water forms according to the equation below: 2h₂(g) + o₂(g) → 2h₂o(g) δhᵣₓₙ = -483.64 kj. how much energy is…

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)?

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)?

Answer

Explanation:

Step1: Analyze reaction - energy relation

The given reaction $2H_2(g)+O_2(g)\rightarrow2H_2O(g)$ has $\Delta H_{rxn}=- 483.64\ kJ$. This means when 2 moles of $H_2O(g)$ are formed, 483.64 kJ of energy is released.

Step2: Calculate energy for 1 - mol $H_2O$

Let $x$ be the energy released when 1 mol of $H_2O(g)$ is formed. We set up a proportion: $\frac{-483.64\ kJ}{2\ mol\ H_2O}=\frac{x}{1\ mol\ H_2O}$. Solving for $x$, we get $x = \frac{-483.64}{2}=-241.82\ kJ$.

Answer:

-241.82 kJ