Type The Correct Answer In The Box.Given:${ SiO_2 + 4 HF \rightarrow SiF_4 + 2 H_2O }$In This Chemical Reaction, How Many Grams Of HF Are Needed For 182 Grams Of ${ SiO_2 }$ To React Completely? Express Your Answer To Three

Understanding the Chemical Reaction

The given chemical reaction is:

${ SiO_2 + 4 HF \rightarrow SiF_4 + 2 H_2O }$

This reaction involves the reaction of silicon dioxide (SiO2) with hydrofluoric acid (HF) to produce silicon tetrafluoride (SiF4) and water (H2O).

Balancing the Chemical Equation

To determine the amount of HF needed for 182 grams of SiO2 to react completely, we first need to balance the chemical equation. The balanced equation is:

${ SiO_2 + 4 HF \rightarrow SiF_4 + 2 H_2O }$

Calculating the Molar Mass of SiO2 and HF

To solve this problem, we need to calculate the molar mass of SiO2 and HF.

• The molar mass of SiO2 is:
  • Silicon (Si): 28.09 g/mol
  • Oxygen (O): 16.00 g/mol
  • Total molar mass of SiO2: 28.09 g/mol + 2(16.00 g/mol) = 60.09 g/mol
• The molar mass of HF is:
  • Hydrogen (H): 1.01 g/mol
  • Fluorine (F): 19.00 g/mol
  • Total molar mass of HF: 1.01 g/mol + 19.00 g/mol = 20.01 g/mol

Determining the Number of Moles of SiO2

To determine the number of moles of SiO2, we can use the formula:

${ \text{Number of moles} = \frac{\text{Mass of SiO2}}{\text{Molar mass of SiO2}} }$

Plugging in the values, we get:

${ \text{Number of moles of SiO2} = \frac{182 \text{ g}}{60.09 \text{ g/mol}} = 3.03 \text{ mol} }$

Determining the Number of Moles of HF Required

According to the balanced chemical equation, 4 moles of HF are required to react with 1 mole of SiO2. Therefore, the number of moles of HF required is:

${ \text{Number of moles of HF} = 4 \times \text{Number of moles of SiO2} }$

Plugging in the value, we get:

${ \text{Number of moles of HF} = 4 \times 3.03 \text{ mol} = 12.12 \text{ mol} }$

Calculating the Mass of HF Required

To calculate the mass of HF required, we can use the formula:

${ \text{Mass of HF} = \text{Number of moles of HF} \times \text{Molar mass of HF} }$

Plugging in the values, we get:

${ \text{Mass of HF} = 12.12 \text{ mol} \times 20.01 \text{ g/mol} = 242.5 \text{ g} }$

Therefore, 242.5 grams of HF are needed for 182 grams of SiO2 to react completely.

Conclusion

Q: What is the difference between a balanced chemical equation and an unbalanced chemical equation?

A: A balanced chemical equation is an equation in which the number of atoms of each element is the same on both the reactant and product sides. An unbalanced chemical equation is an equation in which the number of atoms of each element is not the same on both the reactant and product sides.

Q: How do I balance a chemical equation?

A: To balance a chemical equation, you need to add coefficients (numbers in front of the formulas of reactants or products) to make the number of atoms of each element the same on both sides of the equation. You can start by balancing the elements that appear only once on each side of the equation, and then work your way through the rest of the elements.

Q: What is stoichiometry?

A: Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in chemical reactions. It involves calculating the amounts of reactants and products required for a given reaction.

Q: How do I calculate the number of moles of a substance?

A: To calculate the number of moles of a substance, you need to divide the mass of the substance by its molar mass. The molar mass is the mass of one mole of the substance.

Q: What is the difference between a mole and a gram?

A: A mole is a unit of measurement that represents 6.022 x 10^23 particles (atoms or molecules). A gram is a unit of mass that represents 1/1000 of a kilogram.

Q: How do I calculate the mass of a substance required for a given reaction?

A: To calculate the mass of a substance required for a given reaction, you need to multiply the number of moles of the substance by its molar mass.

Q: What is the significance of balancing chemical equations?

A: Balancing chemical equations is important because it allows us to predict the amounts of reactants and products required for a given reaction. It also helps us to understand the relationships between reactants and products in a chemical reaction.

Q: Can you give an example of how to balance a chemical equation?

A: Yes, here is an example of how to balance a chemical equation:

${ 2H_2 + O_2 \rightarrow 2H_2O }$

To balance this equation, we need to add coefficients to make the number of atoms of each element the same on both sides of the equation. The balanced equation is:

${ 2H_2 + O_2 \rightarrow 2H_2O }$

Q: Can you give an example of how to use stoichiometry to calculate the mass of a substance required for a given reaction?

A: Yes, here is an example of how to use stoichiometry to calculate the mass of a substance required for a given reaction:

Suppose we want to calculate the mass of hydrogen gas (H2) required to react with 10 grams of oxygen gas (O2) in the following reaction:

${ 2H_2 + O_2 \rightarrow 2H_2O }$

First, we need to calculate the number of moles of oxygen gas:

${ \text{Number of moles of O}_2 = \frac{\text{Mass of O}_2}{\text{Molar mass of O}_2} }$

${ \text{Number of moles of O}_2 = \frac{10 \text{ g}}{32 \text{ g/mol}} = 0.3125 \text{ mol} }$

Next, we need to calculate the number of moles of hydrogen gas required to react with 0.3125 moles of oxygen gas:

${ \text{Number of moles of H}_2 = 2 \times \text{Number of moles of O}_2 }$

${ \text{Number of moles of H}_2 = 2 \times 0.3125 \text{ mol} = 0.625 \text{ mol} }$

Finally, we can calculate the mass of hydrogen gas required:

${ \text{Mass of H}_2 = \text{Number of moles of H}_2 \times \text{Molar mass of H}_2 }$

${ \text{Mass of H}_2 = 0.625 \text{ mol} \times 2 \text{ g/mol} = 1.25 \text{ g} }$

Therefore, 1.25 grams of hydrogen gas are required to react with 10 grams of oxygen gas.