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Magazine Chapter 2: Problem 34
How many moles of each element are in one mole of each compound? a. \(\mathrm{H}_{2} \mathrm{O}_{2}\) b. \(\mathrm{N}_{2} \mathrm{O}_{5}\) ?. \(\mathrm{PF}_{3}\) d. \(\mathrm{MgCl}_{2}\) e. \(\mathrm{KBr}\) f. \(\mathrm{AlCl}_{3}\) g. \(\mathrm{CaO}\) h. \(\mathrm{Na}_{2} \mathrm{~S}\) i. \(\mathrm{NH}_{3}\) j. \(\mathrm{CO}_{2}\) k. \(\mathrm{N}_{2} \mathrm{H}_{4}\) l. \(\mathrm{N}_{2} \mathrm{O}\)
Short Answer
Expert verified
Each compound's moles: a. 2 H and 2 O, b. 2 N and 5 O, c. 1 P and 3 F, d. 1 Mg and 2 Cl, e. 1 K and 1 Br, f. 1 Al and 3 Cl, g. 1 Ca and 1 O, h. 2 Na and 1 S, i. 1 N and 3 H, j. 1 C and 2 O, k. 2 N and 4 H, l. 2 N and 1 O.
Step by step solution
01
Understanding the Problem
To find the number of moles of each element in one mole of a compound, we need to look at the subscripts in the chemical formula of each compound. These subscripts indicate the number of atoms of each element per molecule of the compound, which aligns with the number of moles for each element per mole of the compound.
02
Analyze Compound a: \(\mathrm{H}_2 \mathrm{O}_2\)
In \(\mathrm{H}_2 \mathrm{O}_2\), each molecule contains 2 atoms of hydrogen and 2 atoms of oxygen. Thus, in one mole of \(\mathrm{H}_2 \mathrm{O}_2\), there are 2 moles of hydrogen and 2 moles of oxygen.
03
Analyze Compound b: \(\mathrm{N}_2 \mathrm{O}_5\)
In \(\mathrm{N}_2 \mathrm{O}_5\), each molecule contains 2 atoms of nitrogen and 5 atoms of oxygen. Therefore, in one mole of \(\mathrm{N}_2 \mathrm{O}_5\), there are 2 moles of nitrogen and 5 moles of oxygen.
04
Analyze Compound c: \(\mathrm{PF}_3\)
In \(\mathrm{PF}_3\), each molecule contains 1 atom of phosphorus and 3 atoms of fluorine. Therefore, in one mole of \(\mathrm{PF}_3\), there is 1 mole of phosphorus and 3 moles of fluorine.
05
Analyze Compound d: \(\mathrm{MgCl}_2\)
In \(\mathrm{MgCl}_2\), each molecule contains 1 atom of magnesium and 2 atoms of chlorine. Therefore, in one mole of \(\mathrm{MgCl}_2\), there is 1 mole of magnesium and 2 moles of chlorine.
06
Analyze Compound e: \(\mathrm{KBr}\)
In \(\mathrm{KBr}\), each molecule contains 1 atom of potassium and 1 atom of bromine. Therefore, in one mole of \(\mathrm{KBr}\), there is 1 mole of potassium and 1 mole of bromine.
07
Analyze Compound f: \(\mathrm{AlCl}_3\)
In \(\mathrm{AlCl}_3\), each molecule contains 1 atom of aluminum and 3 atoms of chlorine. Therefore, in one mole of \(\mathrm{AlCl}_3\), there is 1 mole of aluminum and 3 moles of chlorine.
08
Analyze Compound g: \(\mathrm{CaO}\)
In \(\mathrm{CaO}\), each molecule contains 1 atom of calcium and 1 atom of oxygen. Therefore, in one mole of \(\mathrm{CaO}\), there is 1 mole of calcium and 1 mole of oxygen.
09
Analyze Compound h: \(\mathrm{Na}_2 \mathrm{S}\)
In \(\mathrm{Na}_2 \mathrm{S}\), each molecule contains 2 atoms of sodium and 1 atom of sulfur. Therefore, in one mole of \(\mathrm{Na}_2 \mathrm{S}\), there are 2 moles of sodium and 1 mole of sulfur.
10
Analyze Compound i: \(\mathrm{NH}_3\)
In \(\mathrm{NH}_3\), each molecule contains 1 atom of nitrogen and 3 atoms of hydrogen. Therefore, in one mole of \(\mathrm{NH}_3\), there is 1 mole of nitrogen and 3 moles of hydrogen.
11
Analyze Compound j: \(\mathrm{CO}_2\)
In \(\mathrm{CO}_2\), each molecule contains 1 atom of carbon and 2 atoms of oxygen. Therefore, in one mole of \(\mathrm{CO}_2\), there is 1 mole of carbon and 2 moles of oxygen.
12
Analyze Compound k: \(\mathrm{N}_2 \mathrm{H}_4\)
In \(\mathrm{N}_2 \mathrm{H}_4\), each molecule contains 2 atoms of nitrogen and 4 atoms of hydrogen. Therefore, in one mole of \(\mathrm{N}_2 \mathrm{H}_4\), there are 2 moles of nitrogen and 4 moles of hydrogen.
13
Analyze Compound l: \(\mathrm{N}_2 \mathrm{O}\)
In \(\mathrm{N}_2 \mathrm{O}\), each molecule contains 2 atoms of nitrogen and 1 atom of oxygen. Therefore, in one mole of \(\mathrm{N}_2 \mathrm{O}\), there are 2 moles of nitrogen and 1 mole of oxygen.
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Chemical Formulas
Chemical formulas act as the essential language of chemistry, representing how elements combine to form compounds. Each formula provides crucial information about the elements involved and their respective proportions.
- The letters in a formula signify the elements present in the compound. For example, in \( \mathrm{H_2O} \), "H" stands for hydrogen, while "O" stands for oxygen.
- Subscripts (small numbers written at the bottom right of an element symbol) indicate the number of atoms present. In \( \mathrm{H_2O} \), the "2" tells us there are two hydrogen atoms for every one oxygen atom.
Molar Ratios
Molar ratios are derived directly from chemical formulas and serve as a bridge between molecular composition and chemical equations. This concept is critical for converting between the microscopic world of atoms and the macroscopic world of moles.
- A molar ratio is a proportional comparison between the amounts of different elements in a compound. For example, in \( \mathrm{PF_3} \), the ratio of phosphorus to fluorine is 1:3.
- This ratio doesn't just apply to individual molecules. It scales up to moles as well, allowing chemists to easily convert between atoms and moles while performing calculations.
Element Composition
Element composition refers to the distribution and proportion of each element within a compound. It highlights the specific number of each type of atom in a compound, providing a deeper understanding of its chemical makeup.
- For example, \( \mathrm{KBr} \) is composed of one potassium atom and one bromine atom per molecule, indicating a 1:1 ratio.
- This concept allows chemists to quantitatively describe the compound's makeup, crucial for applications in both synthesis and analysis.
Stoichiometry
Stoichiometry is the quantitative cornerstone of chemistry. It involves using balanced chemical equations to calculate the relationships between reactants and products in a chemical reaction.
- It encompasses various calculations, including determining the amount of elements or compounds needed or produced in a reaction.
- Stoichiometry uses the concept of moles as a counting unit, allowing for precise measurements in reactions.
