Question

During a spontaneous chemical reaction, it is found that ΔSsys is less than 0. This means that Group of answer choices ΔSsurr is less than 0 and its magnitude is less than ΔSsys. ΔSsurr is less than 0 and its magnitude is greater than ΔSsys. ΔSsurr is greater than 0 and its magnitude is less than ΔSsys. ΔSsurr is greater than 0 and its magnitude is greater than ΔSsys. an error has been made, as Ssys is greater than 0 by necessity for a spontaneous process.

Answer 1

Answer:

The correct option is: ΔSsurr is greater than 0 and its magnitude is greater than ΔSsys.  

Explanation:

For a chemical reaction to be spontaneous, the change in the Gibbs free energy should be negative (ΔG = -ve).

At constant temperature (T) and pressure, the Gibbs free energy is given by the equation: $\Delta G_{system} = \Delta H_{system} - T\Delta S_{system}$

Here, $\Delta H_{system}$ is the enthalpy change and $\Delta S_{system}$ is the entropy change of the system.

Also, according to the second law of thermodynamics, for a spontaneous process, the total entropy, $\Delta S_{universe} = \Delta S_{system} + \Delta S_{surrounding} > 0$

Therefore, for a reaction to be spontaneous, if $\Delta S_{system}$ is less than 0 or negative; then $\Delta S_{surrounding}$ should be greater than 0 or positive. Also, $\Delta S_{surrounding}$ > $\Delta S_{system}$.