For a particular reaction, ΔH∘=−28.4 kJ and ΔS∘=−87.9 J/K. Assuming these values change very little with temperature, at what temperature does the reaction change from nonspontaneous to spontaneous?

282 K.

Explanation:

We know that G = H - T * S

If we want to find the temperature that the spontaneity of the reaction changes, we set the free energy equal to 0 and solve for T.

0 = -24.8 + 0.0879 T  (make sure to keep units all the same in terms of kJ)

T = 282 K.

hope this

explanation:

covalent bonds

consist of pairs of electrons shared by two atoms, and bind the atoms to fixed orientation and requre high energies to break them

ionic bonds

when two atoms differ considerably in their electronegativity, then one of the atoms will lose its electron to the other atom. this results in a positively charged ion(cation) and a negatively charged ion (anion)

the increase of protons   hope this