The reaction of cyanamide displaystyle NH-2-CN-s- with dioxygen was carried out in a bomb calorimeter and displaystyle bigtriangleup U was found to be -742-7-kJ displaystyle mol-1- 298 K- displaystyle NH-2-CN-g-frac-3-2-O-2-g-rightarrow N-2-g-CO-2-g-H-2-O-l- Calculate enthalpy change the reaction 298 K-

Question

The reaction of cyanamide  displaystyle NH-2-CN-s-  with dioxygen was carried out in a bomb calorimeter and  displaystyle bigtriangleup U was found to be -742-7-kJ displaystyle mol-1-  298 K-  displaystyle NH-2-CN-g-frac-3-2-O-2-g-rightarrow N-2-g-CO-2-g-H-2-O-l- Calculate enthalpy change the reaction 298 K-

Toppr Admin · Accepted Answer

For given reaction-xA0-x394-n-1-1-x2212-1-5-0-5-x394-H-x394-U-x394-ngRT-x2212-742-7-0-5-xD7-8-314-xD7-10-x2212-3-xD7-298-x2212-742-7-1-2-x2212-741-5-xA0-kJ-xA0-mole-x2212-1

The reaction of cyanamide $N H_{2} C N (s)$ with dioxygen was carried out in a bomb calorimeter and $△ U$ was found to be $- 742.7 k J m o l^{- 1}$ at 298 K.
$N H_{2} C N (g) + \frac{3}{2} O_{2} (g) \to N_{2} (g) + C O_{2} (g) + H_{2} O (l)$

Calculate enthalpy change for the reaction at 298 K?

For given reaction, $Δ n = 1 + 1 - 1.5 = 0.5$ .

$Δ H = Δ U + Δ n_{g} R T$

$= - 742.7 + 0.5 \times 8.314 \times 10^{- 3} \times 298 = - 742.7 + 1.2 = - 741.5 k J m o l e^{- 1}$

The reaction of cyanamide NH2CN(s) with dioxygen was carried out in a bomb calorimeter and △U was found to be −742.7kJ mol−1 at 298 K. NH2CN(g)+32O2(g)→N2(g)+CO2(g)+H2O(l)Calculate enthalpy change for the reaction at 298 K?

For given reaction, Δn=1+1−1.5=0.5.ΔH=ΔU+ΔngRT=−742.7+0.5×8.314×10−3×298=−742.7+1.2=−741.5 kJ mole−1

The reaction of cyanamide $N H_{2} C N (s)$ with dioxygen was carried out in a bomb calorimeter and $△ U$ was found to be $- 742.7 k J m o l^{- 1}$ at 298 K.
$N H_{2} C N (g) + \frac{3}{2} O_{2} (g) \to N_{2} (g) + C O_{2} (g) + H_{2} O (l)$

Calculate enthalpy change for the reaction at 298 K?

For given reaction, $Δ n = 1 + 1 - 1.5 = 0.5$ .

$Δ H = Δ U + Δ n_{g} R T$

$= - 742.7 + 0.5 \times 8.314 \times 10^{- 3} \times 298 = - 742.7 + 1.2 = - 741.5 k J m o l e^{- 1}$