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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

Verified Answer :

MissPhiladelphia

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. 

27.0 g CH3OH(g) (1 mol/ 32.05g) = 0.84 mol CH3OH(g)
ΔH =+252.8kJ = Q = 0.84 mol (252.8kJ) = 213 kJ

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 \(CH_3OH\).

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

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

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