For a particular reaction, deltaH =-111.4 kJ/mol and deltaS =-25.0 J/mol*K Calcu

Question

For a particular reaction, deltaH =-111.4 kJ/mol and deltaS =-25.0 J/mol*K
Calculate deltaG for this reaction at 298K
________________ kJ/mol
Would this reaction be: A) spontaneous as it is written B) spontaneous in the reverse direction For a particular reaction, deltaH =-111.4 kJ/mol and deltaS =-25.0 J/mol*K
Calculate deltaG for this reaction at 298K
________________ kJ/mol
Would this reaction be: A) spontaneous as it is written B) spontaneous in the reverse direction
Calculate deltaG for this reaction at 298K
________________ kJ/mol
Would this reaction be: A) spontaneous as it is written B) spontaneous in the reverse direction

Explanation / Answer

Answer: Hence we know that delG = delta H - T delta S

so now putting all the given values in kJ and kelvin units we get

delta G = -111.4 - [ 298 ( -0.025 ) ] = -111.4 + 7.45 = - 103.95 Kj/mol

Hence the deta G is = - 103.95 kj/mol

it is negative and we know that for spontaneous reaction delG must be negative hence it is spontaneous as it is written .

Related Questions

Navigate

• Browse (All)
• Browse F
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.