Question

If 3.0 moles of HF react with 4.5 moles of SiO2, how many moles of SiF4 can be formed? Describe the steps.

SiO2(s) + HF(g) → SiF4(g) + H2O(l)

Answer 1

To determine how many moles of SiF4 can be formed when 3.0 moles of HF react with 4.5 moles of SiO2, first determine the limiting reactant (SiO2). Then, use the stoichiometric ratio from the balanced equation to determine the moles of SiF4 that can be formed. The number of moles of SiF4 formed would be the same as the number of moles of the limiting reactant, which is 4.5 moles of SiO2.

Step-by-step explanation:

We first need to determine the limiting reactant to determine how many moles of SiF4 can be formed when 3.0 moles of HF react with 4.5 moles of SiO2. The limiting reactant is the reactant that is completely consumed in a chemical reaction, thereby determining the maximum amount of product that can be formed. To find the limiting reactant, we compare the moles of HF and SiO2 using the stoichiometric ratio from the balanced chemical equation: 1 mole of SiO2 reacts with 4 moles of HF to produce 1 mole of SiF4.

Now that we know SiO2 is the limiting reactant, we can use the stoichiometric ratio to determine the moles of SiF4 that can be formed. From the balanced chemical equation, we know that 1 mole of SiO2 reacts with 1 mole of SiF4. Therefore, the number of moles of SiF4 formed would be the same as the number of moles of the limiting reactant, which is 4.5 moles of SiO2.