If the process below is only 80% efficient, determine the mass of SiO2 required to produce 11 .00 g of P4.12Ca5(PO4)3F  +  43SiO2  + 90C  → 9P4  +  90CO  +  20(3CaO.2SiO2)  +  3SiFGroup of answer choices25.49 g135.4 g1.396g1.955g31.87 g

To solve this problem, we need to use the concept of stoichiometry, which is a section of chemistry that involves using relationships between reactants and/or products in a chemical reaction to determine desired quantitative data.

Here are the steps:

1. First, we need to find the molar mass of P4 and SiO2. The molar mass of P4 is approximately 123.895044 g/mol and the molar mass of SiO2 is approximately 60.0835 g/mol.

2. Next, we need to find the stoichiometric ratio between P4 and SiO2 from the balanced chemical equation. The ratio is 9:43.

3. Now, we can calculate the amount of SiO2 needed to produce 11.00 g of P4. We do this by setting up a proportion: (11.00 g P4 / 123.895044 g/mol P4) = x g SiO2 / (43 mol SiO2 * 60.0835 g/mol SiO2).

4. Solving for x gives us the theoretical yield of SiO2, which is the amount of SiO2 that would be needed if the reaction were 100% efficient.

5. However, the problem states that the process is only 80% efficient. So, we need to adjust our answer from step 4 to account for this. We do this by dividing the theoretical yield by 0.80.

6. The final answer is the mass of SiO2 required to produce 11.00 g of P4 with 80% efficiency.

Please note that the exact answer will depend on the specific values you use for the molar masses of P4 and SiO2, as well as the efficiency of the process.