Water forms according to the equation below:

2H2 (g) + O2 (g) - > 2H2O (g) ΔHrxn = - 483.64 kJ

How much energy is released during the formation of 1 mol H2O (g) ?

__kJ

Question

Rosy

Chemistry

20 January, 07:53

Water forms according to the equation below:

2H2 (g) + O2 (g) - > 2H2O (g) ΔHrxn = - 483.64 kJ

How much energy is released during the formation of 1 mol H2O (g) ?

__kJ

+1

Answers (1)

Know the Answer?

Puck · Answer 1

241.82 kJ is released

Explanation:

The reaction indicates that 483.64 kJ of energy is released when TWO moles of H2O (g) is formed. You're looking to find the amount of energy released when only ONE mole of H2O forms, so that would be half the amount of energy released in the reaction (as one mole is a half of two).

483.64 / 2 = 241.82 kJ

So, your answer would be 241.82 kJ is released.

Water forms according to the equation below:2H2 (g) + O2 (g) - > 2H2O (g) ΔHrxn = - 483.64 kJHow much energy is released during the formation of 1 mol H2O (g) ?__kJ

Water forms according to the equation below:

2H2 (g) + O2 (g) - > 2H2O (g) ΔHrxn = - 483.64 kJ

How much energy is released during the formation of 1 mol H2O (g) ?

__kJ