CHEMISTRY | MOLE CONCEPT | Question 07


a) What mass of hydrogen peroxide should result when 1.45g of barium peroxide is treated with 25.5mL of hydrochloric acid solution containing 0.0277g of HCL per mL?
b) How much of the excess reactant is left?

BaO2(S)+ 2HCL(aq) → H2O(2aq) + BaCL(2aq)


  • DATA GIVEN:


    Mass of BaO2 = 1.45g
    Volume BaO2 = 25.5 mole
    Mass of HCl 0.0277g/dm3
    Asked:
    a) To find the mass of H2O2
    b) To find the mass of excess remain
    Equation for the reaction
    BaO2(s) + 2HCl(aq) → H2O2(aq) + BaCl2(aq)


  • To find mass of HCl
    From: ConC = mass /Volume
    = ConC × volume
    = 0.0277g/mole × 25.5 mole
    = 0.70635g
    To convert 0.70635g into mole
    Mole = mass /Molar mass of HCl
    = 0.70635g /36.5g/mole
    = 0.01935 mole for HCl
    Mole ratio for HCl is 0.00967

    To find the mole for BaO2
    = Mass /Molar mass
    = 1.45g /137g/mole
    = 0.0085
    Mole ratio = mole reacted /Mole coefficient
    = 0.0085 mole /1 mole
    = 0.0085

    The limiting is HCl with 0.01935 mole the excess is BaO2
  • a) To find the mass of H2O2


    a) To find mass of H2O2 mole equivalent between HCl and H2O2
    2 moles of HCl Ξ 1 mole H2O2
    0.01935 mole HCl Ξ ??

    = 0.01935 mole × 1 mole/2 mole
    = 0.009675 mole for H2O2
    Mass = mole × molar mass of H2O2
    = 0.009675 mole × 34g/mole
    = 0.32895g
    0.32895g of hydrogen peroxide (H2O2) was produced
  • b) To find the mass of excess remain


    b) Mass of excess of BaO2 mole equivalent between BaO2 and HCl
    1 mole of BaO2 Ξ 2 moles HCl
    ?? Ξ 0.01058 HCl

    = 1 × 0.01058 /2
    = 0.00529 mole of BaO2

    To convert 0.00529 into mass,
    Mass = 0.00529 × 169
    = 0.89401g BaO2
    Mass remain = 1.45g – 0.894g
    = 0.556g
    The mass remain of BaO2 was 0.556g

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