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Question

The equation for the combustion of glucose is: C6H12O6(s)+6O2(g)6CO2(g)+6H2O(g). How many grams of H2O will be produced when 8.064g of glucose is burned?


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Solution

Step 1: Combustion reaction :

  • It refers to an exothermic chemical reaction that has a high temperature.
  • It happens between a fuel and an oxidant.
  • A combustion reaction in a fire produces a flame, and the heat emitting can thus make it self-sustaining.
  • A combustion reaction is often a complicated sequence of elementary radical reactions.

Step 2: Given information:

  • The amount of glucose is 8.064g.
  • The molar mass of glucose is 180.15588gmol-1.
  • The molar mass of water is 18.01528gmol-1.

Step 3: Balanced chemical equation:

The equation for the combustion of glucose is given as:

C6H12O6(s)+6O2(g)6CO2(g)+6H2O(g)

Step 4: Calculation of the amount of water:

The following conversion will take place;

8.064gofC6H12O6×1molofC6H12O6180.15588gmol-1ofC6H12O6×6molofH2O1molofC6H12O6×18.01528gmol-1ofH2O1molofH2OOncancelling,theamountofwateris:=4.838gofH2O

Thus, approximately 0.8g water will produce.


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