Question

Hydrogen peroxide decomposes to water and oxygen gas. Write out the equation, describing what is oxidized...

Hydrogen peroxide decomposes to water and oxygen gas. Write out the equation, describing what is oxidized and what is reduced, and what material is the oxidizing agent and what material is the reducing agent.

Homework Answers

Answer #1

When Hydrogen Peroxide is decomposed it gives water and Oxygen gas

in the presence of light.

This is an example of disproportionation reaction where oxygen is reduced and oxidized.

In oxygen has the oxidation state

Now at product side , in H2O, the oxidation state Of Oxygen is

and in O2 , the oxidation state of oxygen is

In one case, state of oxygen from -1 to -2 that means it is reduced and in other case the oxidation state from -1 to 0 that means oxidized.

Here oxygen is oxidized and also reduced.

Here H2O2 is the oxidizing agent and the oxygen(O2) is the reducing agent.

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Hydrogen peroxide decomposes to yield water and oxygen. The decomposition is first order with a rate...
Hydrogen peroxide decomposes to yield water and oxygen. The decomposition is first order with a rate constant at 46°C of 1.6 × 10-4 s-1. Calculate the partial pressure of the oxygen produced from 1.25 L of a 0.750 M H2O2 solution at 46°C over a period of 24.0 hours if the gas is collected in a 13.0 L container. Please show all work! Thanks in advance!
Water decomposes to produce hydrogen gas and oxygen gas. How many grams of water would be...
Water decomposes to produce hydrogen gas and oxygen gas. How many grams of water would be required to produce 10.0 moles of hydrogen gas?
Write the two half-reactions involved in the disproportionation of hydrogen peroxide to water and diatomic oxygen....
Write the two half-reactions involved in the disproportionation of hydrogen peroxide to water and diatomic oxygen. Balance the equation . Calcuate Eo for the overall reaction.
What mass of which reagent is left unreacted?Hydrogen peroxide is used as a cleaning agent in...
What mass of which reagent is left unreacted?Hydrogen peroxide is used as a cleaning agent in the treatment of cuts and abrasions for several reasons. It is an oxidizing agent that can directly kill many microorganisms; it decomposes upon contact with blood, releasing elemental oxygen gas (which inhibits the growth of anaerobic microorganisms); and it foams upon contact with blood, which provides a cleansing action. In the laboratory, small quantities of hydrogen peroxide can be prepared by the action of...
Write out the balanced equation (including phases) for the decomposition of hydrogen peroxide
Write out the balanced equation (including phases) for the decomposition of hydrogen peroxide
Write the (a) balanced equation for the formation of liquid water from hydrogen and oxygen gas,...
Write the (a) balanced equation for the formation of liquid water from hydrogen and oxygen gas, and use it to explain the following terms: (b) chemical reaction, (c) reactant, (d) product.
Hydrogen peroxide is unstable and decomposes readily: 2H2O2(aq) → 2H2O(l) + O2(g) This reaction is accelerated...
Hydrogen peroxide is unstable and decomposes readily: 2H2O2(aq) → 2H2O(l) + O2(g) This reaction is accelerated by light, heat, or a catalyst. The concentrations of aqueous hydrogen peroxide solutions are normally expressed as percent by mass. In the decomposition of hydrogen peroxide, how many liters of oxygen gas can be produced at STP from 12.9 g of a 7.50% hydrogen peroxide solution?
If hydrogen peroxide H2O2 decomposes according to the equation: 2H2O2 → 2H2O + O2                      ∆H =...
If hydrogen peroxide H2O2 decomposes according to the equation: 2H2O2 → 2H2O + O2                      ∆H = −196 kJ Calculate the heat evolved on decomposition of 5g of H2O2.
What are the molecular equation, total ionic equation, and net ionic equation for the reactions of:...
What are the molecular equation, total ionic equation, and net ionic equation for the reactions of: a.) tin and silver nitrate b.) tin and zinc nitrate For the following reactions... what is the substance oxidized and reduced? What are the oxidizing agent and reducing agent? a.) Mg + CuSO4 ---> b.) Zn + HCl -->
Indicate the elements oxidized/reduced, as well as their oxidation states before and after the reaction. Determine...
Indicate the elements oxidized/reduced, as well as their oxidation states before and after the reaction. Determine which species is the oxidizing agent and which is the reducing agent.   2 AgNO3(aq) + Cu(s) ……> Cu(NO3)2(aq) + 2 Ag(s) A. Cu 0 à 2+; oxidized, Cu oxidizing agent; Ag + à 1-, reduced, AgNO3 reducing agent B. Cu 0 à 2+; oxidized, Cu oxidizing agent; Ag + à 0, reduced, AgNO3 reducing agent C. Cu 0 à 2+; oxidized, Cu reducing agent;...