0
The balanced equation for the decomposition of hydrogen peroxide?
Wiki User
∙ 16y ago
One molecule of Oxygen Gas (O2) combines with two molecules of Hydrogen Gas (2H2) to form two molecules of water 2H2O.
O2+2H2=> 2H2O
There are the same numbers of H's and O's either side of the = meaning the equation is balanced, in respect of the fact that Oxygen and Hydrogen Gas have diatomic molecules (2 atoms stick together)
Wiki User
∙ 11y ago
Wiki User
∙ 14y ago2H2 + O2 = 2H2O
I know an = should not be used in chemical equations but I have no arrows.
Wiki User
∙ 14y agocatalase(aq)+ O2(g)+2H2O(l) forms 2H2O2(aq)
Wiki User
∙ 10y ago2H2O2 --> 2H2O + O2
This process is really slow naturally, unless you add a catalyst like potassium iodide or manganese oxide. Then it's pretty spectacular. And messy.
Wiki User
∙ 12y ago2h2o → 2h2 + o2
Wiki User
∙ 16y agoH2O2 --> H2 + O2
Wiki User
∙ 13y ago2H2O + O2 <-> 2H2O2 + Energy
Wiki User
∙ 11y agoThe equation is 2 H2O2 -> O2 + 2 H2O.
Add your answer:
Earn +20 pts
What is the balanced equation for H2O2 when it reacts to form gas and H2O?
I think what you are thinking of is the decomposition of Hydrogen peroxide, which has the equation: 2H2O2 --> O2 + 2H2O which when balanced then equals 8. 2(H2O2) --> 2H2O +O2 |4*2|=8 -->|3*2|=6 +2= 8 That is the entire equation completed and balanced. Hope it helped!
Which enzyme is responsible to the breakdown of hydrogen peroxide?
Manganese oxide is a catalyst which speeds up the decomposition of hydrogen peroxide.
Decomposition of hydrogen peroxide endothermic or exothermic?
It is obscenely exothermic This means that Hydrogen Peroxide is releasing heat to the surrounding environment, thus increasing the temperature.
What is an equation for a rusty nail in hydrogen peroxide?
2H2O2-->2H2O+O2 Hydrogen peroxide-->water + oxygen
What two products result from the breakdown of hydrogen peroxide?
H2O2 -> H2O + O2 (Without balancing)
What is the balanced equation for hydrogen peroxide and sodium hydroxide?
There isn't one because there is no reaction beyond the catalysis of the decomposition of the peroxide.
What is the balanced equation of the decomposition of H202?
2 H2O2 → 2 H2O + O2 Check out Wikipedia's entry on Hydrogen Peroxide
Liver plus hydrogen peroxide equals what and what?
When Hydrogen Peroxide (2H2O2) is combined with a small piece of liver, the hydrogen peroxide decomposes. This is because the small piece of liver acts as a catalyst, or the cause, of the decomposition of the Hydrogen Peroxide.The balanced equation is thus:2H2O2 (Hydrogen Peroxide) ---------> 2H2O + O2
What are the products of the decomposition reaction of hydrogen peroxide?
The products of the decomposition of hydrogen peroxide are water and oxygen, as shown in the following equation: 2 H2O2 → 2 H2O + O2
Chemical equation for the decomposition of hydrogen peroxide?
2 H2O2 ---> 2 H2O + O2 + energy, it's exothermic
What is the balanced equation for H2O2 when it reacts to form gas and H2O?
I think what you are thinking of is the decomposition of Hydrogen peroxide, which has the equation: 2H2O2 --> O2 + 2H2O which when balanced then equals 8. 2(H2O2) --> 2H2O +O2 |4*2|=8 -->|3*2|=6 +2= 8 That is the entire equation completed and balanced. Hope it helped!
What is the catalyst for the decomposition of hydrogen peroxide?
manganese sulfide
Which enzyme is responsible to the breakdown of hydrogen peroxide?
Manganese oxide is a catalyst which speeds up the decomposition of hydrogen peroxide.
Why a pinch of manganese dioxide causes hydrogen peroxide to explode?
Manganese dioxide is a catalyst for the decomposition of hydrogen peroxide.
What is the chemical equation on h2o2---h2o?
The decomposition of hydrogen peroxide produces water and oxygen. 2H2O2(l) -->2H2O(l) + O2(g)
What is negative catalyst in the decomposition of hydrogen peroxide?
phosphoric acid
How do you balance H2O2 - H2O?
The equation as given can not be balanced, because it is incomplete: When hydrogen peroxide decomposes to produce water, it also produces oxygen. A proper, balanced equation for the reaction is 2 H2O2 -> 2 H2O + O2.
