Ariel and Marcus know that when sugar burns it undergoes this reaction however they are not sure how much water is produced. Their teacher encourages them to think about the law of conservation of matter C6 H12 O6 +6co+ H20
The reaction you provided is not balanced, so we cannot determine the exact amount of water produced. However, we can still analyze the general concept of the law of conservation of matter.
The law of conservation of matter states that in a chemical reaction, matter cannot be created or destroyed. This means that the total mass of the reactants must equal the total mass of the products.
In the reaction you provided (although unbalanced), we can see that sugar (C6 H12 O6) reacts with oxygen (O2) to produce carbon dioxide (CO2) and water (H2O). The balanced equation would be:
C6 H12 O6 + 6O2 → 6CO2 + 6H2O
From this balanced equation, we can determine that for every 1 mole of C6 H12 O6, 6 moles of H2O are produced. This means that if we have a known mass or number of moles of sugar, we can calculate the mass or number of moles of water produced using stoichiometry.
However, without the balanced equation, we cannot accurately determine the exact amount of water produced from a given amount of sugar.
The law of conservation of matter states that matter cannot be created or destroyed in a chemical reaction, only transformed from one form to another. In the reaction you provided, sugar (C6H12O6) is burning in the presence of oxygen (O2) to produce carbon dioxide (CO2) and water (H2O).
The balanced equation for the reaction can be written as:
C6H12O6 + 6O2 -> 6CO2 + 6H2O
From the balanced equation, we can see that for every molecule of sugar (C6H12O6) that reacts, 6 molecules of water (H2O) are produced. Therefore, in this reaction, 6 molecules of water are formed for every molecule of sugar that burns.
To determine how much water is produced when sugar burns, we can analyze the chemical equation provided. Let me break it down for you:
C6H12O6 + 6O2 -> 6CO2 + 6H2O
This equation represents the combustion reaction of sugar (C6H12O6). When sugar burns, it reacts with oxygen (O2) to produce carbon dioxide (CO2) and water (H2O).
According to the balanced equation, for every 1 mole of sugar (C6H12O6) that reacts, 6 moles of water (H2O) are produced. Therefore, the ratio is 1:6, meaning that for every 1 molecule of sugar, 6 molecules of water are formed.
If Ariel and Marcus are given the amount of sugar they will be burning, they can use stoichiometry to determine the amount of water produced. Here's how they can do it:
1. Determine the amount of moles of sugar (C6H12O6) that will be burned. This can be done by dividing the given mass of sugar by its molar mass (180.16 g/mol).
2. Using the mole ratio from the balanced equation, multiply the moles of sugar by the mole ratio of water to sugar (6 moles of H2O / 1 mole of C6H12O6).
3. Convert the resulting moles of water to grams by multiplying by the molar mass of water (18.02 g/mol).
By following these steps, Ariel and Marcus will be able to calculate the amount of water produced when sugar burns.