ΔH = +572 kJ for the decomposition of water by the reaction 2 H₂O( )→ 2 H₂(g)+ O₂(g).How many grams of water can be decomposed by 5.00 × 10³ kJ of energy?

Question

Quizplus · Accepted Answer

Using the given value of ΔH and stoichiometry of the reaction, we can calculate the amount of heat required to decompose one mole (18 g) of water:

ΔH = 2 mol x 286 kJ/mol = 572 kJ

We can use this conversion factor to determine the amount of water that can be decomposed by 5.00 × 10³ kJ:

5.00 × 10³ kJ x (1 mol/286 kJ) x (18 g/mol) = 315 g

Therefore, the answer is B, 315 g.

ΔH = +572 KJ for the Decomposition of Water by the Reaction