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A chemical engineer is studying the two reactions shown in the table below.
In each case, she fills a reaction vessel with some mixture of the reactants and products at a constant temperature of 57.0Β°C and constant total pressure. Then, she measures that reaction enthalpy delta H and the 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 her 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 or reverse reaction is spontaneous because the system is at equilibrium.

A chemical engineer is studying the two reactions shown in the table below In each case she fills a reaction vessel with some mixture of the reactants and produ class=

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Explanation:

Here are the answers. Do note that I had to convert the enthalpy to joules and temperature to Kelvin to make the unit for entropy work out.

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Enthalpy change is the difference between the enthalpy of the products and the reactant in the reaction. delta G for the reaction is -8.19 kJ and delta S is -151.5 J/K.

What is a spontaneous reaction?

A spontaneous reaction is a that favors product formation. It is estimated by the negative sign of the delta H and the positive sign of [tex]\rm -T\rm \Delta S.[/tex]

[tex]\rm \Delta G[/tex] for the first reaction is calculated as:

[tex]\begin{aligned} \rm \Delta G &= \rm \Delta H - T\Delta S \\\\&= 852000 - (330)(2557)\\\\&= 8190 \;\rm J\end{aligned}[/tex]

Joules are converted to kilojoules and the value of delta G is - 8.19 KJ. Hence the reaction is spontaneous.

For the second reaction delta S is calculated as:

[tex]\begin{aligned} \rm \Delta H &= \rm T\Delta S + \Delta G ^{\circ}\\\\\rm \Delta S &= \rm \dfrac{\Delta H}{T}\\\\&= \dfrac{-50000}{330}\\\\&= -151.5 \;\rm J/K\end{aligned}[/tex]

Since in the reaction the value of delta G is zero the reaction will not be spontaneous.

Therefore, the first reaction is spontaneous, while the second reaction is not spontaneous.

Learn more about enthalpy here:

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