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In 1790, Nicolas Leblanc found a way to form Na₂CO₃ from NaCl. His process, now obsolete, consisted of three steps:2NaCl(s) + H₂SO₄(aq) & → Na₂SO₄(aq) + 2HCl(g)
Na₂SO₄(s) + 2C(s) & → Na₂S(s) + 2CO₂(g)
Na₂S(s) + CaCO₃(s) & → Na₂CO₃(s) + CaS(s)(c) Is the overall process spontaneous at standard-state conditions and 298 K?



Answer :

The overall process is not spontaneous at standard-state conditions and 298 K.

How this is calculated?

  • The entropy change of the cosmos is used to calculate the process to assess how spontaneous a response is. 
  • This process is spontaneous if Delta s is positive. 
  • Negative Delta S indicates a non-spontaneous process.
  • ΔS sun iv=ΔS system+ ΔS surroundings
  • The entropy at 500 degrees Celsius will be -13J/K×mol. 
  • The entropy at 700 degrees Celsius will be -5.8 J/K×mol. 
  • The subsequent melting of NaCl at standard-state circumstances and 298 K is not spontaneous because we know that there is a reduction and that Delta S is less than zero at both dimension temperatures.

Hence, The overall process is not spontaneous at standard-state conditions and 298 K.

To learn more about NaCl, refer to:

https://brainly.com/question/24490939

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