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Chapter 3: Problem 122

\(\mathrm{XF}_{3}\) consists of \(65 \%\) F by mass. The atomic mass of the element X must be (a) 8 u; (b) 11 u; (c) 31 u; (d) 35 u.

Short Answer

Expert verified
The atomic mass of element X in the \(\mathrm{XF}_{3}\) compound is approximately 31u. Therefore, the correct choice is (c).

Step by step solution

01

Identify Given Information

The given information is that \(\mathrm{XF}_{3}\) consists of 65% Fluorine by mass. The atomic mass of Fluorine is 19u.
02

Calculate the Mass of Fluorine in the Compound

Based on the given composition, since there are three atoms of Fluorine in the compound, the total mass of Fluorine is \(3 \times 19u = 57u\).
03

Calculate the Remaining Mass of X

If Fluorine makes up 65% of the compound's mass, then the remaining 35% is element X. Therefore, we can use the equation (mass of compound) = (mass of Fluorine + mass of X) to calculate the mass of X. The total mass is \( \frac{57u}{0.65} \approx 87.69u\), which makes the mass of X approximately \(87.69u - 57u = 30.69u\).
04

Identify the Accurate Atomic Mass

Looking at the options, the atomic mass of X that is closest to the calculated mass is 31u, which means the correct choice is (c).

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Most popular questions from this chapter

Without doing detailed calculations, explain which of these compounds produces the greatest mass of \(\mathrm{H}_{2} \mathrm{O}\) when \(1.00 \mathrm{g}\) of the compound is burned in an excess of oxygen: \(\mathrm{CH}_{4}, \mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}, \mathrm{C}_{10} \mathrm{H}_{8}, \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{OH}\)

Explain which of the following statement(s) is (are) correct concerning glucose (blood sugar), \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\) (a) The percentages, by mass, of \(\mathrm{C}\) and \(\mathrm{O}\) are the same as in CO. (b) The ratio of \(\mathrm{C}: \mathrm{H}: \mathrm{O}\) atoms is the same as in dihydroxyacetone, \(\left(\mathrm{CH}_{2} \mathrm{OH}\right)_{2} \mathrm{CO}\) (c) The proportions, by mass, of \(C\) and \(O\) are equal. (d) The highest percentage, by mass, is that of H.

The important natural sources of boron compounds are the minerals kernite, \(\mathrm{Na}_{2} \mathrm{B}_{4} \mathrm{O}_{7} \cdot 4 \mathrm{H}_{2} \mathrm{O}\) and borax, \(\mathrm{Na}_{2} \mathrm{B}_{4} \mathrm{O}_{7} \cdot 10 \mathrm{H}_{2} \mathrm{O} .\) How much additional mass of mineral must be processed per kilogram of boron obtained if the mineral is borax rather than kernite?

Briefly describe each of the following ideas or methods: (a) mole of a compound; (b) structural formula; (c) oxidation state; (d) carbon-hydrogen- oxygen determination by combustion analysis.

Selenium, an element used in the manufacture of photoelectric cells and solar energy devices, forms two oxides. One has \(28.8 \%\) O, by mass, and the other, 37.8\% O. What are the formulas of these oxides? Propose acceptable names for them.
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