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2 years ago

Nitrogen dioxide, NO2(

Chemistry

2 answers:

Natasha_Volkova [10]2 years ago

7 0

Answer:84.6 kJ of energy released when 2.50 moles of nitrogen dioxide is decomposed.

Explanation:

$N(g)+O_2(g)\rightarrow NO_2(g),\Delta H_f=33.84 kJ/mol$

Energy released when 1 mole of $NO_2$ is formed = 33.84 kJ

And When 1 mole of $NO_2$ is decomposed it gives out 33.84 kJ of energy.

Energy released when 2.50 moles of nitrogen dioxide is decomposed:

$33.84 kJ\times 2.50 =84.6 kJ$

84.6 kJ of energy released when 2.50 moles of nitrogen dioxide is decomposed.

kirza4 [7]2 years ago

5 0

Answer:

Explanation:

took the test

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Answer:

Explanation:

The given overall reaction is as follows:

O 2 N N H ₂( a q ) k → N ₂O ( g ) + H ₂ O( l )

The reaction mechanism for this reaction is as follows:

O ₂ N N H ₂ ⇌ k 1 k − 1 O ₂N N H ⁻ + H ⁺ ( f a s t e q u i l i b r i u m )

O ₂ N N H − k ₂→ N ₂ O + O H ⁻ ( s l ow )

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The rate law of the reaction is given as follows:

k = [ O ₂ N N H ₂ ] / [ H ⁺ ]

The rate law can be determined by the slow step of the mechanism.

r a t e = k ₂ [ O ₂ N N H ⁻ ] . . . ( 1 )

Since, from the equilibrium reaction

k e q = [ O ₂ N N H ⁻ ] [ H ⁺ ] /[ O ₂ N N H ₂ ] = k ₁ /k − 1

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Substitituting the value of equation (2) in equation (1) we get.

r a t e = k ₂ k ₁/ k − 1 × [ O ₂ N N H ₂ ] /[ H ⁺ ]

Therefore, the overall rate constant is

k = k₂k₁/k-1

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2 years ago