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Chapter 9: Problem 17

What quantity serves as the conversion factor between the mass of a sample and how many moles the sample contains?

Short Answer

Expert verified
The quantity that serves as the conversion factor between the mass of a sample and the number of moles the sample contains is the molar mass of the substance, usually expressed in grams per mole (g/mol).

Step by step solution

01

Remember the concept of molar mass

Molar mass is the mass of one mole of a substance, usually expressed in grams per mole (g/mol). It is numerically equivalent to the molecular weight of the substance, but it has a unit of mass. To find the molar mass of a substance, you need to know its chemical formula and the atomic masses of its constituent elements.
02

Understand how molar mass works as a conversion factor

Molar mass can be used as a conversion factor between the mass of a sample and the number of moles it contains. To calculate the number of moles in a given mass of a substance, you can divide the given mass by the substance's molar mass: Number of moles = \(\frac{\text{mass of sample}}{\text{molar mass}}\) This equation allows you to convert between mass and the number of moles for any substance, as long as you know the molar mass of the substance.
03

Identify the conversion factor

In this exercise, we are asked to find the conversion factor between the mass of a sample and the number of moles it contains. Based on our analysis and understanding of molar mass, the conversion factor we are looking for is the molar mass of the substance. In summary, the quantity that serves as the conversion factor between the mass of a sample and the number of moles the sample contains is the molar mass of the substance.

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Most popular questions from this chapter

The more reactive halogen elements are able to replace the less reactive halogens from their compounds. $$\begin{array}{l} \mathrm{Cl}_{2}(g)+\mathrm{NaI}(a q) \rightarrow \mathrm{NaCl}(a q)+\mathrm{I}_{2}(s) \\ \mathrm{Br}_{2}(l)+\mathrm{NaI}(a q) \rightarrow \mathrm{NaBr}(a q)+\mathrm{I}_{2}(s) \end{array}$$ Suppose separate solutions each containing \(25.0 \mathrm{g}\) of NaI are available. If \(5.00 \mathrm{g}\) of \(\mathrm{Cl}_{2}\) gas is bubbled into one NaI solution, and \(5.00 \mathrm{g}\) of liquid bromine is added to the other, calculate the number of grams of elemental iodine produced in each case.

When the sugar glucose, \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6},\) is burned in air, carbon dioxide and water vapor are produced. Write the balanced chemical equation for this process, and calculate the theoretical yield of carbon dioxide when \(1.00 \mathrm{g}\) of glucose is burned completely.

When elemental carbon is burned in the open atmosphere, with plenty of oxygen gas present, the product is carbon dioxide. $$\mathrm{C}(s)+\mathrm{O}_{2}(g) \rightarrow \mathrm{CO}_{2}(g)$$ However, when the amount of oxygen present during the burning of the carbon is restricted, carbon monoxide is more likely to result. $$2 \mathrm{C}(s)+\mathrm{O}_{2}(g) \rightarrow 2 \mathrm{CO}(g)$$What mass of each product is expected when a \(5.00-\mathrm{g}\) sample of pure carbon is burned under each of these conditions?

A student calculated the theoretical yield of barium sulfate in a precipitation experiment to be \(1.352 \mathrm{g}\) When she filtered, dried, and weighed her precipitate, however, her yield was only \(1.279 \mathrm{g}\). Calculate the student's percent yield.

Although mass is a property of matter we can conveniently measure in the laboratory, the coefficients of a balanced chemical equation are not directly interpreted on the basis of mass. Explain why.
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