4.8g of C (diamond) on complete combustion evolves 1584kJ of heat. The standard heat of formation of gaseous carbon is 725 kJ/mol. The energy required for the process i) C(graphite) --> C(gas) ii) C (diamond) --> C(gas) are

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4.8 g

C

(diamond) on complete combustion evolves

1584 k J

of heat. The standard heat of formation of gaseous carbon is

725 k J / m o l

. The energy required for the process
(i)

C

(graphite)

\to C

(Gas) (ii)

C

(diamond)

\to C

(gas) are:

Q. A standard heat of formation of CS2 (I) will be:, given that the standard heat combustion of carbon(s), Sulphur(s) and

C S_{2} (l)

are

- 393.3, - 293.72 a n d - 1108.76 K j / m o l

respectively.

Q. Standard molar heat enthalpy for converting carbon from graphite and diamond form into vapour state directly are 725 and 713 kJ respectively. The standard enthalpy change for polymorphism of 1 g carbon

C_{G \to D}

is _____ .

The standard heat of formation of carbon disulphide $(l)$ given that standard heat of combustion of carbon (s), sulphur (s) and carbon disulphide $(l)$ are -393.3, -293.72 and -1108.76 KJ mol $^{- 1}$ respectively is

Q. Calculate the standard heat of formation of carbon-di-sulphide(l). Given that the standard heats of combustion of carbon(s), sulphur(s) & carbon disulphide(l) are -393.3, -293.7 & -1108.76

k J m o l^{- 1}

respectively.

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