Chromium metal can be produced from the high-temperature reaction of Cr2 O3 [chromium(III) oxide

step 1 Okay, now problem 64, they require you to calculate the mass of aluminum to produce 500 grams ch

Chromium metal can be produced from the high-temperature...

Chromium metal can be produced from the high-temperature reaction of $\mathrm{Cr}_{2} \mathrm{O}_{3}$ [chromium(III) oxide] with silicon or aluminum by each of the following reactions:$$\begin{aligned} \mathrm{Cr}_{2} \mathrm{O}_{3}(s)+2 \mathrm{Al}(\ell) & \rightarrow 2 \mathrm{Cr}(\ell)+\mathrm{Al}_{2} \mathrm{O}_{3}(s) \\2 \mathrm{Cr}_{2} \mathrm{O}_{3}(s)+3 \mathrm{Si}(\ell) & \rightarrow 4 \mathrm{Cr}(\ell)+3 \mathrm{SiO}_{2}(s)\end{aligned}$$.a. Calculate the number of grams of aluminum required to prepare $400.0 \mathrm{g}$ of chromium metal by the first reaction. b. Calculate the number of grams of silicon required to prepare $400.0 \mathrm{g}$ of chromium metal by the second reaction.

Chromium metal can be produced from the high-temperature reaction of $\mathrm{Cr}_{2} \mathrm{O}_{3}$ [chromium(III) oxide] with silicon or aluminum by each of the following reactions:$$\begin{aligned}
\mathrm{Cr}_{2} \mathrm{O}_{3}(s)+2 \mathrm{Al}(\ell) & \rightarrow 2 \mathrm{Cr}(\ell)+\mathrm{Al}_{2} \mathrm{O}_{3}(s) \\2 \mathrm{Cr}_{2} \mathrm{O}_{3}(s)+3 \mathrm{Si}(\ell) & \rightarrow 4 \mathrm{Cr}(\ell)+3 \mathrm{SiO}_{2}(s)\end{aligned}$$.a. Calculate the number of grams of aluminum required to prepare $400.0 \mathrm{g}$ of chromium metal by the first reaction.
b. Calculate the number of grams of silicon required to prepare $400.0 \mathrm{g}$ of chromium metal by the second reaction.

Labs

Want to see this concept in action?

NEW

Explore this concept interactively to see how it behaves as you change inputs.

View Labs

Key Concepts

Stoichiometry

Stoichiometry involves using the mole ratios from a balanced chemical equation to convert between amounts of reactants and products. By applying these ratios, one can determine the precise amount of each reactant required to form a specific amount of product.

Molar Mass

Molar mass is the mass of one mole of a substance, expressed in grams per mole. It serves as a conversion factor between the mass of a substance and the number of moles. This is necessary to convert measured masses into moles for use in stoichiometric calculations.

Mole Concept

The mole concept is fundamental in chemistry as it provides a way to relate the number of particles (atoms, molecules, ions) to measurable amounts of substances in grams by using Avogadro’s number. This concept allows us to move from the microscopic scale to macroscopic amounts and is essential when converting given masses into moles.

Balanced Chemical Equations

Balanced chemical equations are crucial because they reflect the conservation of mass by ensuring the same number of atoms for each element exists on both sides of the equation. They provide the stoichiometric coefficients needed to relate the amounts in moles of reactants and products, thereby allowing accurate calculations of required quantities.

Transcript

Please give Ace some feedback