To find out how many grams of oxygen were consumed in the burning process, we can use the law of conservation of mass, which states that the mass of reactants (in this case, the paper and the oxygen) must equal the mass of the products (ash, carbon dioxide, and water).
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Calculate the total mass of the products:
- Ash: 10.2 grams
- Carbon dioxide: 98.1 grams
- Water: 45.6 grams
Adding these together: \[ \text{Total mass of products} = 10.2 + 98.1 + 45.6 = 153.9 \text{ grams} \]
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Now, set up the equation for the mass of reactants: The mass of the reactants (paper + oxygen) must equal the total mass of products. Let \( x \) be the mass of oxygen consumed.
The total mass of the reactants is then: \[ \text{Mass of paper} + \text{Mass of oxygen} = 115.6 + x \]
According to the conservation of mass: \[ 115.6 + x = 153.9 \]
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Solve for \( x \): \[ x = 153.9 - 115.6 \] \[ x = 38.3 \text{ grams} \]
Thus, the mass of oxygen consumed in the burning process is 38.3 grams.
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