Determine which of the following statement is correct when the equilibrium constant K for a certain reaction is 10 at 298 K and
0.1 at 400 K? 1. The reaction is not spontaneous at any temperature if the standard entropy of reaction is positive.
2. The reaction is endothermic.
3. The reaction is not spontaneous at any temperature if the standard entropy of reaction is negative.
4. The reaction is spontaneous at any temperatures if the standard entropy of reaction is positive.
5. Cannot be determined without knowing what reaction that is.
4. The reaction is spontaneous at any temperatures if the standard entropy of reaction is positive.
Explanation:
Equilibrium constant decreases on increasing the temperature . So the reaction appears to be exothermic . In other words
ΔH is negative .
Δ G = ΔH - TΔS
If ΔS is positive , second term is negative . ΔH is negative so the RHS of the equation is negative at all temperatures . Hence Δ G of the reaction is negative . So reaction is spontaneous at any temperature.
In , 3 ions and 6 ions are present. is formed when two ions bonded to an ions.
Thus, the term in a balanced chemical equation says that there are three formula units, each consisting of two chloride ions bonded to an iron(II) ion.
Magnesium and chlorine form an ionic bond. Covalent bonds are formed when two or more atoms share electrons between them. ... So two chlorine anions form an ionic bond with one magnesium cation for form MgCl2, a neutral chemical compound.