The run of cyanamide NH2CN with dioxygen was carried out in a bomb calorie meter and - u was found to be - 742-7 kJ-mol-Calculate the enthalpy for the reaction at 298 K NH2CN s - 3-2O2-N2 - CO2 - H2O

[ Δ U = #160; 742.71 KJ/mol; Δ H = Δ U + Δn_gRT ] NH_2CN( s ) + 3/2O_2→N_2 + CO_2 + H_2O [ Δn_g = 2 ...

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Standard XII

Chemistry

Enthalpy of Solution

The run of cy...

Question

The run of cyanamide $N H_{2} C N$ with dioxygen was carried out in a bomb calorie meter and $Δ u$ was found to be $- 742.7 k J / m o l$ .
Calculate the enthalpy for the reaction at $298$ K
$N H_{2} C N (s) + \frac{3}{2} O_{2} \to N_{2} + C O_{2} + H_{2} O$

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Solution

$\begin{matrix} Δ U = - 742.71 K J / m o l Δ H = Δ U + Δ n_{g} R T \end{matrix}$
$N H_{2} C N (s) + \frac{3}{2} O_{2} \to N_{2} + C O_{2} + H_{2} O$
$\begin{matrix} Δ n_{g} = 2 - \frac{3}{2} = \frac{1}{2} Δ H = 742.71 + \frac{1}{2} \times 8.314 \times 298 \times 10^{- 3} = - 74.47 K J / m o l \end{matrix}$

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

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The run of cyanamide NH2CN with dioxygen was carried out in a bomb calorie meter and Δu was found to be −742.7kJ/mol.Calculate the enthalpy for the reaction at 298 KNH2CN(s)+32O2→N2+CO2+H2O

ΔU=−742.71KJ/molΔH=ΔU+ΔngRTNH2CN(s)+32O2→N2+CO2+H2OΔng=2−32=12ΔH=742.71+12×8.314×298×10−3=−74.47KJ/mol

The run of cyanamide $N H_{2} C N$ with dioxygen was carried out in a bomb calorie meter and $Δ u$ was found to be $- 742.7 k J / m o l$ .
Calculate the enthalpy for the reaction at $298$ K
$N H_{2} C N (s) + \frac{3}{2} O_{2} \to N_{2} + C O_{2} + H_{2} O$