what mass of H 2 O is needed to completely react with 5.10g SiCl4
Well, let's crunch the numbers. To find out how much water is needed to completely react with 5.10g of SiCl4, we need to know the molar mass of SiCl4.
The molar mass of SiCl4 is approximately 169.9 g/mol.
To calculate the amount of water needed, we need to find out the molar ratio between SiCl4 and H2O in the reaction.
The balanced chemical equation for the reaction is: SiCl4 + 2H2O → Si(OH)4 + 4HCl
From the equation, we can see that 1 mole of SiCl4 reacts with 2 moles of H2O.
Now, let's calculate the amount of water needed:
5.10g SiCl4 * (1 mol / 169.9g SiCl4) * (2 mol H2O / 1 mol SiCl4) * (18.015g H2O / 1 mol H2O)
After crunching the numbers, you'll find that approximately **3.64g H2O** is needed to completely react with 5.10g SiCl4.
But hey, don't forget that too much water can make things pretty wet! So, make sure you're not drowning in H2O while carrying out your reaction. Safety first!
To find out the mass of H2O needed to completely react with 5.10g of SiCl4, we need to determine the stoichiometry of the reaction.
The balanced chemical equation for the reaction between SiCl4 and H2O is:
SiCl4 + 2H2O -> SiO2 + 4HCl
From the stoichiometry, we can see that 1 mole of SiCl4 reacts with 2 moles of H2O. Therefore, we need to convert the mass of SiCl4 to moles and then use the mole ratio to find the moles of H2O required. Finally, we can convert the moles of H2O to grams.
Step 1: Calculate the molar mass of SiCl4.
The molar mass of SiCl4 is:
Si: 28.0855 g/mol
Cl: 35.453 g/mol (4 Cl atoms)
Total molar mass of SiCl4 = 28.0855 g/mol + (4 * 35.453 g/mol) = 169.898 g/mol
Step 2: Convert the mass of SiCl4 to moles.
Moles of SiCl4 = Mass of SiCl4 / Molar mass of SiCl4
Moles of SiCl4 = 5.10g / 169.898 g/mol
Step 3: Use the mole ratio to calculate the moles of H2O.
From the balanced equation, we know that 1 mole of SiCl4 reacts with 2 moles of H2O.
Moles of H2O = Moles of SiCl4 * (2 moles H2O / 1 mole SiCl4)
Step 4: Convert the moles of H2O to grams.
Mass of H2O = Moles of H2O * Molar mass of H2O
Note: The molar mass of H2O is 18.015 g/mol.
By following these steps and performing the necessary calculations, you will be able to find the mass of H2O needed to completely react with 5.10g of SiCl4.
To determine the mass of water (H2O) needed to completely react with 5.10g of SiCl4, we first need to remember the balanced chemical equation for the reaction between SiCl4 and water:
SiCl4 + 2H2O -> SiO2 + 4HCl
From the balanced equation, we can see that 1 mole of SiCl4 reacts with 2 moles of H2O. To calculate the moles of SiCl4, we can use its molar mass, which is 169.9 g/mol.
Moles of SiCl4 = mass of SiCl4 / molar mass = 5.10g / 169.9 g/mol ≈ 0.03 mol
Since the mole ratio between SiCl4 and H2O is 1:2, the moles of H2O needed will be:
Moles of H2O = 2 × moles of SiCl4 = 2 × 0.03 mol = 0.06 mol
Finally, we can convert the moles of H2O to grams using its molar mass, which is 18.015 g/mol:
Mass of H2O = moles of H2O × molar mass = 0.06 mol × 18.015 g/mol ≈ 1.08g
Therefore, approximately 1.08 grams of H2O are needed to completely react with 5.10 grams of SiCl4.
SiCl4 + 2 H2O → SiO2 + 4 HCl
The ratio r of mass of H2O to SiCl4 is therefore
r = 2*(molar mass of water)/(molar mass of SiCl4)