Use the thermodynamic information below to determine the free energy change for the following reaction, which is run under standard state conditions and at 25°C. Then calculate the temperature at which the reaction will become spontaneous. SiO2(s) + 4 HF(aq) → SİF4(9) + 2 H2O(1) A G° = kJ Temperature at which the reaction will become spontaneous. K

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Use the thermodynamic information below to
determine the free energy change for the
following reaction, which is run under standard
state conditions and at 25°C.
Then calculate the temperature at which the reaction will become
spontaneous.
SiO2(s) + 4 HF(aq) → SIF4(g) + 2 H2O(1)
A G°=
kJ
Temperature at which the reaction will become spontaneous.
K
s (
J
kJ
Substance | AH;(-
mol
S°
mol K
Si0,(s)
-911
42
HF(aq)
-333
-14
(3)"
SiF (g)
-1615
283
H,O(1)
-286
70
Transcribed Image Text:Use the thermodynamic information below to determine the free energy change for the following reaction, which is run under standard state conditions and at 25°C. Then calculate the temperature at which the reaction will become spontaneous. SiO2(s) + 4 HF(aq) → SIF4(g) + 2 H2O(1) A G°= kJ Temperature at which the reaction will become spontaneous. K s ( J kJ Substance | AH;(- mol S° mol K Si0,(s) -911 42 HF(aq) -333 -14 (3)" SiF (g) -1615 283 H,O(1) -286 70
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