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Chapter 9: Problem 48

In words, what is the mass of 1 mole of any molecule?

Short Answer

Expert verified
The mass of 1 mole of any molecule is equal to the molecular weight of that molecule expressed in grams per mole.

Step by step solution

01

Definition of a mole

A mole is a standard unit of measurement used in chemistry to express the amount of particles (atoms, molecules, ions, or electrons) in a substance. One mole of any substance contains Avogadro's number (\(6.022 \times 10^{23}\)) of particles.
02

Molecular weight

Molecular weight is the sum of the atomic weights of all the atoms present in a molecule. The atomic weight of an element is expressed in atomic mass units (amu) and is approximately equal to the number of protons and neutrons contained within the nucleus of an atom.
03

Mass of one mole

To find the mass of one mole of any molecule, we need to multiply its molecular weight by the molar mass constant, which is 1 gram per mole (g/mol). The molecular weight of a molecule will depend on the specific substance, but the mass of one mole of any molecule can be found using the expression: Mass of 1 mole = Molecular weight (g/mol) In words, the mass of one mole of any molecule is equal to the molecular weight of that molecule expressed in grams per mole.

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Most popular questions from this chapter

Consider the following unbalanced chemical equation: \(\mathrm{P}+\mathrm{O}_{2} \rightarrow \mathrm{P}_{2} \mathrm{O}_{5}\) (a) How many grams of phosphorus (P) are required to react completely with \(20.0 \mathrm{~g}\) of \(\mathrm{O}_{2} ?\) (b) What is the theoretical yield in grams if you combine the amounts of reactants in part (a)?

A \(2.230-\mathrm{g}\) sample of a solid is subjected to combustion analysis, yielding \(76.59 \% \mathrm{C}\) and \(6.39 \% \mathrm{H}\). It may also contain oxygen. (a) What is the empirical formula for this compound? (b) The molar mass of this compound is determined to be about \(94 \mathrm{~g} / \mathrm{mol}\). What is the molecular formula for this compound?

(a) Write a balanced chemical equation for the combustion of \(\mathrm{CH}_{4}(\mathrm{~g})\) with \(\mathrm{O}_{2}(g)\) to form \(\mathrm{CO}_{2}(g)\) and \(\mathrm{H}_{2} \mathrm{O}(g)\) (b) Consider the reaction of three molecules of \(\mathrm{CH}_{4}(g)\) with four molecules of \(\mathrm{O}_{2}(g)\). The following boxes represent before and after pictures of the tiny, sealed container in which this reaction takes place. Draw pictures to show the contents of this container before and after the reaction happens:

Ethylene glycol, used for antifreeze, has the molecular formula \(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}_{2}\). Calculate the mass percent of each element in ethylene glycol.

What is the maximum possible value of the percent yield of a chemical reaction?
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