Hydrogen gas (H2), methane gas (CH4), and a liquid called hexane (C6H14) all burn when lit with a match. They all combine with oxygen to produce carbon dioxide gas (CO2) and water (H2O) when they burn. Looking at these molecules, what conclusion can you draw about exergonic reactions?

It is observed that H2 gas gives out 286kJ/m, Methane gives out 802.3kJ/m and hexane gives out 4163kJ/m of heat. They are all exergonic or exothermic reaction but have different values of heat given out. The amount of carbon atom present, is what determines the heat given out, as higher carbon compound like Hexane gave out more heat than Methane and Hydrogen gas have out the least.

Explanation:

Hydrogen gas (H2), methane gas (CH4), and a liquid called hexane (C6H14) all burn when lit with a match. They all combine with oxygen to produce carbon dioxide gas (CO2) and water (H2O) when they burn. Looking at these molecules, what conclusion can you draw about exergonic reactions?

- During exergonic reactions, complex chemicals are converted into simple chemicals.

- During exergonic reactions, more energy is released than is put in as activation energy.

- During exergonic reactions, useful energy is lost in the form of heat.

- During exergonic reactions, organic compounds are converted into inorganic compounds.

- During exergonic reactions, nonpolar bonds are broken and polar bonds are created.

-During exergonic reactions, nonpolar bonds are broken and polar bonds are created.

Explanation:

Hydrogen, methane, hexane are high energy non polar bonds which when combusted, produces polar bond like water and co2 while giving out energy during reaction.

it would be b. 6co2 + 6h2o --> c6h12o6 + 6o2