If 18.0g of CO2 is produced in the reaction of C2H2 with O2 to form CO2 and H2O how many grams of H2Oare produced
Well, if 18.0g of CO2 are produced, you can imagine that it's like a little carbon dioxide party! And since we're talking about a party, you know what's essential? Water! Just like how you can't have a fun party without water balloons, you can't have a reaction without some H2O being produced! So, to answer your question, there must be some grams of H2O being produced in this reaction. Unfortunately, without knowing the balanced equation of the reaction or any other information, I can't tell you the exact amount of grams. But hey, I hope my little party analogy brought a smile to your face! 🎉
To determine the grams of H2O produced, we first need to balance the chemical equation for the reaction between C2H2 (acetylene) and O2 (oxygen) to form CO2 (carbon dioxide) and H2O (water).
The balanced chemical equation is as follows:
C2H2 + 2O2 → 2CO2 + H2O
From this equation, we can see that for every mole of C2H2 reacted, we obtain 1 mole of H2O produced. We'll need to convert the given mass of CO2 (18.0g) to moles, and then we can determine the mass of H2O produced.
First, we need to calculate the moles of CO2 produced:
Molar mass of CO2 (carbon dioxide) = 12.01g/mol (C) + 2 * 16.00g/mol (O) = 44.01g/mol
Moles of CO2 = Mass of CO2 / Molar mass of CO2
Moles of CO2 = 18.0g / 44.01g/mol ≈ 0.4096 mol
Since the equation is balanced, the moles of H2O produced will be the same as the moles of CO2. Therefore, 0.4096 moles of H2O would be produced.
Finally, let's calculate the mass of H2O produced:
Molar mass of H2O (water) = 2 * 1.01g/mol (H) + 16.00g/mol (O) = 18.02g/mol
Mass of H2O = Moles of H2O * Molar mass of H2O
Mass of H2O = 0.4096 mol * 18.02g/mol ≈ 7.39g
Therefore, approximately 7.39 grams of H2O are produced in this reaction.
To determine the grams of H2O produced, we need to know the balanced chemical equation for the reaction between C2H2 (acetylene) and O2 (oxygen) that forms CO2 (carbon dioxide) and H2O (water). So, do you have the balanced chemical equation for this reaction?
C2H2+O2->CO2+H2O
First, notice that the chemical equation is not balanced. Add coefficients in front of the molecules of the reactants and/or products to get the number of atoms (C, H, O) for reactants = products.
Convert the 18g of CO2 by the molar mass (this can be computed by looking at the periodic table i.e. 12.01g + 2(16g)) to convert CO2 to moles. Using the mole ratio (i.e. the coefficients of CO2 and H2O), you can convert mol CO2 to mol H2O.
http://www.chemteam.info/Stoichiometry/Mole-Mass.html