A chemical engineer is studying he two reactions shown in the table below. In ea

Question

A chemical engineer is studying he two reactions shown in the table below. In each case, he fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 83.0 degree C and constant total pressure. Then, the measures the reaction enthalpy delta H and reaction entropy delta S of the first reaction. The results of his measurements are shown in the table. Complete the table. That is, calculate delta G for the first reaction and delta S for the second. (Round your answer to zero decimal places.) Then, decide whether, under the conditions the engineer has set up, the reaction is spontaneous, the reverse reaction is spontaneous, or neither forward nor reverse reaction is spontaneous because the system is at equilibrium. 2H_2O(g) rightarrow 2H_2(g) + O_2 (g) delta H = 484, kJ delta S = 1432 J/K delta G = kJ Which is spontaneous? this reaction the reverse reaction neither C_3H_8 (g) + 5O_2 (g) rightarrow 3CO_2 (g) + 4H_2O(l) delta H = -2220, kJ delta S = J/K delta G = 30. kJ Which is spontaneous? this reaction the reverse reaction neither

Explanation / Answer

Q1.

dG = dH - T*dS

change T = Kelvin,and }Entropy to kJ/mol

dG = 484 - (83+273)*(1432/1000)

dG = -25.79 kJ/mol

this is negative, so this favours the reaction in the forward direaction

B)

dG = dH - T*dS

30 = -2220 - (83+273)*dS

dS = (30 +2220 ) / (83+273)

dS = 6.320224 KJ/molK

dS = 6320.224 J/molK

since dG < 0 , this must favour REVERSE reaction

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

---

---

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