Chemistry

Hydrogen peroxide(H2O2) slowly decomposes to form water and oxygen gas. Calculate the mass of Hydrogen peroxide needed to obtain 0.460L of oxygen gas at STP

  1. 👍 0
  2. 👎 1
  3. 👁 885
  1. 2H2O2 ==> 2H2O + O2
    mols O2 gas = 0.460L/22.4 = ?
    Using the coefficients in the balanced equation, convert mols O2 gas to mols H2O2.
    Now convert mols H2O2 to grams. g = mols x molar mass.

    1. 👍 0
    2. 👎 1

Respond to this Question

First Name

Your Response

Similar Questions

  1. Science

    Hydrogen peroxide, H2O2, is unstable under certain conditions and decomposes as follows: 2 H2O2 → 2 H2O + O2 ? g 34.00 g 15.98 g What mass of hydrogen peroxide, to the nearest hundredth of a gram, is decomposed in this reaction?

  2. chemistry

    When hydrogen peroxide (H2O2) is used in rocket fuels, it produces water, oxygen, and heat. 2H2O2(l)⟶2H2O(l)+O2(g)ΔH=−196kJ How many kilojoules are released when 2.65 moles of H2O2 reacts? How many kilojoules are released

  3. Science

    Hydrogen peroxide can be prepared in several ways. One method is the reaction between hydrogen and oxygen, another method is the reaction between water and oxygen. Calculate the ΔG°rxn of each reaction below? 1) H2(g) + O2(g)

  4. science

    drogen peroxide, H2O2, is unstable under certain conditions and decomposes as follows: 2 H2O2 → 2 H2O + O2 ? g 34.00 g 15.98 g What mass of hydrogen peroxide, to the nearest hundredth of a gram, is decomposed in this reaction?

  1. chemistry

    Liquid hydrogen peroxide, an oxidizing agent in many rocket fuel mixtures, releases oxygen gas on decomposition. 2 H2O2(l) 2 H2O(l) + O2(g) Hrxn = -196.1 kJ How much heat is released when 529 kg H2O2 decomposes? ( ......... ) KJ

  2. chemistry

    Hydrogen peroxide, H2O2, is used to disinfect contact lenses. What volume of O2, in mL, or O2(g) at 31 degree celsius, and 741mmHg can be liberated from 10.0mL of an aqueous solution containing 3.00% H2O2 by mass? The density of

  3. chemistry

    2mno4 - + 5h2o2 + 6h= 2mn 2+ + 5o2(gás) + 8h2o You must determine the percentage of hydrogen peroxide (H2O2) in a solution by permangan titration. In an acid solution, the permanganations will oxidize hydrogen peroxide to oxygen

  4. AP Chem

    A solution of hydrogen peroxide, H2O2, is titrated with a solution of potassium permanganate, KMnO4. It requires 51.7 mL of 0.145 M KMnO4 to titrate 20.0 g of the solution of hydrogen peroxide. What is the mass percentage of H2O2

  1. Chemistry

    The following reaction represents the decomposition of hydrogen peroxide 2H2O2 -> o2 (g) + 2H2O (l) How many molecules of water are produced from the decomposition of 3.4g of Hydrogen peroxide, H2O2? Please walk me through this

  2. CHE1

    Hydrogen peroxide decomposes to water and oxygen at constant pressure by the following reaction: 2H2O2(l) → 2H2O(l) + O2(g) ΔH = -196 kJ Calculate the value of q (kJ) in this exothermic reaction when 4.60 g of hydrogen peroxide

  3. Chemistry

    Hydrogen peroxide can be prepared by the reaction of barium peroxide with sulfuric acid according to BaO2+H2SO4 -> BaSO4 +H2O2 How many milliliters of 3.50 M H2SO4(aq) are needed to react completely with 12.1 g of BaO2(s)?

  4. Chemistry

    Redox titrations are used to determine the amounts of oxidizing and reducing agents in solution. For example, a solution of hydrogen peroxide, , can be titrated against a solution of potassium permanganate, . The following

You can view more similar questions or ask a new question.