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garik1379 [7]
2 years ago
7

From the following data, calculate the average bond enthalpy for the NOH bond: NH3(g) ¡NH2(g) 1 H(g) ¢H° 5 435 kJ/mol NH2(g) ¡NH

(g) 1 H(g) ¢H° 5 381 kJ/mol NH(g) ¡N(g) 1 H(g) ¢H° 5 360 kJ/mol
Chemistry
1 answer:
Sphinxa [80]2 years ago
4 0

Answer:

The average bond enthalpy for the N-H bond is 392 kJ/mol.

Explanation:

NH_3(g) \rightarrow NH_2(g) +1 H(g),\Delta H^o_{1}= 435 kJ/mol..[1]

NH_2(g) \rightarrow NH(g) + H(g),\Delta H^o_{2}= 381 kJ/mol..[2]

NH(g) \rightarrow N(g)+ 1 H(g),\Delta H^o_{3}= 360 kJ/mol..[3]

On adding [1] , [2] and [3] , we get:

NH_3(g) \rightarrow N(g) +3H(g),\Delta H^o_{4}= ?

\Delta H^o_{4}=\Delta H^o_{1}+\Delta H^o_{2}+\Delta H^o_{3}

= 435 kJ/mol+381 kJ/mol +360 kJ/mol = 1,176 kJ/mol

There three bonds N-H bond sin ammonia. Then average bond enthalpy of single N-H bond is :

\Delta H^o_{N-H}=\frac{1,176 kJ/mol}{3}=392 kJ/mol

The average bond enthalpy for the N-H bond is 392 kJ/mol.

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From the statement of Hess' law, the enthalpy of the reaction A---> C is +90 kJ

<h3>What is Hess' law?</h3>

Hess' law of constant heat summation states that for a multistep reaction, the standard enthalpy of reaction is always constant and is independent of the pathway or intermediate routes taken.

From Hess' law, the enthalpy change for the reaction A ----> C is calculated as follows:

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Therefore, the enthalpy of the reaction A---> C is +90 kJ

The above reaction A---> C can be shown in the enthalpy diagram below:

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\ /

\ / (ΔH = +60 kJ)

(ΔH = +30 J) \ /

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Learn more about enthalpy and Hess law at: brainly.com/question/9328637

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