Oxygen is often produced in laboratories with a certain mass fraction of hydrogen peroxide solution

1) According to the law of conservation of mass, the total mass before the reaction is equal to the total mass after the reaction. Before the reaction, the residual mass plus the mass of oxygen released after the reaction should also be equal to grams, so the oxygen mass is grams.

2) Calculated according to the chemical equation. Let the mass of hydrogen peroxide be x2h2o2=mno2=2h2o+o2

x solution gives x = grams.

then the mass fraction of hydrogen peroxide is.

Solution: grams of hydrogen peroxide solution, 1 gram of mnO2 is added, the mixture weighs grams, and the mass of the residue is weighed in grams after complete reaction. Reduce grams. Let the mass of the released oxygen be x grams and the mass of hydrogen peroxide reacted to be y grams.

2H2O2 = Mno2 = 2H2O + O2 Mass Reduction.

68 36 32 32 grams.

y x grams.

Then: x = 32 = grams.

y = 68 = grams.

The mass fraction of hydrogen peroxide solution was: =8%.

A: ...Respectfully, thank you!

1) Oxygen Quality: Mass is conserved.

2) Hydrogen peroxide mass of the reaction: negative monovalent generates 0-valent redox reaction.

The mass fraction of the hydrogen peroxide solution (

1 Conservation of mass Oxygen mass.

2 Write the equation for the chemical reaction Calculate the amount of hydrogen peroxide consumed based on the mass of oxygen and divide it by the mass of the hydrogen peroxide solution = answer.

Hydrogen peroxide for oxygen production in the laboratory - junior high school chemistry experiment.

Oxygen mass: 2+

2h2o2 ===2h2o + o2

68 32x =

Mass fraction of solute in hydrogen peroxide solution:

Mass of oxygen generated: 2g+

2h2o2 =mno2=2h2o + o268 32

x68/x=32/

x = mass fraction of solute in hydrogen peroxide solution:

Because the title says that "when producing oxygen, only a certain quality of the above-mentioned hydrogen peroxide is taken, and then the same mass of water is added for mixing", so it should be multiplied by 50.

Laboratory with 5% hydrogen peroxide solution and manganese dioxide.

To produce oxygen, if you want to produce 16g of oxygen dust to sell, you need 5% hydrogen peroxide solution to tease the mass of the sedan car.

2h2o2=mno2=2h2o+o2

x*5% 16g

68/32=x*5%/16g

x=680g

To make 20g of oxygen with hydrogen oxide solution, how many grams of 15% H2O2 solution are needed (calculation process)!

Let the mass of the hydrogen peroxide solution be x.

2h2o2=mno2=2h2o+o2↑

15%x68/15%x=32/

x = A: Hydrogen peroxide solution is required.

1) The filter residue is still grams. Manganese dioxide has no reaction and is only catalytic.

2）2h2o2=2h2o+o2

x grams) solute mass in grams.

The mass of the catalyst does not change before and after the chemical reaction.

m Filter residue The mass of hydrogen peroxide to be generated is x

2h2o2＝mno2＝2h2o＋o2xx＝

h2o2％＝

Answer: The mass fraction of the solute in the original hydrogen peroxide solution is.

Add a suitable amount of water to 10 g of hydrogen peroxide solution with a high mass of 30% to prepare 60g of 5% hydrogen peroxide.

x*30%=60g*5%

x=10g

Add an appropriate amount of water to (10)g of hydrogen peroxide solution with a mass fraction of 30% to prepare 60g of 5% hydrogen peroxide.

Let the mass of 30% hydrogen peroxide solution be x.

30%x=60*5%

x=10g

Set the mass x of hydrogen peroxide required

2h2o2mno.2h2o+o2↑

68 32x＝

Solution: x= so theoretically the mass of the hydrogen peroxide solution is required:

A: Theoretically, the mass of this hydrogen peroxide solution is 68g