Given (in kJ mol^-1): C(gr) + O2(g) -> CO2(g), Delta H=-393.5; CO(g) + 1/2 O2(g) -> CO2(g), Delta H=-283.0; H2(g) + 1/2 O2(g) -> H2O(l), Delta H=-285.8; H2O(l) -> H2O(g), Delta H=+44.0. Select the correct statement(s).

C(gr) + H2O(g) -> CO(g) + H2(g) has Delta H=+131.3

CO(g) + H2O(g) -> CO2(g) + H2(g) has Delta H=+41.2

The heat released on burning one mole of H2 to H2O(g) is 285.8

JEE Advanced levelOne or more correct optionsDifficulty 3 of 3td153

Given (in $kJ mo l^{- 1}$ ): $C (gr) + O X_{2} (g) CO X_{2} (g)$ , $Δ H = - 393.5$ ; $CO (g) + \frac{1}{2} O X_{2} (g) CO X_{2} (g)$ , $Δ H = - 283.0$ ; $H X_{2} (g) + \frac{1}{2} O X_{2} (g) H X_{2} O (l)$ , $Δ H = - 285.8$ ; $H X_{2} O (l) H X_{2} O (g)$ , $Δ H = + 44.0$ . Select the correct statement(s).

A $Δ_{f} H (CO (g)) = - 110.5$
B $C (gr) + H X_{2} O (g) CO (g) + H X_{2} (g)$ has $Δ H = + 131.3$
C $CO (g) + H X_{2} O (g) CO X_{2} (g) + H X_{2} (g)$ has $Δ H = + 41.2$
DThe heat released on burning one mole of $H X_{2}$ to $H X_{2} O (g)$ is $285.8$

Δ_{f} H (CO) = - 393.5 - (- 283.0) = - 110.5

(true).

Δ_{f} H (H X_{2} O (g)) = - 285.8 + 44.0 = - 241.8

. The water-gas reaction:

- 110.5 - (- 241.8) = + 131.3

(true). The shift reaction:

- 393.5 - (- 110.5 - 241.8) = - 41.2

, not

+ 41.2

(false). Burning

H X_{2}

to steam releases

241.8

, not

285.8

(false).