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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.

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a. $\mathrm{V}=\mathrm{nRT} / \mathrm{P}=\left[\left(4.4 \mathrm{E}-3 \mathrm{mol} \mathrm{O}_{2}\right)(0.0821 \mathrm{L} \mathrm{atm} / \mathrm{mol} \mathrm{K})(273 \mathrm{K})\right] / 1.0 \mathrm{atm}=0.099 \mathrm{L}$b. 9.9

Chemistry 102

Chapter 12

Physical Properties of Solutions

Solutions

University of Maryland - University College

University of Kentucky

University of Toronto

Lectures

03:58

In chemistry, a solution is a homogeneous mixture composed of two or more substances. The term "solution" is also used to refer to the resultant mixture. The solution is usually a fluid. The particles of a solute are dispersed or dissolved in the solvent. The resulting solution is also called the solvent. The solvent is the continuous phase.

05:06

In physics and thermodynamics, the natural tendency of a system to change its state is its tendency to increase the entropy of the system. It is a measure of the disorder in a system.

02:37

Hydrogen peroxide solution…

03:34

Dilute aqueous hydrogen pe…

05:04

Hydrogen peroxide is unsta…

03:29

So we have a 3% hydrogen peroxide. It goes under the composition to produce oxygen, and we want to compute the volume off this oxygen produced. So the first step is to write down the equation. So the decomposition off hydrogen peroxide. Okay, you might be inclined to ride something like this. Hydrogen plus o two. But that's know what actually happens to hydrogen peroxide. When when this molecule goes under the composition, it will actually form water. It's much more stable than hydrogen came. And the extra oxygen Well, uh, find another extra oxygen to form oxygen. Okay, So, actually, we need to hear to balance this equation and to hear. So that important information from here is the We produced one mole off 02 given two moles off hydrogen peroxide. Okay. Ah, Another important note is the standard temperature and pressure. Can't recall that. That is 273 Calvin in one a. T. M. Camp. Oops. Recall that now we can go ahead and compute the number off most of oxygen that will be produced. Okay. All right. So the first thing, what's the for the starting point? We know that we used 10 milliliters off the solution. So I'm going to use that information tan middle letters off this solution. Okay? And we know that the solutions 3%. That means that I have three grams off hydrogen peroxide. Okay, for each 100 milliliters off solution. Great. So if you compute this look, you will find a mass off hydrogen peroxide in this 10 middle leaders. Okay, So, having the mass, the next step is to convert that to moles using them or mess. So one mole off hydrogen peroxide has 34 grams. So this is the molar mass. A camp. All right. So adding this new factor could this with this Oops, I forgot a to hear hydrogen peroxide. So putting in this factor, we will have the number of moles of hydrogen peroxide. Now, from our reaction, we know the ratio off oxygen and hydrogen peroxide that will, uh, and that we will have in this reaction during this transformation. So one mole off oxygen right here is produced for each two moles off hydrogen peroxide. So we put two moles off age too. Oh, too raped. So that's everything we need and computing all this. You should get 4.4. I'm staying to the negative three. No. So that's the number off malls off oxygen that were producing from this 10 milliliters of solution. Great. So what now? Well, if we have the number of malls, we also have temperature and pressure. Remember the we're on the STP. We can actually compute the volume off the oxygen or any gas, Right? Given that information. So the volume will be number of malls. Gas Causton temperature divided by pressure. Let's plant those numbers in number of malls. Okay, Uh, now are I'm gonna choose 0.8 to a T M leader for Calhoun Perm. All those air Dione. It's, um And the temperature will be to 73 Kelvin's hoop and the pressure is just one 18. Okay, so the only thing to be careful here is, um, first temperature, always calving. Okay, You don't want sell shoes. And also the units off the are that you choose. They have to match. So we going to verify that? Let's do this, Samo. We cancel with mall Calvin with Calvin, a team would ate him so that final unit is litter clean. And if you compute that, you should get something like 0.0, nine a blizter. Okay, so that is equivalent to more or less nine a mill letters. Okay, So the final step, which is item B, is to compute the ratio between the volume of oxygen and the volume of the solution that we started. So remember that we started from 10 milliliters of solution. So all we have to do for be is to take the ratio nine a over 10 and that is obviously 9.19 point eight.

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