Question

The phase change between white tin and gray tin is difficult to observe directly. Both substances can be burned, however. From these equations, calculate AHⓇ for the conversion of gray tin into white tin:
Sn(s, white) + O2(g) + SnO2(g) AH = -580.69 kJ
Sn(s, gray) + O2(g) + SnO2(g) AH° = -582.78 kJ
AH = _________ kJ

Answer 1

Answer: Thus $\Delta H$ for the conversion of gray tin to white tin is -20.9 kJ

Explanation:

According to Hess’s law of constant heat summation, the heat absorbed or evolved in a given chemical equation is the same whether the process occurs in one step or several steps.

According to this law, enthalpy change of the overall reaction is the sum of the enthalpy changes of the intermediate reactions.

The final reaction is

$Sn(s, gray)\rightarrow Sn(s, white)$  $\Delta H=?$

The intermediate balanced chemical reaction will be,

$Sn(s, gray)+O_2(g)\rightarrow SnO_2(g)$  $\Delta H^0=-582.78kJ$    (1)

$Sn(s, white)+O_2(g)\rightarrow SnO_2(g)$  $\Delta H^0=-580.69kJ$     (2)    

substarcting (2) form (1) we get

$\Delta H=\Delta H_1-\Delta H_2$

$\Delta H=-582.78-(-580.69kJ)$

$\Delta H=-20.9kJ$