A piece of aluminum foil 1.00 cm square and 0.560 ...

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A piece of aluminum foil 1.00 cm square and 0.560 mm thick is allowed to react with bromine to form aluminum bromide.How many moles of aluminum were used? (The density of aluminum is 2.699 g/cm3.)

Jules Bruno · Accepted Answer

We are being asked to calculate the number of moles of aluminum used.We are given the following measurementsarea aluminum foil = 1.00 cm2thickness aluminum foil = 0.560 mmdensity aluminum = 2.699 g/cm3mol aluminum = ?To calculate the number of moles, we will use dimensional analysis.Recall: We use dimensional analysis as a fail proof process to convert from one unit to another.[readmore]We also need to take note of the following when doing unit conversions:• Put units you need to cancel out on opposite places (i.e. if it’s in the numerator then put the conversion factor with the same unit in the denominator)• Always raise the units to the necessary number especially when dealing with volume, area, etc.First, we need to calculate the volume of aluminumRecall: Volume is the quantity of three-dimensional space enclosed by a closed surface. Volume = area × widthWe convert mm to cm for us to be able to cancel out the unitsthickness Al = 0.560 mm ×10-1 cm1 mmthickness Al = 0.0560 cmWe plug in the values into the formulaVolume Al= 1.00 cm2×0.0560 cmvolume Al= 0.0560 cm3We calculate the mass of aluminum using density then convert it to molRecall: Density represents the mass of an object or compound within a given volume. Density = mass / volumeTo determine mass, we isolate mass on one side of the equationvolumeDensity = massvolume volumeWe have the formula for mass from densitymass = Density × volumeWe plug in the values into the formulamass Al = 2.699 gcm3 × 0.0560 cm3mass Al = 0.151144 g Next, convert mass to mol using molar massRecall: The molar mass is the mass of a given chemical element or chemical compound (g) divided by the amount of substance (mol).Molar mass =gramsmolTo calculate mol, we isolate mol on one side of the equationmolMolar mass =gramsmolmolmolMolar mass Molar mass=gramsMolar massWe have the formula of mol from molar massmol=gramsMolar massThe molar mass of aluminum based from the periodic table is 26.98 g/molSubstitute the values into the formulamolar mass Al = 26.98 g/molmass Al = 0.151144 gmol Al=0.151144 g26.98 gmolmol = 0.0056 mol AlThere were 0.0056 moles of aluminum used.

Problem: A piece of aluminum foil 1.00 cm square and 0.560 mm thick is allowed to react with bromine to form aluminum bromide.How many moles of aluminum were used? (The density of aluminum is 2.699 g/cm3.)

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Problem: A piece of aluminum foil 1.00 cm square and 0.560 mm thick is allowed to react with bromine to form aluminum bromide.How many moles of aluminum were used? (The density of aluminum is 2.699 g/cm3.)

FREE Expert Solution

Problem Details

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