What is the change in energy, in kJ, when 45.3 grams of methanol, CH3OH, combusts? 2\text{CH}_3\text{OH}\left(l\right) + 3\text{O}_2\left(g\right)\rightarro w2\text{CO}_2\left(g\right)+4\text{ H}_2\text{O}\left(g\right)\hskip .5in \Delta\text{H}=-726\text{ kJ}2 CH 3 OH ( l ) + 3 O 2 ( g ) → 2 CO 2 ( g ) + 4 H 2 O ( g ) Δ H = − 726 kJ Group of answer choices -513 kJ +2,050 kJ -1,030 kJ -2,050 kJ +513 kJ

-1,030 kJ

Explanation:

To calculate the number of moles we use the equation:

    .....(1)

Putting values in equation 1, we get:

The balanced chemical reaction is:

Given :

Energy released when 1 mole of combusts = 726k J

Thus Energy released when 1.42 moles of combusts =  

Thus 1030 kJ of heat is released and as is negative for exothermic reaction,

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