the decomposition of methanol, ch₃oh(g), to form ch₄(g) and o₂(g) absorbs 252.8 kj of heat per mole of…

the decomposition of methanol, ch₃oh(g), to form ch₄(g) and o₂(g) absorbs 252.8 kj of heat per mole of oxygen formed. write a balanced thermochemical equation for this reaction.\na 2 ch₃oh(g) → 2 ch₄(g) + o₂(g) δh = +252.8 kj\nb 2 ch₄oh(g) → 2 ch₄(g) + o₂(g) δh = +252.8 kj\nc ch₃oh(g) → ch₄(g) + o₂(g) δh = -252.8 kj\nd 2 ch₃oh(g) → 2 ch₄(g) + o₂(g) δh = -252.8 kj

the decomposition of methanol, ch₃oh(g), to form ch₄(g) and o₂(g) absorbs 252.8 kj of heat per mole of oxygen formed. write a balanced thermochemical equation for this reaction.\na 2 ch₃oh(g) → 2 ch₄(g) + o₂(g) δh = +252.8 kj\nb 2 ch₄oh(g) → 2 ch₄(g) + o₂(g) δh = +252.8 kj\nc ch₃oh(g) → ch₄(g) + o₂(g) δh = -252.8 kj\nd 2 ch₃oh(g) → 2 ch₄(g) + o₂(g) δh = -252.8 kj

Answer

Explanation:

Step1: Determine the reaction type

It's an endothermic reaction as heat is absorbed, so $\Delta H> 0$.

Step2: Balance the chemical equation

The balanced equation for the decomposition of methanol to methane and oxygen is $2\mathrm{CH_3OH(g)}\rightarrow2\mathrm{CH_4(g)}+\mathrm{O_2(g)}$. And since 252.8 kJ of heat is absorbed per mole of oxygen formed, $\Delta H = + 252.8\mathrm{kJ}$.

Answer:

A. $2\mathrm{CH_3OH(g)}\rightarrow2\mathrm{CH_4(g)}+\mathrm{O_2(g)}\ \Delta H = +252.8\mathrm{kJ}$