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Solved: Hydrogen peroxide with a concentration of 3.0
Chapter 12, Problem 99P(choose chapter or problem)
Hydrogen peroxide with a concentration of 3.0 percent (3.0 g of \(\mathrm{H}_{2} \mathrm{O}_{2}\) in 100 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.
Questions & Answers
QUESTION:
Hydrogen peroxide with a concentration of 3.0 percent (3.0 g of \(\mathrm{H}_{2} \mathrm{O}_{2}\) in 100 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.
ANSWER:Step 1 of 4
We know the Ideal gas equation
Complete balanced equation for the reaction is