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.

adding or remove a gaseous reactant or product changes the concentrations. if the concentration of reactant or product is increased, the system will shift away from the side in which concentration was increased (i.e. if the concentration of reactants is increased, the system will shift toward the products. if more products are added, the system will shift to form more reactants). conversely, if the concentration of reactant or product is decreased, the system will shift toward the side in which concentration was decreased (i.e. if reactants are removed, the system will shift to form more reactants. if the concentration of products is decreased, the equilibrium will shift toward the products).

explanation: