Question

If instead of the theoretical 2 mol, the actual reaction uses reaction (8.29x10^2) grams of methanol (CH3OH), how much energy does the reaction produce? The correct answer must have 3 SIGNIFICANT FIGURES and use unit symbols whenever applicable.

Answer 1

Suppose the quantity of enerny in the theoritical reaction of 2 mole methanol is x J.

To calculate the amount of energy which is produce by 8.29x10^2 grams of methanol first determine the number of moles of methanol in this amount by its molar mass:

Molar mass of methanol = 32.04 g / mol

Number of methanol = 8.29x10^2 grams / 32.04 g / mol = 25.9 mol

If the quantity of enerny in the theoritical reaction of 2 mole methanol = x J

the quantity of enerny in the theoritical reaction of 25.9 mole methanol = 25.9 *x J

hence the amount of energy which is produce by 8.29x10^2 grams of methanol is 25.9 times of the energy when theoretical 2 mol of methanol is participated in the reaction.