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Chapter 9: Problem 31

What is the mass percent of each element in hydrogen peroxide, \(\mathrm{H}_{2} \mathrm{O}_{2} ?\)

Short Answer

Expert verified
In hydrogen peroxide (\(\mathrm{H}_{2}\mathrm{O}_{2}\)), the mass percent of hydrogen is approximately 5.88% and the mass percent of oxygen is approximately 94.12%.

Step by step solution

01

Find the molar mass of hydrogen peroxide

The molecular formula of hydrogen peroxide is \(\mathrm{H}_{2}\mathrm{O}_{2}\). To find the molar mass, we need to add up the molar masses of all the elements in the molecule. The molar masses of hydrogen (H) and oxygen (O) are respectively 1 g/mol and 16 g/mol. So, the molar mass of hydrogen peroxide is: Molar mass of \(\mathrm{H}_{2}\mathrm{O}_{2} = 2 \times 1 + 2 \times 16 = 34\,\text{g/mol}\).
02

Calculate the mass percent of hydrogen

Now that we have the molar mass of hydrogen peroxide, we can determine the mass percent of hydrogen (H). The mass of 2 moles of hydrogen in the molecule is: Mass of hydrogen = 2 × 1 = 2 g Next, we'll calculate the mass percentage of hydrogen: Mass percent of hydrogen = \(\frac{\text{mass of hydrogen}}{\text{molar mass of }\mathrm{H}_{2}\mathrm{O}_{2}}\) × 100% = \(\frac{2}{34}\times100\% \approx 5.88\%\)
03

Calculate the mass percent of oxygen

Next, we calculate the mass percent of oxygen (O). The mass of 2 moles of oxygen in the molecule is: Mass of oxygen = 2 × 16 = 32 g Now, determine the mass percentage of oxygen: Mass percent of oxygen = \(\frac{\text{mass of oxygen}}{\text{molar mass of }\mathrm{H}_{2}\mathrm{O}_{2}}\) × 100% = \(\frac{32}{34}\times100\% \approx 94.12\%\) So, the mass percent of hydrogen and oxygen in hydrogen peroxide (\(\mathrm{H}_{2}\mathrm{O}_{2}\)) are approximately 5.88% and 94.12%, respectively.

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Most popular questions from this chapter

(a) What is the molar mass of sucrose \(\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right) ?\) (b) What is the mass of \(1.25\) moles of sucrose? (c) How many sucrose molecules are in \(1.25\) moles? (d) How many hydrogen atoms are in \(1.25\) moles of sucrose? (e) What is the mass in grams of the hydrogen atoms in part (d)?

Which has the greatest mass: 1 mole of ethylene gas \(\left(\mathrm{C}_{2} \mathrm{H}_{4}\right), 1\) mole of carbon monoxide gas, or 1 mole of nitrogen gas \(\left(\mathrm{N}_{2}\right) ?\)

How many grams of sulfur hexafluoride would you need to have \(5.25 \times 10^{24}\) fluorine atoms?

Ethylene gas \(\left(\mathrm{C}_{2} \mathrm{H}_{4}\right)\) reacts with fluorine gas \(\left(\mathrm{F}_{2}\right)\) to form carbon tetrafluoride gas and hydrogen fluoride gas. If \(2.78 \mathrm{~g}\) of ethylene reacted with an excess of fluorine, how many grams of each product could theoretically be produced?

A \(2.230-\mathrm{g}\) sample of a solid is subjected to combustion analysis, yielding \(76.59 \% \mathrm{C}\) and \(6.39 \% \mathrm{H}\). It may also contain oxygen. (a) What is the empirical formula for this compound? (b) The molar mass of this compound is determined to be about \(94 \mathrm{~g} / \mathrm{mol}\). What is the molecular formula for this compound?
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