Question

The equilibrium reaction CaCO3(s) ↔ CaO(s) + CO2(g) reaches ΔG° = 0 at 835°C. At this temperature: the pressure of CO2 is 1 atm the percent yield of CaO reaches 100% ΔH° = ΔS° the decomposition of CaCO3 begins the reaction becomes exothermic

Answer 1

1) we know that

dGo = dHo - TdSo

given

dGo = 0

so

dHo = TdSo

2)

the percent yield of CaO does not reach 100 %

3)

the decomposition had already started

4)

the given reaction is endothermic

5)

now

we know that

dGo = -RT lnK

given

dGo = 0

T = 1108 kelvin

so

0 = -RTlnk

K = 1

so

the value of equilibrium constant is 1

now

consider the given reaction

CaC03 (s) ---> CaO (s) + C02 (g)

we know that

solids are not consider for equilibrium expression

so

K = pC02

1 = pC02

pC02 = 1

so

the pressure of C02 is 1 atm

So

the answer is

presusre of C02 is 1 atm