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QuestionHow many grams of hydrogen H2\mathrm{H}_{2} are produced in the reaction: 2Al+6HCl→2AlCl3+3H22 \mathrm{Al} + 6 \mathrm{HCl} \rightarrow 2 \mathrm{AlCl}_{3} + 3 \mathrm{H}_{2}? A. 2.02 g B. 539.38 g C. 101.86 g D. 6.06 g

Studdy Solution

STEP 1

Assumptions1. The balanced chemical equation is given as Al+6HCl→AlCl3+3H \mathrm{Al} +6 \mathrm{HCl} \rightarrow \mathrm{AlCl}_{3} +3 \mathrm{H}_{} . The mass of Al used in the reaction is53.96 g3. The mass of HCl used in the reaction is218.76 g4. The mass of AlCl3 formed in the reaction is266.66 g5. We need to find the mass of H formed in the reaction

STEP 2

We can use the concept of stoichiometry to solve this problem. Stoichiometry is a section of chemistry that involves using relationships between reactants and/or products in a chemical reaction to determine desired quantitative data.

STEP 3

First, we need to determine the molar mass of Al and H2. The molar mass of Al is approximately26.98 g/mol and the molar mass of H2 is approximately2.02 g/mol.

STEP 4

Next, we need to calculate the number of moles of Al used in the reaction. We can do this by dividing the mass of Al by its molar mass.
Moles of Al=Mass of AlMolar mass of Al\text{Moles of Al} = \frac{\text{Mass of Al}}{\text{Molar mass of Al}}

STEP 5

Now, plug in the given values for the mass of Al and the molar mass of Al to calculate the number of moles of Al.
Moles of Al=53.96 g26.98 g/mol\text{Moles of Al} = \frac{53.96 \, \text{g}}{26.98 \, \text{g/mol}}

STEP 6

Calculate the number of moles of Al.
Moles of Al=53.96 g26.98 g/mol=2 moles\text{Moles of Al} = \frac{53.96 \, \text{g}}{26.98 \, \text{g/mol}} =2 \, \text{moles}

STEP 7

From the balanced chemical equation, we can see that2 moles of Al react to produce3 moles of H2. Therefore, the number of moles of H2 produced is3.

STEP 8

Now, we can calculate the mass of H2 produced in the reaction by multiplying the number of moles of H2 by its molar mass.
Mass of H2=Moles of H2×Molar mass of H2\text{Mass of H}_{2} = \text{Moles of H}_{2} \times \text{Molar mass of H}_{2}

STEP 9

Plug in the values for the number of moles of H2 and the molar mass of H2 to calculate the mass of H2.
Mass of H2=3 moles×2.02 g/mol\text{Mass of H}_{2} =3 \, \text{moles} \times2.02 \, \text{g/mol}

STEP 10

Calculate the mass of H2.
Mass of H2=3 moles×2.02 g/mol=6.06 g\text{Mass of H}_{2} =3 \, \text{moles} \times2.02 \, \text{g/mol} =6.06 \, \text{g}Therefore, the mass of H2 formed in the reaction is6.06 grams.

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