I need help on solving: How many grams of water are obtained if 487.8 grams of carbon dioxide are formed?
You have pieces of a problem but not a complete one. Repost with a complete problem; perhaps someone can help.
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To solve this problem, you need to understand the stoichiometry of the chemical reaction involved. In this case, we're given the mass of carbon dioxide and need to calculate the mass of water produced.
First, let's write the balanced equation for the reaction:
C + O2 → CO2
As per the equation, one mole of carbon dioxide (CO2) is formed from one mole of carbon (C). Now, we need to determine the molar mass of CO2. Carbon (C) has a molar mass of approximately 12.01 g/mol, and oxygen (O2) has a molar mass of approximately 32.00 g/mol (16.00 g/mol per oxygen atom). Adding these masses together, we find that the molar mass of CO2 is approximately 44.01 g/mol.
To convert grams of CO2 to moles, divide the given mass by the molar mass of CO2:
487.8 g CO2 / 44.01 g/mol ≈ 11.09 mol CO2
According to the stoichiometry of the balanced equation, one mole of CO2 produces one mole of water (H2O). Therefore, the number of moles of water formed is also 11.09 mol.
Finally, to convert moles of water to grams, multiply the number of moles by the molar mass of water. The molar mass of water (H2O) is approximately 18.02 g/mol (2 x 1.01 g/mol for hydrogen + 16.00 g/mol for oxygen):
11.09 mol H2O x 18.02 g/mol ≈ 199.90 g H2O
Therefore, approximately 199.90 grams of water are obtained when 487.8 grams of carbon dioxide are formed.