Question

Consider the following reaction:

2CH3OH(g)→2CH4(g)+O2(g)ΔH=+252.8kJ
Calculate the amount of heat transferred when 27.0g of CH3OH(g) is decomposed by this reaction at constant pressure.

If someone could help me with the steps I can figure it out on my own, thank you so much

Answer 1

Answer : The amount of heat transferred in the reaction is 213.4 kJ

Explanation :

Mass of
`CH_3OH` = 27.0 g

Molar mass of
`CH_3OH` = 32 g/mole

Enthalpy of reaction = +252.8 kJ

First we have to calculate the moles of
`CH_3OH`.

`\text{ Moles of }CH_3OH=\frac{\text{ Mass of }CH_3OH}{\text{ Molar mass of }CH_3OH}=(27.0g)/(32g/mole)=0.844moles`

Now we have to calculate the amount of heat transferred in the reaction.

The given balanced chemical reaction is:

`2CH_3OH(g)\rightarrow 2CH_4(g)+O_2(g)`

From the reaction, we conclude that

As, 2 moles of
`CH_3OH` transfer heat = 252.8 kJ

So, 0.844 moles of
`CH_3OH` transfer heat = 0.844 × (252.8 kJ)

= 213.4 kJ

Therefore, the amount of heat transferred in the reaction is 213.4 kJ