Answer : The enthalpy change for the reaction is 1043 kJ/mol.
Explanation :
The given chemical reaction is:
As we know that:
The enthalpy change of reaction = E(bonds broken) - E(bonds formed)
![\Delta H=[(2\times B.E_{C\equiv O})+(1\times B.E_{O\equiv O})]-[2\times B.E_{C=O}]](https://tex.z-dn.net/?f=%5CDelta%20H%3D%5B%282%5Ctimes%20B.E_%7BC%5Cequiv%20O%7D%29%2B%281%5Ctimes%20B.E_%7BO%5Cequiv%20O%7D%29%5D-%5B2%5Ctimes%20B.E_%7BC%3DO%7D%5D)
Given:
= 1074 kJ/mol
= 499 kJ/mol
= 802 kJ/mol
Now put all the given values in the above expression, we get:
![\Delta H=[(2\times 1074kJ/mol)+(1\times 499kJ/mol)]-[2\times 802kJ/mol]](https://tex.z-dn.net/?f=%5CDelta%20H%3D%5B%282%5Ctimes%201074kJ%2Fmol%29%2B%281%5Ctimes%20499kJ%2Fmol%29%5D-%5B2%5Ctimes%20802kJ%2Fmol%5D)
Therefore, the enthalpy change for the reaction is 1043 kJ/mol.
Answer:
Helium
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When the temperature rises some materials experience thermal expansion which means they get bigger, so it may make them harder to close because they don't fit as well.
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