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Chapter 3: Problem 33

Carbon has two stable isotopes, \({ }_{6}^{12} \mathrm{C}\) and \({ }_{6}^{13} \mathrm{C},\) and fluorine has only one stable isotope, \({ }_{9}^{19} \mathrm{~F}\). How many peaks would you observe in the mass spectrum of the positive ion of \(\mathrm{CF}_{4}^{+}\) ? Assume that the ion does not break up into smaller fragments.

Short Answer

Expert verified
There will be two peaks observed in the mass spectrum for the positive ion \(\mathrm{CF_4}^{+}\).

Step by step solution

01

Identify Isotopes and Possible Combinations

We know that carbon has 2 isotopes (\({ }_{6}^{12}\mathrm{C}\), \({ }_{6}^{13}\mathrm{C}\)) and fluorine has 1 isotope (\({ }_{9}^{19}\mathrm{F}\)). The molecule in question is \(\mathrm{CF_4}\). Therefore, the possible combinations for \(\mathrm{CF_4}\) are \({ }_{6}^{12}\mathrm{CF_4}\) and \({ }_{6}^{13}\mathrm{CF_4}\).
02

Calculate Total Masses for Each Combination

To calculate the total mass, add the mass number of carbon isotope to the mass of 4 fluorine isotopes. This gives us: - For \({ }_{6}^{12}\mathrm{CF_4}\), total mass = 12 (C) + 4 * 19 (F) = 88. - For \({ }_{6}^{13}\mathrm{CF_4}\), total mass = 13 (C) + 4 * 19 (F) = 89.
03

Identify Mass Spectrum Peaks

In mass spectroscopy, each different mass-to-charge ratio translates to a different peak. Since the ion \(\mathrm{CF_4}^{+}\) doesn't break up into smaller fragments, we consider the whole mass of each molecule. Therefore, we will have two peaks in the mass spectrum, corresponding to the two combinations from step 2.

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Most popular questions from this chapter

Balance the following equations using the method outlined in Section 3.7 : (a) \(\mathrm{C}+\mathrm{O}_{2} \longrightarrow \mathrm{CO}\) (b) \(\mathrm{CO}+\mathrm{O}_{2} \longrightarrow \mathrm{CO}_{2}\) (c) \(\mathrm{H}_{2}+\mathrm{Br}_{2} \longrightarrow \mathrm{HBr}\) (d) \(\mathrm{K}+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{KOH}+\mathrm{H}_{2}\) (e) \(\mathrm{Mg}+\mathrm{O}_{2} \longrightarrow \mathrm{MgO}\) (f) \(\mathrm{O}_{3} \longrightarrow \mathrm{O}_{2}\) (g) \(\mathrm{H}_{2} \mathrm{O}_{2} \longrightarrow \mathrm{H}_{2} \mathrm{O}+\mathrm{O}_{2}\) (h) \(\mathrm{N}_{2}+\mathrm{H}_{2} \longrightarrow \mathrm{NH}_{3}\) (i) \(\mathrm{Zn}+\mathrm{AgCl} \longrightarrow \mathrm{ZnCl}_{2}+\mathrm{Ag}\) (j) \(\mathrm{S}_{8}+\mathrm{O}_{2} \longrightarrow \mathrm{SO}_{2}\) (k) \(\mathrm{NaOH}+\mathrm{H}_{2} \mathrm{SO}_{4} \longrightarrow \mathrm{Na}_{2} \mathrm{SO}_{4}+\mathrm{H}_{2} \mathrm{O}\) (l) \(\mathrm{Cl}_{2}+\mathrm{NaI} \longrightarrow \mathrm{NaCl}+\mathrm{I}_{2}\) \((\mathrm{m}) \mathrm{KOH}+\mathrm{H}_{3} \mathrm{PO}_{4} \longrightarrow \mathrm{K}_{3} \mathrm{PO}_{4}+\mathrm{H}_{2} \mathrm{O}\) (n) \(\mathrm{CH}_{4}+\mathrm{Br}_{2} \longrightarrow \mathrm{CBr}_{4}+\mathrm{HBr}\)

One of the reactions that occurs in a blast furnace, where iron ore is converted to cast iron, is $$ \mathrm{Fe}_{2} \mathrm{O}_{3}+3 \mathrm{CO} \longrightarrow 2 \mathrm{Fe}+3 \mathrm{CO}_{2} $$ Suppose that \(1.64 \times 10^{3} \mathrm{~kg}\) of Fe are obtained from a \(2.62 \times 10^{3}-\mathrm{kg}\) sample of \(\mathrm{Fe}_{2} \mathrm{O}_{3}\). Assuming that the reaction goes to completion, what is the percent purity of \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) in the original sample?

Use the formation of water from hydrogen and oxygen to explain the following terms: chemical reaction, reactant, product.

Explain clearly what is meant by the statement "The atomic mass of gold is 197.0 amu."

Urea \(\left[\left(\mathrm{NH}_{2}\right)_{2} \mathrm{CO}\right]\) is used for fertilizer and many other things. Calculate the number of \(\mathrm{N}, \mathrm{C}, \mathrm{O},\) and \(\mathrm{H}\) atoms in \(1.68 \times 10^{4} \mathrm{~g}\) of urea.
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