If you want to produce 2.00 kg of ethylene glycol from the reaction of C2H4Cl2 and Na2CO3, what is the minimum amount of C2H4Cl2 that is needed? C2H4Cl2(l) + Na2CO3(s) + H2O(l)C2H6O2(l) + 2NaCl(aq) + CO2(g)
First, let's find the molar masses of the substances involved:
C2H4Cl2 = (2 * 12.01 g/mol) + (4 * 1.01 g/mol) + (2 * 35.45 g/mol) = 98.96 g/mol
C2H6O2 (ethylene glycol) = (2 * 12.01 g/mol) + (6 * 1.01 g/mol) + (2 * 16.00 g/mol) = 62.07 g/mol
Now, we use stoichiometry to find the amount of C2H4Cl2 needed to produce 2.00 kg (2000 g) of ethylene glycol:
1. Convert the mass of ethylene glycol to moles: moles of ethylene glycol = mass / molar mass
moles of ethylene glycol = 2000 g / 62.07 g/mol ≈ 32.22 moles
2. Use the balanced equation to relate moles of ethylene glycol to moles of C2H4Cl2:
1 mole of C2H4Cl2 → 1 mole of C2H6O2 (ethylene glycol)
32.22 moles of C2H4Cl2 → 32.22 moles of C2H6O2
3. Convert moles of C2H4Cl2 to grams: mass of C2H4Cl2 = moles * molar mass
mass of C2H4Cl2 = 32.22 moles * 98.96 g/mol ≈ 3188.84 g
The minimum amount of C2H4Cl2 needed to produce 2.00 kg of ethylene glycol is approximately 3188.84 grams.
To determine the minimum amount of C2H4Cl2 needed to produce 2.00 kg of ethylene glycol (C2H6O2), we'll need to use stoichiometry.
First, let's write out the balanced chemical equation for the reaction:
C2H4Cl2(l) + Na2CO3(s) + H2O(l) -> C2H6O2(l) + 2NaCl(aq) + CO2(g)
From the equation, we can see that for every 1 mole of C2H4Cl2, we can produce 1 mole of C2H6O2.
Next, we need to convert the given mass of ethylene glycol (2.00 kg) to moles.
The molar mass of ethylene glycol (C2H6O2) is:
C: 12.01 g/mol
H: 1.01 g/mol (x6)
O: 16.00 g/mol (x2)
So, the molar mass of C2H6O2 is 62.07 g/mol.
To convert the mass of C2H6O2 to moles, we'll use the equation:
moles = mass / molar mass
moles = 2000 g / 62.07 g/mol
moles = 32.23 mol
Since the stoichiometry of the reaction tells us that 1 mole of C2H4Cl2 produces 1 mole of C2H6O2, the minimum amount of C2H4Cl2 needed is also 32.23 moles.
Finally, to convert moles to grams, we'll use the molar mass of C2H4Cl2.
The molar mass of C2H4Cl2 is:
C: 12.01 g/mol
H: 1.01 g/mol (x4)
Cl: 35.45 g/mol (x2)
So, the molar mass of C2H4Cl2 is 98.96 g/mol.
Now, we can calculate the minimum amount of C2H4Cl2 needed:
mass = moles * molar mass
mass = 32.23 mol * 98.96 g/mol
mass = 3193.99 g
Therefore, the minimum amount of C2H4Cl2 needed to produce 2.00 kg of ethylene glycol is approximately 3194 g.
To determine the minimum amount of C2H4Cl2 needed to produce 2.00 kg of ethylene glycol (C2H6O2), we need to use stoichiometry and the balanced chemical equation for the reaction.
The balanced equation is:
C2H4Cl2(l) + Na2CO3(s) + H2O(l) → C2H6O2(l) + 2NaCl(aq) + CO2(g)
First, we need to determine the molar mass of ethylene glycol:
C = 12.01 g/mol
H = 1.01 g/mol
O = 16.00 g/mol
Molar mass of C2H6O2 = (2 * 12.01 g/mol) + (6 * 1.01 g/mol) + (2 * 16.00 g/mol) = 62.07 g/mol
Next, we calculate the number of moles of ethylene glycol required:
Number of moles = mass / molar mass
Number of moles = 2000 g / 62.07 g/mol = 32.22 mol
From the balanced equation, we can see that the stoichiometric ratio between C2H4Cl2 and C2H6O2 is 1:1. This means that for every 1 mol of C2H4Cl2, we will produce 1 mol of C2H6O2.
Therefore, the minimum amount of C2H4Cl2 needed will also be 32.22 mol.
To convert the moles of C2H4Cl2 to grams, we can use the molar mass of C2H4Cl2:
C = 12.01 g/mol
H = 1.01 g/mol
Cl = 35.45 g/mol
Molar mass of C2H4Cl2 = (2 * 12.01 g/mol) + (4 * 1.01 g/mol) + (2 * 35.45 g/mol) = 98.96 g/mol
Mass of C2H4Cl2 = number of moles * molar mass
Mass of C2H4Cl2 = 32.22 mol * 98.96 g/mol = 3185.1 g
Therefore, the minimum amount of C2H4Cl2 needed is approximately 3185.1 grams.