The heat of formation of CO(g) and CO2 (g) are Δ H = -110 and Δ H = - 393 kJ mol-1 respectively. What is the heat of reaction (Δ H) (in kJ mol-1) for the following reaction ? CO(g)+ (1/2)O2(g) → CO2(g)

Question

The heat of formation of CO(g) and CO2 (g) are Δ H = -110 and Δ H = - 393 kJ mol-1 respectively. What is the heat of reaction (Δ H) (in kJ mol-1) for the following reaction ? CO(g)+ (1/2)O2(g) → CO2(g) (A) -283 (B) 504 (C) -504 (D) -142.5

Tardigrade Admin · Accepted Answer

C(s)+1/20 2(g) → CO(g) ; Δ H =-110 KJ/mol dots (1) C(s)+O2(g) → CO2(g); Δ H =-393 KJ/mol dots (2) or CO(g) → C(s)+1/2O2(g) ; Δ H=110 kJ/mol dots (3) Adding (2) and (3) CO(g)+1/2 O2(g) → CO2(g) Δ H=(-393+110)kJ =-283 kJ/mol

Q. The heat of formation of $C O_{(g)}$ and $C O_{2 (g)}$ are $Δ H = - 110$ and $Δ H = - 393 k J m o l^{- 1}$ respectively. What is the heat of reaction $(Δ H)$ (in $k J m o l^{- 1})$ for the following reaction ?
$C O_{(g)} + \frac{1}{2} O_{2 (g)} \to C O_{2 (g)}$

$- 283$

$504$

$- 504$

$- 142.5$

Q. The heat of formation of CO(g)​ and CO2(g)​ are ΔH=−110 and ΔH=−393kJmol−1 respectively. What is the heat of reaction (ΔH) (in kJmol−1) for the following reaction ? CO(g)​+21​O2(g)​→CO2(g)​

−283

504

−504

−142.5

C(s)​+1/202(g)​→CO(g)​;ΔH=−110KJ/mol…(1) C(s)​+O2(g)​→CO2(g)​;ΔH=−393KJ/mol…(2) or CO(g)​→C(s)​+1/2O2(g)​;ΔH=110kJ/mol…(3) Adding (2) and (3) CO(g)​+1/2O2(g)​→CO2(g)​ ΔH=(−393+110)kJ =−283kJ/mol

Q. The heat of formation of $C O_{(g)}$ and $C O_{2 (g)}$ are $Δ H = - 110$ and $Δ H = - 393 k J m o l^{- 1}$ respectively. What is the heat of reaction $(Δ H)$ (in $k J m o l^{- 1})$ for the following reaction ?
$C O_{(g)} + \frac{1}{2} O_{2 (g)} \to C O_{2 (g)}$

$- 283$

$504$

$- 504$

$- 142.5$