Question

Consider the chemical equations shown here.

Upper N Upper O (g) + Upper O Subscript 3 Baseline (g) right arrow Upper N Upper O Subscript 2 Baseline (g) + Upper O Subscript 2 Baseline (g) delta Upper H Subscript 1 Baseline = negative 198.9 kilojoules. StartFraction 3 Over 2 EndFraction Upper O Subscript 2 Baseline (g) right arrow Upper O Subscript 3 Baseline (g) delta Upper H Subscript 2 Baseline = 142.3 kilojoules. Upper O (g) right arrow one half Upper O Subscript 2 Baseline (g) delta Upper H Subscript 3 Baseline = negative 247.5 kilojoules.

What is Delta.Hrxn for the reaction shown below?

Upper n upper O (g) plus upper O (g) right arrow upper N upper O subscript 2 (g).

Answer 1

Answer:

-304.1

Explanation:

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Answer 2

The enthalpy change for the target reaction is obtained as -304.1 kJ.

What is Hess law?

The Hess law of constant heat summation states that; the heat of reaction can be obtained as the sum of the heat of several reactions.

In this case, the enthalpy change for the target reaction can be identified as; -198.9 + 142.3 + (-247.5) = -304.1 kJ.

Learn more about Hess law:https://brainly.com/question/14561923

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