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Chapter 3: Problem 25

Calculate the molar mass of a compound if 0.372 mole of it has a mass of \(152 \mathrm{~g}\).

Short Answer

Expert verified
The molar mass of the compound is approximately \(408.6 \frac{g}{mole}\).

Step by step solution

01

Identify the given values

First, we identify our given values. We are told that 0.372 moles of the compound have a mass of 152g.
02

Write down the formula to calculate molar mass

The formula for calculating molar mass is: \(Molar Mass = \frac{Given Mass}{Number of Moles}\). This formula gives us the mass of one mole of the compound.
03

Substitute the given values into the formula

Next, we substitute our given values into our formula: \(Molar Mass = \frac{152g}{0.372 mole}\).
04

Calculate the molar mass

Finally, we calculate the molar mass by doing the division: \(Molar Mass ≈ 408.6 \frac{g}{mole}\).

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Most popular questions from this chapter

Consider the combustion of carbon monoxide (CO) in oxygen gas $$ 2 \mathrm{CO}(g)+\mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{CO}_{2}(g) $$ Starting with 3.60 moles of \(\mathrm{CO},\) calculate the number of moles of \(\mathrm{CO}_{2}\) produced if there is enough oxygen gas to react with all of the CO.

A sample containing \(\mathrm{NaCl}, \mathrm{Na}_{2} \mathrm{SO}_{4},\) and \(\mathrm{NaNO}_{3}\) gives the following elemental analysis: Na: 32.08 percent; O: 36.01 percent; Cl: 19.51 percent. Calculate the mass percent of each compound in the sample.

The atomic masses of \({ }_{3}^{6} \mathrm{Li}\) and \({ }_{3}^{7} \mathrm{Li}\) are \(6.0151 \mathrm{amu}\) and 7.0160 amu, respectively. Calculate the natural abundances of these two isotopes. The average atomic mass of Li is 6.941 amu.

Propane \(\left(\mathrm{C}_{3} \mathrm{H}_{8}\right)\) is a component of natural gas and is used in domestic cooking and heating. (a) Balance the following equation representing the combustion of propane in air: $$ \mathrm{C}_{3} \mathrm{H}_{8}+\mathrm{O}_{2} \longrightarrow \mathrm{CO}_{2}+\mathrm{H}_{2} \mathrm{O} $$ (b) How many grams of carbon dioxide can be produced by burning 3.65 moles of propane? Assume that oxygen is the excess reagent in this reaction.

Use ammonia \(\left(\mathrm{NH}_{3}\right)\) to explain what is meant by the percent composition by mass of a compound.
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