How many grams of water are needed to make at least 50.0g of C2H2 in this reaction?
CaC2 + 2H2O = Ca(OH)2 + C2H2
The numbers inside are suppose to be small but you can't do that on a laptop... Thanks
50g*1mol/26.04g*2molh20/1molC2H2*18.02g/1molh20
69.20g H20 needed to make 50g c2h2
To determine the amount of water needed to produce at least 50.0g of C2H2, we need to use the stoichiometry of the reaction.
First, let's determine the molar mass of C2H2 (acetylene).
The atomic mass of carbon (C) is 12.01 g/mol, and the atomic mass of hydrogen (H) is 1.01 g/mol. Since there are two carbons and two hydrogens in C2H2, the molar mass of C2H2 is:
(2 * 12.01 g/mol) + (2 * 1.01 g/mol) = 26.04 g/mol.
Next, we need to determine the stoichiometric ratio between C2H2 and H2O in the balanced equation.
From the balanced equation: CaC2 + 2H2O = Ca(OH)2 + C2H2, we can see that for every 1 mole of C2H2 produced, 2 moles of H2O are needed.
Now, we can calculate the amount of water needed to produce 50.0g of C2H2.
(1) Convert the given mass of C2H2 to moles:
moles of C2H2 = mass of C2H2 / molar mass of C2H2
moles of C2H2 = 50.0g / 26.04 g/mol ≈ 1.9226 moles of C2H2
(2) Use the stoichiometric ratio to find the moles of H2O:
moles of H2O = 2 * moles of C2H2
moles of H2O = 2 * 1.9226 ≈ 3.8452 moles of H2O
(3) Finally, convert the moles of water to grams:
mass of H2O = moles of H2O * molar mass of H2O
mass of H2O = 3.8452 moles * (2 * 1.01 g/mol) ≈ 7.7755 g of H2O
Therefore, at least 7.7755 grams of water are needed to produce 50.0 grams of C2H2 in this reaction.