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the complete oxidation of one mole of a sugar produces carbon dioxide and water. 2000 kj of heat is transferred from the system to the surroundings. the rearrangement of bonds as 0.5 moles of the sugar are oxidized generates heat in an open test tube (101 j•l–1pressure and 300 k temperature).

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Change in enthalpy is -1000kJ.

According to the first law of thermodynamics,

ΔU = q + w                    

w = 0.

Heat (q) generated by 0.5 mole of sugar = -2000 kJ

So, 1 mole of sugar will generate amount of heat is

     = -2000kJ * 0.5

     = -1000 kJ

So, putting the values into the formula

ΔU = q + w    

     = -1000 kJ + 0

     = -1000 kJ

Additionally, in accordance with the definition of enthalpy, enthalpy and internal energy have the following relationships.

ΔH = ΔU + PΔV

As change in volume is 0.

ΔH = ΔU

     = -1000 kJ

As a result, we may say that the system's change in enthalpy (ΔH) is -1000 kJ.

To learn more about enthalpy click the given link

https://brainly.com/question/14047927

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