The reaction of cyanamide NH2CNs with oxygen was run in a bomb calorimeter and - U was found to be -742-24 kJ mol-1- The magnitude of - H298K for the reaction NH2CNs - 32O2g - N2g -O2g-H2Ol is kJ mol-1- Rounded off to the nearest integer-Assume ideal gases and R - 8-314 J mol-1 K-1-

NH_2CN(s) + 32O_2(g) → N_2(g) +O_2(g)+H_2O(l) Δ n_g=(1+1) 32=12 Δ H amp;=Δ U+Δ n_gRT amp;= 742.24+1/2× 8.314 × 298 ×11000 amp;= 742.24+1.24 ...

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Standard XII

Chemistry

Entropy

The reaction ...

Question

The reaction of cyanamide $N H_{2} C N (s)$ with oxygen was run in a bomb calorimeter and $Δ U$ was found to be $- 742.24 k J m o l^{- 1} .$ The magnitude of $Δ H_{298 K}$ for the reaction $N H_{2} C N (s) + \frac{3}{2} O_{2} (g) \to N_{2} (g) + O_{2} (g) + H_{2} O (l)$ is ______ ${kJ mol}^{- 1}$ . (Rounded off to the nearest integer).
[Assume ideal gases and $R = 8.314 J {mol}^{- 1} K^{- 1}]$

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Solution

$N H_{2} C N (s) + \frac{3}{2} O_{2} (g) \to N_{2} (g) + O_{2} (g) + H_{2} O (l)$
$Δ n_{g} = (1 + 1) - \frac{3}{2} = \frac{1}{2}$

$\begin{matrix} Δ H & = Δ U + Δ n_{g} R T = - 742.24 + \frac{1}{2} \times 8.314 \times 298 \times \frac{1}{1000} = - 742.24 + 1.24 = - 741 {kJ mol}^{- 1} \end{matrix}$

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Similar questions

Q. The reaction of cyanamide,

N H_{2} C N (s)

with oxygen was run in a bomb calorimeter and

Δ U

was found to be

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

.The magnitude of

Δ H_{298}

for the reaction

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

is ______ kJ. (Rounded off to the nearest integer)

[Assume ideal gases and $R = 8.314 J m o l^{- 1} K^{- 1}$ ]

The reaction of cyanamide, NH₂CN_(s),with dioxygen was carried out in a bomb calorimeter, and ΔU was found to be –742.7 kJ mol^–1at 298 K. Calculate enthalpy change for the reaction at 298 K.

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

Q. The reaction of cyanamide

N H_{2} C N (s)

with dioxygen was carried out in a bomb calorimeter and

Δ U

was found to be

- 742.7

k J m o l^{- 1}

298 K

. Calculate enthalpy change for the following reaction at

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)

Q. The reaction of cyanamide

(N H_{2} C N)

with dioxygen was carried out in a bomb calorimeter and

Δ U

was found to be

- 742.7 {kJmol}^{- 1}

298 K

. Calculate the enthalpy change for the reaction at

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)

Q. When the following reaction was carried out in a bomb calorimeter,

Δ U

is found to be

1742.7 k J / m o l

N H_{2} C N (s)

at 300 K.

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

Calculate

{Δ H}_{3000 K}

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

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NH2CN(s)+32O2(g)→N2(g)+O2(g)+H2O(l) Δng=(1+1)−32=12 ΔH=ΔU+ΔngRT=−742.24+12×8.314×298×11000=−742.24+1.24=−741 kJ mol−1