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

Question

A chemical engineer is studying the two reactions shown in the table below. In each case, he fills a reaction v with some mixture of the reactants and products at a constant temperature of 80.0 degree C and constant total pressure. Then, he measures the reaction enthalpy Delta H and reaction entropy Delta S of the first reaction, and the reaction enthalpy Delta H and reaction free energy Delta G of the second 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.

Explanation / Answer

Q1.

dG = dH - T*dS

substitute data, dS must be in KJ so divide by 1000

dG = -1207 - (80+273)*(-3418/1000) = -0.446 kJ/mol

this is almost in equilibrium, but will favour slightly more PRODUCTS i.e. the reaction as shown

Q2.

Apply

dG = dH - T*dS

-6 = 140 - (80+273)*dS/1000

dS =( -6 - 140 ) /(80+273) * 1000 = -413.59 J/K

this has a negative dG so

this must favour FORWARD reaction

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