibrium.

Name: for a reaction for which h 642 kjmol and s 285 jmol k which of the following statements is true a the reaction is spontaneous only above 225 k b the reaction is spontaneous only below 225 k 12922
Uploaded: 2022-06-14T02:29:25-08:00
Duration: 2 min 45 s
Channel: Adi S
Description: for a reaction for which h 642 kjmol and s 285 jmol k which of the following statements is true a the reaction is spontaneous only above 225 k b the reaction is spontaneous only below 225 k 12922

          For a reaction for which ΔH = -64.2 kJ/mol and ΔS = +285 J/mol K, which of the following statements is true? 
A) The reaction is spontaneous only above 225 K. 
B) The reaction is spontaneous only below 225 K. 
C) The reaction will never reach equilibrium. 
D) The reaction is always at equilibrium.

for a reaction for which h 642 kjmol and s 285 jmol k which of the following statements is true a the reaction is spontaneous only above 225 k b the reaction is spontaneous only below 225 k 12922

Added by Jennifer G.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Adi S

06/14/2022

Step 1

Step 1: We can use the equation ΔG = ΔH - TΔS to determine the spontaneity of the reaction, where ΔG is the change in Gibbs free energy, ΔH is the change in enthalpy, T is the temperature in Kelvin, and ΔS is the change in entropy. Show more…

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For a reaction for which ΔH = -64.2 kJ/mol and ΔS = +285 J/mol K, which of the following statements is true? A) The reaction is spontaneous only above 225 K. B) The reaction is spontaneous only below 225 K. C) The reaction will never reach equilibrium. D) The reaction is always at equilibrium.