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At standard conditions, if the change in...

At standard conditions, if the change in the enthalpy for the following reaction is -109KJ`mol^(-1)`
`H_2(g) + Br_2(g) rarr 2HBr(g)`
Given that bond energy of `H_2 and Br_2` is 435kj`mol^(-1)` and 192kj`mol^(-1)`, respectively. What is the bond energy of HBr ?

A

368

B

736

C

518

D

259

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The correct Answer is:
A
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H_(2)(g) +(1)/(2)O_(2)(g) rarr H_(2)O(g) DeltaH =- 242 kJ mol^(-1) Bond energy of H_(2) and O_(2) is 436 and 500 kJ mol^(-1) , respectively. What is bond energy of O-H bond?

The net enthalpy change of a reaction is the amount of energy required to break all the bonds in reactant molecules minus amount of energy required to form all the bonds in the product molecules.What will be the enthalpy change for the following reaction. H_(2)(g) + Br_(2)(g) to 2HBr(g) Given that bond energy of H_(2), Br_(2) and HBr is 435 kJ mol^(-1) , 192 kJ mol^(-1) and 368 kJ mol^(-1) respectively.

Use the bond enthalpies listed below to estimate the enthalpy change for the reaction H_(2)(g)+Br_(2)(g)rarr2HBr(g) Given: BE of H_(2), Br_(2) , and HBr is 435, 192 , and 368 kJ mol^(-1) , respectively.

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