how many milliliters of 4 M h2so4 are needed to react completely with 23.7g of Bao2
figure the moles of Ba(OH)2 (note formula) in 23.7grams
molesBa(OH)2= 23.7/formulamassBa(OH)2
I get about 0.14 moles
then consider the balanced equation:
Ba(OH)2 + H2SO4 >>> 2H2O + BaSO4
so you need the same amount of moles of sulfuric acid.
Molarityacid=molesacid/volumeinLiters
volumeacid=.14about/4=.045liters= about 45 ml
Your formula writing has to improve very quickly if you do not want to flunk. In chemsitry, there are great differences between capital letters and small letters.
To determine how many milliliters of 4 M H2SO4 are needed to react completely with 23.7g of BaO2, we will follow these steps:
Step 1: Calculate the molar mass of BaO2
BaO2:
Ba: 1 atom x atomic mass of Ba = 1 x 137.33 g/mol = 137.33 g/mol
O: 2 atoms x atomic mass of O = 2 x 16.00 g/mol = 32.00 g/mol
Molar mass of BaO2 = 137.33 g/mol + 32.00 g/mol = 169.33 g/mol
Step 2: Convert the mass of BaO2 to moles
Moles = mass / molar mass
Moles of BaO2 = 23.7 g / 169.33 g/mol = 0.140 mol
Step 3: Calculate the stoichiometric ratio between BaO2 and H2SO4
From the balanced chemical equation:
BaO2 + H2SO4 -> BaSO4 + H2O2
The stoichiometric ratio between BaO2 and H2SO4 is 1:1.
Step 4: Calculate the volume of H2SO4 using the molarity
Moles of H2SO4 = moles of BaO2 = 0.140 mol
Molarity of H2SO4 = 4 M
Volume = moles / molarity
Volume of H2SO4 = 0.140 mol / 4 M = 0.035 L
Step 5: Convert the volume to milliliters
1 L = 1000 mL
0.035 L x 1000 mL/L = 35 mL
Therefore, 35 milliliters of 4 M H2SO4 are needed to react completely with 23.7g of BaO2.
To determine the number of milliliters of 4 M H2SO4 required to react completely with 23.7g of BaO2, we need to follow these steps:
Step 1: Write a balanced chemical equation for the reaction.
The balanced equation for the reaction between BaO2 and H2SO4 is:
BaO2 + H2SO4 → BaSO4 + H2O
Step 2: Calculate the number of moles of BaO2.
Using the given mass of BaO2 (23.7g) and its molar mass, which can be found by summing the atomic masses of its elements from the periodic table, we can calculate the number of moles of BaO2.
Molar mass of BaO2: (1 × 137.33) + (2 × 16.00) = 169.33 g/mol
Number of moles of BaO2 = Mass / Molar mass = 23.7g / 169.33 g/mol
Step 3: Use stoichiometry to determine the moles of H2SO4 required.
By examining the balanced equation, we can see that the stoichiometric ratio between BaO2 and H2SO4 is 1:1. This means that 1 mole of BaO2 reacts with 1 mole of H2SO4. Therefore, the number of moles of H2SO4 required is equal to the number of moles of BaO2.
Step 4: Convert moles of H2SO4 to milliliters.
Since we know the molarity (4 M) of H2SO4, we can use its definition to convert moles to milliliters. Molarity is defined as moles of solute per liter of solution.
Molarity (M) = Moles of solute / Volume of solution (in liters)
To convert moles to milliliters, we can rearrange the equation:
Volume of solution (in liters) = Moles of solute / Molarity
Volume of solution (in milliliters) = (Moles of solute / Molarity) × 1000
Now, let's plug in the values and calculate the volume of 4 M H2SO4 required:
Volume of 4 M H2SO4 = (Number of moles of H2SO4 / Molarity of H2SO4) × 1000
Note: The Molarity of H2SO4 is given as 4 M.
By following these steps, we can determine the number of milliliters of 4 M H2SO4 required to react completely with 23.7g of BaO2.