How much heat is liberated by the combustion of 206 g of hydrogen? ΔHcomb = -286 kJ/mol
Answers
Answer:
When 206 g of Hydrogen undergoes complete combustion, 58916 KJ of heat is liberated.
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Explanation:
The heat of combustion is the amount of heat liberated when 1 mole of a substance is undergoes complete combustion in the presence of excess oxygen.
In simpler terms, it is the energy released per mole of substance undergoing combustion in the presence of excess oxygen.
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ΔHcomb = -286 kj/mol this means that for every mole of hydrogen that undergoes combustion, 286Kj of energy is liberated
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For us to get the amount of energy released/liberated when 206 g of hydrogen undergoes combustion, we need to find how many moles are in 206 g of H
Moles of 206 g of H
Moles = mass / molar mass
Molar mass of hydrogen is 1 gmol ⁻¹
Moles = 206g / 1 gmol ⁻¹
= 206 moles
Therefore, the numbers moles in 206 g of H is 206 moles
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⇒ We can then calculate the amount of heat liberated, If 1 mole of H liberates 286 Kj:
If 1 mole = 286 KJ
Then 206 moles = 286 KJ × 206moles/ 1 mole
= 58916 KJ
58916 KJ of heat is liberated when 206 g of Hydrogen is heated.