CaC2 (s) + 2 H20 (g) -> Ca(OH)2 (s) + C2H2 (g)
The complete reaction of 22.7 g of CaC2 requires consumption of ________g of H2O.
I did 22.7 g CaC2* (2/64 mols CaC2) = .709
Right?!?!
You are correct that the reaction consumed 0.709 mols H2O; however, the problem asked for grams.
To determine the grams of H2O required for the complete reaction of 22.7 g of CaC2, you can follow these steps:
1. Begin by calculating the molar mass of CaC2:
- Ca: 40.08 g/mol
- C: 12.01 g/mol
- Total molar mass of CaC2: 40.08 g/mol + 2(12.01 g/mol) = 64.10 g/mol
2. Use the molar mass of CaC2 to convert the given mass of CaC2 into moles:
- Moles of CaC2 = 22.7 g CaC2 * (1 mol CaC2 / 64.10 g CaC2)
3. Based on the balanced chemical equation, the stoichiometric ratio between CaC2 and H2O is 1:2. This means that 1 mol of CaC2 reacts with 2 moles of H2O.
4. Use the mole-to-mole ratio to find the number of moles of H2O:
- Moles of H2O = Moles of CaC2 * (2 mol H2O / 1 mol CaC2)
5. Finally, convert the moles of H2O into grams by multiplying it by the molar mass of H2O:
- Grams of H2O = Moles of H2O * Molar mass of H2O
Plug in the values to calculate the exact grams of H2O required for the complete reaction of 22.7 g of CaC2.