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Chapter 5: Problem 97

A common demonstration in chemistry courses involves adding a tiny speck of manganese(IV) oxide to a concentrated hydrogen peroxide \(\left(\mathrm{H}_{2} \mathrm{O}_{2}\right)\) solution. Hydrogen peroxide decomposes quite spectacularly under these conditions to produce oxygen gas and steam (water vapor). Manganese(IV) oxide is a catalyst for the decomposition of hydrogen peroxide and is not consumed in the reaction. Write the balanced equation for the decomposition reaction of hydrogen peroxide.

Short Answer

Expert verified
The balanced equation for the decomposition reaction of hydrogen peroxide, catalyzed by manganese(IV) oxide, is: \( 2 \mathrm{H}_{2} \mathrm{O}_{2} \rightarrow \mathrm{O}_{2} + 2 \mathrm{H}_{2} \mathrm{O} \)

Step by step solution

01

Write the unbalanced equation

To begin, let's write down the unbalanced equation for the reaction, with reactants on the left and products on the right: H₂O₂ → O₂ + H₂O This equation represents the decomposition of hydrogen peroxide into oxygen gas and water.
02

Checking for catalyst

Since manganese(IV) oxide is a catalyst, it does not take part in the reaction, and thus it will not be included in the balanced chemical equation.
03

Balancing the equation

Now, let's balance the chemical equation. We'll start by counting the atoms of each element on the reactant and product sides: Reactants: 2 H atoms 2 O atoms Products: 2 H atoms 2 + 1 = 3 O atoms The hydrogen atoms are already balanced, but there is one extra oxygen atom in the products. To balance the equation, we can add coefficients before the chemical species to equalize the number of atoms for each element: 2 H₂O₂ → O₂ + 2 H₂O Now, we have: Reactants: 4 H atoms 4 O atoms Products: 4 H atoms 2 + 2 = 4 O atoms The equation is now balanced.
04

Write the balanced equation

The balanced equation for the decomposition reaction of hydrogen peroxide is: 2 H₂O₂ → O₂ + 2 H₂O

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Most popular questions from this chapter

Cumene is a compound containing only carbon and hydrogen that is used in the production of acetone and phenol in the chemical industry. Combustion of \(47.6 \mathrm{mg}\) cumene produces some \(\mathrm{CO}_{2}\) and \(42.8 \mathrm{mg}\) water. The molar mass of cumene is between 115 and \(125 \mathrm{g} / \mathrm{mol} .\) Determine the empirical and molecular formulas.

In 1987 the first substance to act as a superconductor at a temperature above that of liquid nitrogen \((77 \mathrm{K})\) was discovered. The approximate formula of this substance is \(\mathrm{YBa}_{2} \mathrm{Cu}_{3} \mathrm{O}_{7}\) Calculate the percent composition by mass of this material.

Arrange the following substances in order of increasing mass percent of carbon. a. caffeine, \(\mathrm{C}_{8} \mathrm{H}_{10} \mathrm{N}_{4} \mathrm{O}_{2}\) b. sucrose, \(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\) c. ethanol, \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\)

Give the balanced equation for each of the following. a. The combustion of ethanol \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right)\) forms carbon dioxide and water vapor. A combustion reaction refers to a reaction of a substance with oxygen gas. b. Aqueous solutions of lead(II) nitrate and sodium phosphate are mixed, resulting in the precipitate formation of lead(II) phosphate with aqueous sodium nitrate as the other product. c. Solid zinc reacts with aqueous HCl to form aqueous zinc chloride and hydrogen gas. d. Aqueous strontium hydroxide reacts with aqueous hydrobromic acid to produce water and aqueous strontium bromide.

There are two binary compounds of mercury and oxygen. Heating either of them results in the decomposition of the compound, with oxygen gas escaping into the atmosphere while leaving a residue of pure mercury. Heating 0.6498 g of one of the compounds leaves a residue of 0.6018 g. Heating 0.4172 g of the other compound results in a mass loss of 0.016 g. Determine the empirical formula of each compound.
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