Is it possible for a reaction with + ΔG° to still be spontaneous in the forward direction? Explain.

See explanation.

Explanation:

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In this case, according to the thermodynamic definition of the Gibbs free energy:

In the scenario by which G>0 (nonspontaneous) it would be possible for reaction to have a G<0 (spontaneous) if:

- If H>0 and S>0, then the temperature should be increased until the process was entropy-driven for it to be possible.

- If H> and S<0, then it'd be impossible to have an spontaneous process.

- If H<0 and S>0 then the process was not spontaneous.

- If H<0 and S<0 it is possible if the temperature is not high enough to ensure the process is enthalpy-driven.

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water at room temperature is flowing through a pipe with pressure taps located 10 ft apart along one section of the pipe, which are connected to a mercury (s=13.6) manometer.

> b takes place in the gas phase in an isothermal tubular reactor. the feed is one mole of a per one mole of c, an inert. the entering temperature and pressure are 427°c and 10 atm, respectively. the gas constant r = 0.08206 atm · l/mol · k.