What mass of acetylene, C2H2, will be produced for the reaction of 90.g of calcium carbide, CaC2, with water in the following reacion?
CaC2(s) + 2H20(l) ---> C2H2(g) + Ca(OH)2(s)
To calculate the mass of acetylene (C2H2) produced in the given reaction, we need to use stoichiometry. The balanced equation provides the molar ratio between calcium carbide (CaC2) and acetylene (C2H2).
Let's follow these steps to find the mass of acetylene produced:
Step 1: Determine the molar mass of CaC2.
The molar mass of CaC2 can be calculated by adding up the atomic masses of its constituents:
Ca: 40.08 g/mol
C: 12.01 g/mol
Total molar mass of CaC2 = (40.08 g/mol) + 2 * (12.01 g/mol) = 64.1 g/mol
Step 2: Convert the given mass of CaC2 to moles.
We are given the mass of CaC2, which is 90.0 g. To convert this mass to moles, we can use the molar mass calculated in Step 1:
Moles of CaC2 = mass / molar mass = 90.0 g / 64.1 g/mol ≈ 1.402 mol
Step 3: Use the stoichiometric ratio to calculate the moles of C2H2 produced.
From the balanced equation, we can see that the molar ratio between CaC2 and C2H2 is 1:1. This means that 1 mole of CaC2 will produce 1 mole of C2H2. Therefore, the number of moles of C2H2 produced is also 1.402 mol.
Step 4: Convert the moles of C2H2 to mass.
To convert moles of C2H2 to grams, we need to use its molar mass:
Molar mass of C2H2 = (2 * 12.01 g/mol) + (2 * 1.008 g/mol) ≈ 26.04 g/mol
Mass of C2H2 produced = moles of C2H2 * molar mass of C2H2
= 1.402 mol * 26.04 g/mol ≈ 36.52 g
Therefore, approximately 36.52 g of acetylene (C2H2) will be produced in the given reaction.