Ncert Exercises & Solutions

Q.12. Enthalpies of formation of $C O_{(g)}, C O_{2 (g)}, N_{2} O_{(g)} a n d N_{2} O_{4 (g)}$

are –110 kJ $m o l^{- 1}$ , – 393 kJ $m o l^{- 1}$ , 81 kJ $m o l^{- 1}$ and 9.7 kJ $m o l^{- 1}$ respectively. Find the value of $∆_{r} H$ for the reaction:

$N_{2} O_{4 (g)} + 3 C O_{(g)} \to N_{2} O_{(g)} + 3 C O_{2 (g)}$

NEETprep Answer:

Formation of

C O_{2}

from carbon and dioxygen gas can be represented as:

C_{(s)} + O_{2 (g)} \to C O_{2 (g)} ∆_{f} H = - 393.5 k J m o l^{- 1}

(1 mole = 44 g)
Heat released on formation of 44 g

C O_{2}

= –393.5 kJ

m o l^{- 1}

∴

Heat released on formation of 35.2 g

C O_{2}

= \frac{- 393.5 k J m o l^{- 1}}{44 g} \times 35.2 g

= - 314.8 k J m o l^{- 1}

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