4BF3+3H2O=H3BO3+3HBF4
if the reaction vessel contains 0.496 mol BF3 and 5.63g of H2O, which compound is the limiting reactant? how many molesof HBF4 can be produced?
good
To determine the limiting reactant, we need to compare the number of moles of each reactant.
Given:
- Moles of BF3: 0.496 mol
- Mass of H2O: 5.63 g
First, let's calculate the number of moles of H2O:
The molar mass of H2O is 18.015 g/mol.
Moles of H2O = (Mass of H2O) / (Molar mass of H2O)
= 5.63 g / 18.015 g/mol
≈ 0.312 mol
Now, let's compare the mole ratios of BF3 and H2O in the balanced equation:
From the balanced equation: 4BF3 + 3H2O → H3BO3 + 3HBF4
The mole ratio of BF3 to H2O is 4:3.
Using the mole ratios, we can determine which reactant is the limiting reactant.
Moles of BF3 / Mole ratio of BF3 to H2O = moles of H2O / Mole ratio of H2O to BF3
Plugging in the values, we get:
0.496 mol BF3 / 4 = 0.312 mol H2O / 3
0.124 mol BF3 = 0.104 mol H2O
Since BF3 has a higher number of moles, it is not the limiting reactant.
Thus, H2O is the limiting reactant.
To calculate the moles of HBF4 that can be produced, we need to use the mole ratio between H2O and HBF4 from the balanced equation (which is 3:3).
Each mole of H2O will produce one mole of HBF4.
Therefore, the moles of HBF4 that can be produced is equal to the moles of H2O, which is 0.312 mol.
To identify the limiting reactant and calculate the number of moles of HBF4 that can be produced, we need to compare the given amounts of reactants to their stoichiometric coefficients in the balanced equation.
The balanced equation for the reaction is:
4 BF3 + 3 H2O → H3BO3 + 3 HBF4
First, let's calculate the number of moles for each reactant:
Moles of BF3 = 0.496 mol
Moles of H2O = mass / molar mass = 5.63 g / molar mass of H2O
To determine the molar mass of H2O, we need to know the atomic masses of hydrogen (H) and oxygen (O). The atomic masses are approximately: H = 1 g/mol and O = 16 g/mol.
Molar mass of H2O = 2(1 g/mol) + 16 g/mol = 18 g/mol
Now we can calculate the number of moles of H2O:
Moles of H2O = 5.63 g / 18 g/mol
Next, we compare the moles of BF3 and H2O to their stoichiometric coefficients in the balanced equation to determine the limiting reactant.
From the balanced equation, we see that BF3 has a coefficient of 4, and H2O has a coefficient of 3. This means that 4 moles of BF3 react with 3 moles of H2O.
To find out which reactant is the limiting reactant, we compare their ratios. Divide the number of moles of each reactant by their respective stoichiometric coefficients:
Moles of BF3 / Stoichiometric coefficient of BF3 = 0.496 mol / 4 = 0.124 mol BF3
Moles of H2O / Stoichiometric coefficient of H2O = (5.63 g / 18 g/mol) / 3
Now we can compare the two results:
0.124 mol BF3 vs. (5.63 g / 18 g/mol) / 3 mol H2O
By comparing the two, we can see that the limiting reactant is the one that produces the smaller amount of the product (HBF4) based on the stoichiometry. Therefore, whichever reactant produces the smaller number of moles of HBF4 will be considered the limiting reactant.
To calculate the moles of HBF4 produced, we need to convert the moles of the limiting reactant (in this case, H2O) into moles of HBF4 using stoichiometry.
Using the balanced equation, we see that for every 3 moles of H2O, we produce 3 moles of HBF4.
Moles of HBF4 = Moles of H2O × (3 moles HBF4 / 3 moles H2O)
Finally, substitute the value of Moles of H2O calculated earlier to find the moles of HBF4 that can be produced.
Please note that this explanation assumes all reactions go to completion, and the reaction goes according to the stoichiometry.