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Chapter 3: Problem 2

A student makes two different compounds of nitrogen and oxygen using the masses shown below. In both cases, all of the elemental substances are completely used up. Compound \(1 \quad 10.0 \mathrm{~g}\) nitrogen \(+11.42 \mathrm{~g}\) oxygen Compound \(2 \quad 10.0 \mathrm{~g}\) nitrogen \(+22.84 \mathrm{~g}\) oxygen What is the percent oxygen in each compound?

Short Answer

Expert verified
The percent of oxygen in Compound 1 is 53.3% and in Compound 2 is 69.5%.

Step by step solution

01

Calculating the total mass of each compound

First, we need to calculate the total mass of each compound by adding the mass of nitrogen and the mass of oxygen. For Compound 1: Total mass = mass of nitrogen + mass of oxygen = 10.0 g + 11.42 g For Compound 2: Total mass = mass of nitrogen + mass of oxygen = 10.0 g + 22.84 g
02

Calculate the percent of oxygen in each compound

To find the percent of oxygen in each compound, we need to divide the mass of oxygen by the total mass of the compound and multiply by 100. For Compound 1: Percent oxygen = \( \frac{mass_{oxygen}}{total_{mass}}\times 100\% \) = \( \frac{11.42\mathrm{~g}}{10\mathrm{~g} + 11.42\mathrm{~g}}\times 100\% \) For Compound 2: Percent oxygen = \( \frac{mass_{oxygen}}{total_{mass}}\times 100\% \) = \( \frac{22.84\mathrm{~g}}{10\mathrm{~g} + 22.84\mathrm{~g}}\times 100\% \)
03

Calculate the percent of oxygen in each compound

Now, we will use the formulas we found in step 2 to calculate the actual percentages. For Compound 1: Percent oxygen = \( \frac{11.42\mathrm{~g}}{21.42\mathrm{~g}}\times 100\% \) = 53.3 % For Compound 2: Percent oxygen = \( \frac{22.84\mathrm{~g}}{32.84\mathrm{~g}}\times 100\% \) = 69.5 % So, the percent of oxygen in Compound 1 is 53.3% and in Compound 2 is 69.5%.

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Most popular questions from this chapter

For each pair, indicate which atom loses an electron more easily: (a) \(\mathrm{Na}\) or \(\mathrm{K}\) (b) Na or Al (c) \(\mathrm{Rb}\) or \(\mathrm{Ca}\) (d) \(\mathrm{S}\) or \(\mathrm{Cl}\) (e) Br or Kr

(a) The elements in group IA (1) are called (b) The elements in group IIA (2) are called (c) The elements in group VIIA(17) are called (d) The elements in group VIIIA (18) are called

Fill in the following table: $$ \begin{array}{lcccc} & { }_{8}^{15} \mathrm{O}^{+} & ? & ? & ? \\ \hline \text { Mass number } & ? & 27 & ? & 58 \\ \text { Atomic number } & ? & ? & 15 & ? \\ \text { Number of protons } & ? & 13 & ? & ? \\ \text { Number of neutrons } & ? & ? & 16 & 30 \\ \text { Number of electrons } & ? & ? & ? & 27 \\ \text { Charge on ion } & ? & +3 & -3 & +1 \\ \hline \end{array} $$

Although not discussed until the next chapter, what process do you think chemists mean by an atom's second ionization energy?

Explain the difference between mass number and atomic mass.
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