Answer:
5.73 g of solid copper, can be theoretically produced in this reaction.
Explanation:
We start from the begining with the balanced equation:
2Al (s) + 3CuSO₄ (aq) → Al₂(SO₄)₃ (aq) + 3Cu (s)
To determine the limiting reactant we need to know the moles of each.
2.2 g / 26.98 g/mol = 0.0815 moles of Al
14.4 g / 159.6 g/mol = 0.0902 moles of copper (II) sulfate.
Ratio is 2:3. Let's find out the limtiing reactant,
2 moles of Al react to 3 moles of copper (II) sulfate
Then 0.0815 moles of Al, may react to (0.0815 . 3) / 2 = 0.122 moles of salt.
We only have 0.0902 moles of sulfate and we need 0.122 moles to complete the reaction, as the sulfate we have, is not enough, the salt is the limting reagent. We use this to determine the solid copper that can be theoretically produced.
This ratio is 3:3, so If we have 0.0902 moles of copper (II) sulfate, we may produce 0.0902 moles of solid copper.
Let's conver the moles to mass → 0.0902 mol . 63.5 g/mol = 5.73 g
0.025 M will be the resulting concentration
Explanation:
To find the resulting concentration we use the following formula:
initial concentration × initial volume = final concentration × final volume
initial concentration = 0.15 M
initial volume = 2 mL
final concentration = ?
final volume = 10 + 2 = 12 mL
0.15 × 2 = final concentration × 12
final concentration = (0.15 × 2) / 12
final concentration = 0.025 M
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molar concentration
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Learning Objective
Define the law of conservation of mass
Key Points
The law of conservation of mass states that mass in an isolated system is neither created nor destroyed by chemical reactions or physical transformations.
According to the law of conservation of mass, the mass of the products in a chemical reaction must equal the mass of the reactants.
The law of conservation of mass is useful for a number of calculations and can be used to solve for unknown masses, such the amount of gas consumed or produced during a reaction.
Terms
reactantAny of the participants present at the start of a chemical reaction. Also, a molecule before it undergoes a chemical change.
law of conservation of massA law that states that mass cannot be created or destroyed; it is merely rearranged.
productA chemical substance formed as a result of a chemical reaction.
History of the Law of the Conservation of Mass
The ancient Greeks first proposed the idea that the total amount of matter in the universe is constant. However, Antoine Lavoisier described the law of conservation of mass (or the principle of mass/matter conservation) as a fundamental principle of physics in 1789.
Antoine LavoisierA portrait of Antoine Lavoisier, the scientist credited with the discovery of the law of conservation of mass.
This law states that, despite chemical reactions or physical transformations, mass is conserved — that is, it cannot be created or destroyed — within an isolated system. In other words, in a chemical reaction, the mass of the products will always be equal to the mass of the reactants.
The Law of Conservation of Mass-Energy
This law was later amended by Einstein in the law of conservation of mass-energy, which describes the fact that the total mass and energy in a system remain constant. This amendment incorporates the fact that mass and energy can be converted from one to another. However, the law of conservation of mass remains a useful concept in chemistry, since the energy produced or consumed in a typical chemical reaction accounts for a minute amount of mass.
We can therefore visualize chemical reactions as the rearrangement of atoms and bonds, while the number of atoms involved in a reaction remains unchanged. This assumption allows us to represent a chemical reaction as a balanced equation, in which the number of moles of any element involved is the same on both sides of the equation. An additional useful application of this law is the determination of the masses of gaseous reactants and products. If the sums of the solid or liquid reactants and products are known, any remaining mass can be assigned to gas.
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Precipitation - What makes clouds, rain, snow, hail and sleet. When warm, wet air rises, it cools, and water vapor condenses out to form clouds. A cloud is made up of small drops of water or ice crystals, depending on its height and how cold is the surrounding air.
