Question

Water forms according to the equation below: 2H2(g) + O2(g) jpg 2H2O(g)

Hrxn = -483.64 kJ How much energy is released during the formation of 1 mol H2O(g)? kJ

Answer 1

2H2(g) + O2(g)=2H2O -483.64 kJ
2 mol. of H2O ----> -483.64 kJ
1 mol. of H2O ----> X


`x = (1 * - 483.64)/(2) = -241,82 \: kj`

Answer 2

Answer : The amount of energy released is, -241.82 KJ

Explanation : Given,

`\Delta H_(rxn)=-483.64KJ`

The balanced chemical reaction is,

`2H_2(g)+O_2(g)\rightarrow 2H_2O(g)`

From this we conclude that,

As, 2 moles of
`H_2O` released amount of energy = -483.64 KJ

So, 1 mole of
`H_2O` released amount of energy =
`(-483.64KJ)/(2)=-241.82KJ`

Therefore, the amount of energy released is, -241.82 KJ