CaSiO3(s) +6 HF (g)-> CaF2(aq) + SiF4 (g) + 3 H2O(l)
If a 65.6 g sample of CaSiO3 is reacted in an inert 83 L container at 25.5°C with HF at 1.00 atm pressure find the following.
a. the mass of water, and CaF2 produced in the reaction and the mass of HF that remains.
b. The partial pressure of SiF4 in the container after the temperature has returned to 25.5°C.
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To find the mass of water, CaF2, and HF produced in the reaction, we need to use stoichiometry. Stoichiometry is the calculation of reactants and products in chemical reactions.
Here are the steps to solve part (a) of the question:
1. Write a balanced chemical equation:
The balanced equation for the reaction is:
CaSiO3(s) + 6 HF(g) -> CaF2(aq) + SiF4(g) + 3 H2O(l)
2. Calculate the number of moles of CaSiO3:
Given the mass of CaSiO3 is 65.6 g, we can calculate the number of moles using its molar mass. The molar mass of CaSiO3 can be found by adding up the atomic masses of its constituent elements (Ca: 40.08 g/mol, Si: 28.08 g/mol, O: 16.00 g/mol). Therefore, the molar mass of CaSiO3 is 40.08 + 28.08 + (16.00 * 3) = 128.24 g/mol.
Moles of CaSiO3 = mass / molar mass
Moles of CaSiO3 = 65.6 g / 128.24 g/mol
3. Determine the limiting reactant:
To find the limiting reactant, we compare the moles of CaSiO3 with the stoichiometric ratio in the balanced equation. From the equation, we can see that the molar ratio between CaSiO3 and HF is 1:6.
Moles of HF = Moles of CaSiO3 * (6 moles of HF / 1 mole of CaSiO3)
4. Calculate the moles of all products:
Using the stoichiometric ratio, we can determine the moles of CaF2, SiF4, and H2O produced in the reaction.
Moles of CaF2 = Moles of CaSiO3 * (1 mole of CaF2 / 1 mole of CaSiO3)
Moles of SiF4 = Moles of CaSiO3 * (1 mole of SiF4 / 1 mole of CaSiO3)
Moles of H2O = Moles of CaSiO3 * (3 moles of H2O / 1 mole of CaSiO3)
5. Convert moles to mass:
Now, we can calculate the mass of water, CaF2, and HF produced using the molar masses of each compound.
Mass of water = Moles of H2O * molar mass of H2O
Mass of CaF2 = Moles of CaF2 * molar mass of CaF2
Mass of HF remaining = Moles of HF * molar mass of HF
To solve part (b), we need to use the ideal gas law to calculate the partial pressure of SiF4.
1. Convert the volume of the container to liters at the given temperature:
83 L remains the same since it is already given in liters.
2. Calculate the number of moles of SiF4:
Using the ideal gas law equation:
PV = nRT
Where:
P = pressure (atm)
V = volume (L)
n = number of moles
R = gas constant (0.0821 L.atm/mol.K)
T = temperature (K)
Since we have the pressure, volume, and temperature, we can rearrange the equation to calculate the number of moles:
n = PV / RT
3. Calculate the partial pressure of SiF4:
To find the partial pressure, we need to consider the moles of SiF4 in the total moles of all gases present:
Partial pressure of SiF4 = (moles of SiF4 / total moles of gas) * total pressure
Now, you can follow these steps to solve both parts (a) and (b) of the question.