Calcium carbonate will decompose when heated to produce calcium oxide and carbon dioxide as shown in the following reaction. $CaCO_{3} (s) ? CaO (s) + CO_{2} (g)$ Given that $? H^{?} = 177.5 kJ / mol$ and $? G^{?} = 130.4 kJ / mol$ at $2 5^{?} C$ , above what minimum temperature will the reaction become spontaneous under standard state conditions? Hint: Assume $? H$ and $? S$ are independent of $T$ Hint: Think about the value of $? G$ when a reaction goes from nonspontaneous to spontaneous. $1, 123 K$ $321 K$ $127 K$ $401 K$ $3.9 K$

Question

Calcium carbonate will decompose when heated to produce calcium oxide and carbon dioxide as shown in the following reaction.

CaCO_{3} (s) ? CaO (s) + CO_{2} (g)

Given that

? H^{?} = 177.5 kJ / mol

and

? G^{?} = 130.4 kJ / mol

at

2 5^{?} C

, above what minimum temperature will the reaction become spontaneous under standard state conditions? Hint: Assume

? H

and

? S

are independent of

T

Hint: Think about the value of

? G

when a reaction goes from nonspontaneous to spontaneous.

1, 123 K

321 K

127 K

401 K

3.9 K

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