The O-H bond energy is 464 kJ/mol and the HI bond energy is 291 kJ/mol. Remembering that breaking any bond is an endothermic process and making any bond is exothermic, what is the net enthalpy change involved in the reaction between HI and H2O? Is this reaction endothermic or exothermic?

Explanation:

The reaction equation will be as follows.

In this reaction, breakage of hydrogen and chlorine bond takes place whereas the formation of O-H bond takes place.

Therefore, enthalpy of the reaction will be calculated as follows.

                        =

                       = 432 kJ/mol - 464 kJ/mol

                       = -32 kJ/mol

Negative sign indicates that heat is liberating.

Thus, we can conclude that the given reaction is exothermic in nature and net enthalpy change is 32 kJ/mol.

the ideal gas law equation is as follows

pv = nrt

where p - pressure

v - volume

n - number of moles

r - universal gas constant

t - temperature

so if the pressure, volume and temperature are already known

we are left with n and r

since r is the universal gas constant that has a known fixed value then r too is known

so we are left with 'n'

once we know temperature volume and pressure

we can find the number of moles of gas present using the ideal gas law equation

this is not my own answer, this is an answer for the same question by the user blahblahmali. i do not claim ownership of this account.