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Standard XII

Chemistry

Heat of Formation

If the enthal...

Question

If the enthalpy of formation of $H^{+} (g)$ is 1536 kJ/mole then determine the heat of formation of $H_{2}$ gas?

3072 kJ

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1536 kJ

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-1536 kJ

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-3072 kJ

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Solution

The correct option is D 0
$H \to H^{+} + e^{-}$ $Δ_{f o r m a t i o n} H_{(H^{+})} = + 1536 k J / m o l e$
$H + e^{-} \to H^{-}$ $Δ_{f o r m a t i o n} H_{(H^{-})} = - 1536 k J / m o l e$
On adding both these equation ;
$2 H + e^{-} \to H_{2} + e^{-}$
or $2 H \to H_{2}$ $Δ_{f o r m a t i o n} H_{(H^{+})} + Δ_{f o r m a t i o n} H_{(H^{-})} = + 1536 - 1536 = 0$

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If the enthalpy of formation of H+(g) is 1536 kJ/mole then determine the heat of formation of H2 gas?

The correct option is D 0H→H++e− ΔformationH(H+)=+1536kJ/moleH+e−→H− ΔformationH(H−)=−1536kJ/moleOn adding both these equation ; 2H+e−→H2+e−or 2H→H2 ΔformationH(H+)+ΔformationH(H−)=+1536−1536=0

If the enthalpy of formation of $H^{+} (g)$ is 1536 kJ/mole then determine the heat of formation of $H_{2}$ gas?