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Thermodynamic Processes

Consider the ...

Question

Consider the following sequence of reactions
Which of the following is always true?

Δ H_{1} = Δ H_{2} + Δ H_{3} + Δ H_{4}

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Δ H_{2} = Δ H_{1} + Δ H_{3} + Δ H_{4}

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Δ H_{3} = Δ H_{1} + Δ H_{2} + Δ H_{4}

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Δ H_{4} = Δ H_{1} + Δ H_{2} + Δ H_{3}

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Solution

The correct option is B $Δ H_{2} = Δ H_{1} + Δ H_{3} + Δ H_{4}$
Solution:- (B) $Δ H_{2} = Δ H_{1} + Δ H_{3} + Δ H_{4}$
According to Hess's Law, regardless of the multiple stages or steps of a reaction, the total enthalpy change for the reaction is the sum of all changes.
Hence,
$Δ H_{2} = Δ H_{1} + Δ H_{3} + Δ H_{4}$

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Similar questions

O_{(g)} + e^{-} \to O_{(g)}^{-}, Δ H_{1}

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C l_{(g)} + e^{-} \to C l_{(g)}^{-}, Δ H_{3}

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N H_{3} (g) + 3 C l_{2} (g) ⇌ N C l_{3} (g) + 3 H C l (g); - Δ H_{1}

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N C l_{3}

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$N_{2 (g)} + 3 H_{2 (g)} \to 2 N H_{3 (g)}$ ; $Δ H_{2}$

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The heat of formation of $N C I_{3}$ in terms of $Δ H_{1}, Δ H_{2} a n d Δ H_{3}$ is

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C O (g) + \frac{1}{2} O_{2} (g) \to C O_{2} (g); Δ H_{2} = b

C (s) + C O_{2} (g) \to 2 C O (g); Δ H_{3} = c

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