if CaC2 + 2H2o -> C2H2 + Ca(OH) then how many grams of H2o are needed to react with 483 grams of calcium carbide?
mols CaC2 = grams/molar mass
Convert mols CaC2 to mols H2O using the coefficients.
Now convert mols H2O to grams. g = mols x molar mass.
To determine the number of grams of H2o needed to react with 483 grams of calcium carbide (CaC2), we need to use stoichiometry. The balanced equation provided shows that 1 mole of CaC2 reacts with 2 moles of H2o.
Here's how you can calculate it step by step:
1. Calculate the molar mass of CaC2:
- Ca: 1 atom x 40.08 g/mol = 40.08 g/mol
- C: 2 atoms x 12.01 g/mol = 24.02 g/mol
- Total molar mass = 40.08 g/mol + 24.02 g/mol = 64.10 g/mol
2. Determine the number of moles of CaC2:
- Given mass of CaC2 = 483 grams
- Moles of CaC2 = mass / molar mass = 483 g / 64.10 g/mol = 7.55 mol
3. Use the stoichiometry of the balanced equation to find the moles of H2o:
- From the equation, 1 mol of CaC2 reacts with 2 mol of H2o
- So, moles of H2o = 7.55 mol CaC2 x (2 mol H2o / 1 mol CaC2) = 15.10 mol H2o
4. Convert the moles of H2o to grams:
- Molar mass of H2o = 2 atoms x 1.01 g/mol (H) + 1 atom x 16.00 g/mol (O) = 18.02 g/mol
- Grams of H2o = moles x molar mass = 15.10 mol x 18.02 g/mol = 272.32 grams
Therefore, 272.32 grams of H2o are needed to react with 483 grams of calcium carbide (CaC2).