When a 0.1 m h2so4 solution is added to pulverized blackboard chalk, the following reaction takes place.
caco3(s) + h2so4(aq) --> caso4(s) + co2(g) + h2o(l)
at 25°c, the reaction is spontaneous and has:
a. negative δg' and positive δs'
b. negative δg' and negative δs'
c. positive δg' and negative δs'
d. positive δg' and positive δs'

Option A ( negative ΔG' and positive ΔS') is correct.

Explanation:

If a process is spontaneous or not can be determined by the following equation:

process that occurs at constant temperature and pressure, spontaneity can be determined using the change in Gibbs free energy, which is given by:

ΔG = ΔH - TΔS

→ with ΔH = changes in enthalpy

 → with ΔS = changes in entropy

 → with T = The temperature

To be spontaneous ΔG should be negative, this happens when:

When ΔS > 0 and ΔH < 0, the process is always spontaneous as written.

When ΔS > 0 and ΔH > 0, the process will be spontaneous at high temperatures and non-spontaneous at low temperatures.

When ΔS < 0 and ΔH < 0, the process will be spontaneous at low temperatures and non-spontaneous at high temperatures.

The reaction will not be spontaneous:

When ΔS < 0 and ΔH > 0, the process is never spontaneous, but the reverse process is always spontaneous.

To be spontaneous ΔG should be negative so only option A and B are possible.

The entropy is increasing, so ΔS>0,  because a gas (CO2) is being produced and the number of molecules is increasing.

Option A ( negative ΔG' and positive ΔS') is correct.

where are the choice options?