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Properties of Enthalpy

Which of the ...

Question

Which of the following is an endothermic reaction?

2 H_{2} (g) + O_{2} (g) \to 2 H_{2} O (l)

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N_{2} (g) + O_{2} (g) \to 2 N O (g)

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N a O H (a q .) + H C l (a q .) \to N a C l (a q .) + H_{2} O (l)

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C_{2} H_{5} (a q .) + 3 O_{2} (g) \to 2 {C O}_{2} (g) + 3 H_{2} O (l)

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Solution

The correct option is B $N_{2} (g) + O_{2} (g) \to 2 N O (g)$
$N_{2} (g) + O_{2} (g) \to 2 N O (g)$ is an endothermic reaction because heat is absorbed in this reaction. All the other reactions are exothermic as the heat is released during the process.

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Similar questions

C (s) + O_{2} (g) \to C O_{2} (g); Δ H = - 394 k J / m o l

2 H_{2} (g) + O_{2} (g) \to 2 H_{2} O (l); Δ H = - 568 k J / m o l

C_{2} H_{5} O H (l) + 3 O_{2} (g) \to 2 C O_{2} (g) + 3 H_{2} O (l); Δ H = - 1058 k J / m o l

C (s) + O_{2} (g) \to C O_{2} (g)

Δ H = - 394

2 H_{2} (g) + O_{2} (g) \to 2 H_{2} O (l), Δ H = - 568

C_{2} H_{5} O H (l) + 3 O_{2} (g) \to 2 C O_{2} (g) + 3 H_{2} O (l)

Δ H = - 1058

Δ H \neq Δ U

N a O H (a q) + H C l (a q) ⟶ N a C l (a q) + H_{2} O (l)

B a (O H)_{2} + H_{2} S O_{4} (a q) ⟶ B a S O_{4} (s) + 2 H_{2} O (l)

2 H_{2} O (l) ⟶ 2 H_{2} (g) + O_{2} (g)

N_{2} (g) + 3 H_{2} (g) ⟶ 2 N H_{3} (g)

C a C O_{3} (s) ⟶ C a O (s) + C O_{2} (g)

N H_{3} (g) + C O_{2} (g) + H_{2} O (l) ⟶ N H_{4} H C O_{3} (a q)

0.10

N H_{4} H C O_{3}

H_{2} O (l)

\frac{y}{100}

y

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