The heats of combustion of graphite and carbon monoxide, respectively are, - text 393.5 text kJ text mol-1 and -283 text kJ text mol-1 . Therefore, the heat of formation of carbon monoxide in, kJ text mol-1 is:

Question

The heats of combustion of graphite and carbon monoxide, respectively are, - text 393.5 text kJ text mol-1 and -283 text kJ text mol-1 . Therefore, the heat of formation of carbon monoxide in, kJ text mol-1 is: (A) 172.5 (B)  -110.5  (C)  -1070  (D)  -676.5

Tardigrade Admin · Accepted Answer

Combustion of graphite is as follows: C(s)+O2(g) xrightarrow[]CO2(g)+393.5 kJ ...(i) Combustion of carbon monoxide is, CO(g)+(1/2)(g) xrightarrow[]CO2(g)+283 kJ ...(ii) For obtaining CO as a product we reverse the Eq. (ii) as CO2(g) xrightarrow[]CO(g)+(1/2)O2(g)-283 kJ ...(iii) C(g)+O2(g) xrightarrow[]CO2(g)+393.5 kJ ...(iv) On adding Eq. (i) and Eq. (iii) C+(1/2)O2 xrightarrow[]CO+(393.5-283) =+110.5 text kJ ∴ Heat of formation of CO is =+ text 110.5 text kJ ∴ Δ H=-110.5 text kJ

Q. The heats of combustion of graphite and carbon monoxide, respectively are, $- 393.5 k J m o l^{- 1}$ and $- 283 k J m o l^{- 1}$ . Therefore, the heat of formation of carbon monoxide in, $k J m o l^{- 1}$ is:

172.5

$- 110.5$

$- 1070$

$- 676.5$

110.5

Q. The heats of combustion of graphite and carbon monoxide, respectively are, −393.5kJmol−1 and −283kJmol−1 . Therefore, the heat of formation of carbon monoxide in, kJmol−1 is:

172.5

−110.5

−1070

−676.5

110.5

Q. The heats of combustion of graphite and carbon monoxide, respectively are, $- 393.5 k J m o l^{- 1}$ and $- 283 k J m o l^{- 1}$ . Therefore, the heat of formation of carbon monoxide in, $k J m o l^{- 1}$ is:

$- 110.5$

$- 1070$

$- 676.5$