Question
Question: Which of the following contains the largest number of atoms? A. \(4{\text{g}}\) of \({{\text{H}}_2...
Which of the following contains the largest number of atoms?
A. 4g of H2
B. 16g of O2
C. 28g of N2
D. 18g of H2O
Solution
Stoichiometry is the study of the quantitative aspects of chemical reactions. Chemical equations are concise representations of chemical reactions. Mole is defined as the quantity of a substance that contains the same number of ultimate particles as are present in 12g of carbon−12.
Complete step by step answer:
Stoichiometry deals with the numerical relationships of elements and compounds and the mathematical proportions of reactants and products in chemical transformations. Concentration is the amount of solute dissolved in a given amount of solution. There are different types of concentration units. Formula and molecular mass deal with individual atoms and molecules. Mole is the unit that relates the number of particles and mass.
One mole of an element contains 6.022×1023 particles. This absolute number is called Avogadro’s number. Mass of one mole of substance is called molar mass. Or molar mass of an element is equal to the molecular weight.
A. Molar mass of H2, MH2=2g
Mass of H2, mH2=4g
Number of moles of H2, nH2=MH2mH2=2g.mol−14g=2mol
2mol of H2 contains 2×(6.022×1023) atoms.
B. Molar mass of O2, MO2=32g
Mass of O2, mO2=16g
Number of moles of O2, nO2=MO2mO2=32g.mol−116g=0.5mol
0.5mol of O2 contains 0.5×(6.022×1023) atoms.
C. Molar mass of N2, MN2=28g
Mass of N2, mN2=28g
Number of moles of N2, nN2=MN2mN2=28g.mol−128g=1mol
1mol of N2 contains 1×(6.022×1023) atoms.
D. Molar mass of H2O, MH2O=18g
Mass of H2O , mH2O=18g
Number of moles of H2O, nH2O=MH2OmH2O=18g.mol−118g=1mol
1mol of H2O contains 1×(6.022×1023) atoms.
Hence 4g of H2 contains 2×(6.022×1023) atoms which is larger than others.
Hence option A is correct.
Note:
Moles provide a bridge from molecular scale to real-world scale. One mole of molecules or formula units contain Avogadro number times the number of atoms or ions of each element in the compound. Each chemical equation provides information about the amount of reactants produced.