Hydrogen peroxide with a concentration of 3.0 percent (3.0 g of H2 O2 in 100 mL of solution) is

step 1 So we have a 3 % hydrogen peroxide. It goes under decomposition to produce oxygen. And we want t

Hydrogen peroxide with a concentration of 3.0 percent (3.0 g...

Hydrogen peroxide with a concentration of 3.0 percent (3.0 g of $\mathrm{H}_{2} \mathrm{O}_{2}$ in $100 \mathrm{mL}$ of solution) is sold in drugstores for use as an antiseptic. For a 10.0 -mL. 3.0 percent $\mathrm{H}_{2} \mathrm{O}_{2}$ solution, calculate (a) the oxygen gas produced (in liters) at STP when the compound undergoes complete decomposition and (b) the ratio of the volume of $\mathrm{O}_{2}$ collected to the initial volume of the $\mathrm{H}_{2} \mathrm{O}_{2}$ solution.

Hydrogen peroxide with a concentration of 3.0 percent (3.0 g of $\mathrm{H}_{2} \mathrm{O}_{2}$ in $100 \mathrm{mL}$ of solution) is sold in drugstores for use as an antiseptic. For a 10.0 -mL.
3.0 percent $\mathrm{H}_{2} \mathrm{O}_{2}$ solution, calculate (a) the oxygen gas produced (in liters) at STP when the compound undergoes complete decomposition and (b) the ratio of the volume of $\mathrm{O}_{2}$ collected to the initial volume of the $\mathrm{H}_{2} \mathrm{O}_{2}$ solution.

Key Concepts

Standard Temperature and Pressure (STP) and Molar Volume

At STP, one mole of any ideal gas occupies a known volume (typically 22.4 liters). This concept is used to convert the number of moles of a gas produced in a reaction into the volume it would occupy under standard conditions.

Stoichiometry

Stoichiometry involves using the balanced chemical equation to relate the quantities of reactants to products. It enables the calculation of the number of moles or grams of substances involved in the reaction, which is essential for determining the output of products from a given quantity of reactants.

Percent Concentration

This concept refers to the amount of solute present in a given volume or mass of solution, expressed as a percentage. It is important for converting between the mass of the solute and the volume of the solution, providing the basis for further stoichiometric calculations.

Chemical Decomposition Reaction

This is a type of reaction where a single compound breaks down into two or more products. In stoichiometric problems, understanding the balanced equation of a decomposition reaction is crucial to determine the relationships between the quantities of reactants and products.