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Calorimetry

The reaction:...

Question

The reaction:- NH2CN(s)+ 3/2O2(g)---->N2(g)+ CO2(g)+ H2O(l) was carried out in a bomb calorimeter. The heat released was 743KJ/mol. Find the value of delta(H)300K for this reaction. 1) -740.5 KJ/mol 2) -741.75 KJ/mol 3) -743 KJ/mol 4) -744.25 KJ/mol

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N H_{2} C N (s) + \frac{3}{2} O_{2} (g) \to N_{2} (g) + C O_{2} (g) + H_{2} O (l)

300 k

742 k J m o l^{- 1}

△ H_{300 K}

Δ E

742.7 k J / m o l

N H_{2} C N (s)

298 K .

N H_{2} C N (s) + \frac{3}{2} O_{2} (g) \to N_{2} (g) + C O_{2} (g) + H_{2} O (l)

Δ H_{298}

(N H_{2} C N)

Δ U

- 742.7 {kJmol}^{- 1}

298 K

298 K

N H_{2} C N (s) + \frac{3}{2} O_{2} (g) \to N_{2} (g) + C O_{2} (g) + H_{2} O (l)

Δ U

1742.7 k J / m o l

N H_{2} C N (s)

{N H}_{2} C N (s) + \frac{3}{2} O_{2} (g) ⟶ N_{2} (g) + {C O}_{2} (g) + H_{2} O (l)

{Δ H}_{3000 K}

(R = 8 J / m o l e - K)

N H_{2} C N (s)

Δ U

- 742.24 k J m o l^{- 1} .

Δ H_{298 K}

N H_{2} C N (s) + \frac{3}{2} O_{2} (g) \to N_{2} (g) + O_{2} (g) + H_{2} O (l)

{kJ mol}^{- 1}

R = 8.314 J {mol}^{- 1} K^{- 1}]

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