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Chemistry
Chemistry
Problem
For a reaction
M
2
O
(
s
)
→
2
M
(
s
)
+
1
2
O
2
(
g
)
\text{M}_2\text{O}(s) \rightarrow 2\text{M}(s) + \frac{1}{2}\text{O}_2(\text{g})
M
2
O
(
s
)
→
2
M
(
s
)
+
2
1
O
2
(
g
)
;
Δ
H
=
30
kJ mol
−
1
\Delta H = 30 \text{ kJ mol}^{-1}
Δ
H
=
30
kJ mol
−
1
and
Δ
S
=
0.07
kJ K
−
1
mol
−
1
\Delta S = 0.07 \text{ kJ K}^{-1} \text{ mol}^{-1}
Δ
S
=
0.07
kJ K
−
1
mol
−
1
at 1 atm. Calculate up to which temperature the reaction would not be spontaneous?
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