Calculate delta g reaction at 298 k under the conditions 2hg+o2

The balanced chemical reaction is 2Hg + O2 -> 2HgO. To calculate the delta G, we use the formula: ΔG = ΔH – TΔS. The ΔH is computed by subtracting the standard enthalpy of formation of the reactants from the products, multiplied correspondingly with their stoichiometric coefficients. The same is to obtain ΔS.

The necessary information all at 298 K are:

ΔH_Hg = 0 kJ/mol; since it is at its standard state

ΔS_Hg = 75.90 kJ/mol

ΔH_O2 = 0 kJ/mol; since it is at its standard state

ΔS_O2 = 0.161 kJ/mol K

ΔH_HgO = -90 kJ/mol

ΔS_HgO = 0.070 kJ/mol K

Thus, the delta G of reaction is -132.022 kJ. The negative value denotes a spontaneous reaction. 

explanation:

metals have excess of electrons whereas non-metals have deficiency of electrons. thus, in order to gain stability metals easily donate their electrons to the non-metals.

for example, electronic configuration of sodium is and electronic configuration of phosphorous is .

when a phosphorous atom and sodium atom combine together then sodium will donate is extra one electron to the phosphorous atom. as a result there will be formation of ionic bond between sodium and phosphorous.

the reaction will be as follows.

there, are three sodium sodium atoms and each of them will donate its one extra electron to phosphorous atom. thus, the sub-shell of phosphorous gets completely filled.  

thus, we can conclude that electrons are transferred from atoms of sodium to atoms of phosphorous. this transfer makes the sodium atoms donate one electron and the phosphorous atoms to gain one electron. as a result, the sodium and phosphorus atoms strongly attract each other.

so here we go

atomic mass

239 + 1 = y + 134 + 3 combine like terms

240 = y + 137             subtract 137 from both terms

240 - 137 = y

103 = y

atomic number

94 = z +54 + 0

94 = z + 54               subtract 54 from both sides.

40 = z

answer