Hydrogen peroxide can be produced in the lab by reacting barium peroxide with hydrochloric acid. another product of the reaction is barium chloride.
1). what is the balanced chemical equation for the reaction?
2). what mass of hydrogen peroxide should result when 1.50g of barium peroxide is reacted with 25.0 mL of 0.50 M hydrochloric acid?
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To find the balanced chemical equation for the reaction, we need to first determine the chemical formulas of the reactants and products involved.
1) The reactants are barium peroxide (BaO2) and hydrochloric acid (HCl). The products are hydrogen peroxide (H2O2) and barium chloride (BaCl2).
Now, we can write the balanced chemical equation by making sure that the number of atoms of each element is the same on both sides of the equation:
BaO2 + 2 HCl → H2O2 + BaCl2
2) To find the mass of hydrogen peroxide produced when 1.50g of barium peroxide reacts with 25.0 mL of 0.50 M hydrochloric acid, we need to follow these steps:
Step 1: Calculate the number of moles of barium peroxide.
The molar mass of barium peroxide (BaO2) is:
Ba → 137.33 g/mol
O → 16.00 g/mol (there are two oxygen atoms)
Molar mass of BaO2 = 137.33 g/mol + 2(16.00 g/mol) = 169.33 g/mol
Number of moles of barium peroxide = mass / molar mass
Number of moles = 1.50 g / 169.33 g/mol
Step 2: Calculate the number of moles of hydrochloric acid.
The molarity (M) of hydrochloric acid is given as 0.50 M. Molarity is defined as moles of solute per liter of solution.
Number of moles of hydrochloric acid = molarity × volume (in liters)
Volume in liters = 25.0 mL × (1 L / 1000 mL) = 0.025 L
Number of moles of hydrochloric acid = 0.50 M × 0.025 L
Step 3: Determine the limiting reactant.
We compare the number of moles of barium peroxide with the number of moles of hydrochloric acid obtained in steps 1 and 2. The reactant that produces fewer moles of product is the limiting reactant.
Since the balanced equation shows that 1 mole of barium peroxide reacts with 2 moles of hydrochloric acid, we need to divide the number of moles of hydrochloric acid by 2 to determine its stoichiometrically equivalent amount.
Step 4: Calculate the moles of hydrogen peroxide produced.
Since the stoichiometry of the balanced equation shows that 1 mole of barium peroxide produces 1 mole of hydrogen peroxide, we can conclude that the number of moles of hydrogen peroxide produced is equal to the limiting reactant's stoichiometrically equivalent amount.
Step 5: Calculate the mass of hydrogen peroxide produced.
Finally, we can calculate the mass of hydrogen peroxide produced by multiplying the number of moles obtained in step 4 by the molar mass of hydrogen peroxide (34.02 g/mol).
I hope this explanation helps you find the balanced chemical equation and calculate the mass of hydrogen peroxide produced.