Δ Hfo of CO2(.g.),CO(.g.),N2O(.g.) and NO2(.g.) in kJ/mol are respectively -393,-110,81 and 34 . Calculate the Δ H in kJ of the following reaction 2NO2(.g.)+3CO(.g.) arrow N2O(.g.)+3CO2(.g.)

Question

Δ Hfo of CO2(.g.),CO(.g.),N2O(.g.) and NO2(.g.) in kJ/mol are respectively -393,-110,81 and 34 . Calculate the Δ H in kJ of the following reaction 2NO2(.g.)+3CO(.g.) arrow N2O(.g.)+3CO2(.g.) (A) 836 (B) 1460 (C) -836 (D) -1460

Tardigrade Admin · Accepted Answer

Δ Hr x n=1.Δ Hfo(.N2O,g.)+3.Δ Hfo(.CO2,g.)-[.2Δ Hfo(.NO2,g.)+3Δ Hfo(.CO,g.)]. =81kJ+3× (- 393) kJ-2[× 34 kJ + 3 (- 110 kJ)] =81-1179-68+330 kJ/mol =-836 kJ/mol

Q. $Δ H_{f}^{o}$ of $C O_{2} (g), CO (g), N_{2} O (g)$ and $N O_{2} (g)$ in kJ/mol are respectively $- 393, - 110, 81$ and $34$ . Calculate the $Δ H$ in kJ of the following reaction
$2 N O_{2} (g) + 3 CO (g) \to N_{2} O (g) + 3 C O_{2} (g)$

836

1460

-836

-1460

$Δ H_{r x n} = 1.Δ H_{f}^{o} (N_{2} O, g) + 3.Δ H_{f}^{o} (C O_{2}, g) - [2Δ H_{f}^{o} (N O_{2}, g) + 3Δ H_{f}^{o} (CO, g)]$
$= 81 k J + 3 \times (- 393) k J - 2 [\times 34 k J + 3 (- 110 k J)]$
$= 81 - 1179 - 68 + 330 k J / m o l$
$= - 836 k J / m o l$

Q. ΔHfo​ of CO2​(g),CO(g),N2​O(g) and NO2​(g) in kJ/mol are respectively −393,−110,81 and 34 . Calculate the ΔH in kJ of the following reaction 2NO2​(g)+3CO(g)→N2​O(g)+3CO2​(g)

836

1460

-836

-1460

ΔHrxn​=1.ΔHfo​(N2​O,g)+3.ΔHfo​(CO2​,g)−[2ΔHfo​(NO2​,g)+3ΔHfo​(CO,g)] =81kJ+3×(−393)kJ−2[×34kJ+3(−110kJ)] =81−1179−68+330kJ/mol =−836kJ/mol

Q. $Δ H_{f}^{o}$ of $C O_{2} (g), CO (g), N_{2} O (g)$ and $N O_{2} (g)$ in kJ/mol are respectively $- 393, - 110, 81$ and $34$ . Calculate the $Δ H$ in kJ of the following reaction
$2 N O_{2} (g) + 3 CO (g) \to N_{2} O (g) + 3 C O_{2} (g)$

$Δ H_{r x n} = 1.Δ H_{f}^{o} (N_{2} O, g) + 3.Δ H_{f}^{o} (C O_{2}, g) - [2Δ H_{f}^{o} (N O_{2}, g) + 3Δ H_{f}^{o} (CO, g)]$
$= 81 k J + 3 \times (- 393) k J - 2 [\times 34 k J + 3 (- 110 k J)]$
$= 81 - 1179 - 68 + 330 k J / m o l$
$= - 836 k J / m o l$