Calculate Delta H in kJ for the following rea | vedclass

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(A) Given equations:$(i) \ H_2O_{(g)} + C_{(g)} \longrightarrow CO_{(g)} + H_{2(g)} ; \Delta H = +131 \ kJ$$(ii) \ CO_{(g)} + \frac{1}{2} O_{2(g)} \lo

Vedclass · Accepted Answer

$-393$

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(A) Given equations:$(i) \ H_2O_{(g)} + C_{(g)} \longrightarrow CO_{(g)} + H_{2(g)} ; \Delta H = +131 \ kJ$$(ii) \ CO_{(g)} + \frac{1}{2} O_{2(g)} \longrightarrow CO_{2(g)} ; \Delta H = -282 \ kJ$$(iii) \ H_{2(g)} + \frac{1}{2} O_{2(g)} \longrightarrow H_2O_{(g)} ; \Delta H = -242 \ kJ$To find $\Delta H$ for $C_{(g)} + O_{2(g)} \longrightarrow CO_{2(g)}$,add equations $(i)$,$(ii)$,and $(iii)$:$(H_2O_{(g)} + C_{(g)} + CO_{(g)} + \frac{1}{2} O_{2(g)} + H_{2(g)} + \frac{1}{2} O_{2(g)})$ $\longrightarrow (CO_{(g)} + H_{2(g)} + CO_{2(g)} + H_2O_{(g)})$Canceling common species on both sides gives:$C_{(g)} + O_{2(g)} \longrightarrow CO_{2(g)}$The enthalpy change is the sum of the individual enthalpy changes:$\Delta H = (+131) + (-282) + (-242) \ kJ$$\Delta H = 131 - 524 \ kJ = -393 \ kJ$

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