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grigory [225]
3 years ago
5

Infrared (IR) and Nuclear Magnetic Resonance (NMR) are two spectroscopic techniques you've encountered in organic chemistry I, C

HM2210. In organic chemistry laboratory, IR and NMR are common tools used to characterize a given product. Consider what you learned in CHM22110, and select the concepts that you feel confident about: Group of answer choices Assigning 1H NMR signals to a given molecule The theory behind NMR Identify splitting patterns I do not recall/understand much about NMR correlate the intensity of a 1H NMR signal to the number of protons The theory behind IR I do not recall/understand much about IR Assigning 13C NMR signals to a given molecule Identify functional groups based on IR absorptions Understanding (de)sheilding Deduce the structure of an unknown given its molecular formula, IR and NMR spectra
Chemistry
1 answer:
zalisa [80]3 years ago
8 0

Answer:

The solution to this question can be defined as follows:

Explanation:

Please find the attached file for the solution:

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I NEED HELP PLEASE, THANKS! :)
EleoNora [17]

Answer:

\large \boxed{\text{2.20 g Pb}}

Explanation:

They gave us the masses of two reactants and asked us to determine the mass of the product.

This looks like a limiting reactant problem.

1. Assemble the information

We will need a chemical equation with masses and molar masses, so, let's gather all the information in one place.

Mᵣ:       239.27   32.00        207.2

            2PbS   +   3O₂   ⟶  2Pb   +   2SO₃

m/g:      2.54        1.88

2. Calculate the moles of each reactant

\text{Moles of PbS} = \text{2.54 g PbS } \times \dfrac{\text{1 mol PbS}}{\text{239.27 g PbS}} = \text{0.010 62 mol PbS}\\\\\text{Moles of O}_{2} = \text{1.88 g O}_{2} \times \dfrac{\text{1 mol O}_{2}}{\text{32.00 g O}_{2}} = \text{0.058 75 mol O}_{2}

3. Calculate the moles of Pb from each reactant

\textbf{From PbS:}\\\text{Moles of Pb} =  \text{0.010 62 mol PbS} \times \dfrac{\text{2 mol Pb}}{\text{2 mol PbS}} = \text{0.010 62 mol Pb}\\\\\textbf{From O}_{2}:\\\text{Moles of Pb} =\text{0.058 75 mol O}_{2} \times \dfrac{\text{2 mol Pb}}{\text{3 mol O}_{2}}= \text{0.039 17 mol  Pb}\\\\\text{PbS is the $\textbf{limiting reactant}$ because it gives fewer moles of Pb}

4. Calculate the mass of Pb

\text{ Mass of Pb} = \text{0.010 62 mol Pb} \times \dfrac{\text{207.2 g Pb}}{\text{1 mol Pb}} = \textbf{2.20 g Pb}\\\\\text{The reaction produces $\large \boxed{\textbf{2.20 g Pb}}$}

4 0
2 years ago
When an atom of calcium (Ca) forms an ion by losing two electrons, what is the ion’s type and charge?
posledela

Answer:

cation +2

Explanation:

A cation is a positively charged ion, while an anion is a negatively charged ion. Contrary to how it sounds, when an atom loses electrons, it's charge becomes more positive. Since the calcium atom lost 2 electrons, it is a positive (+2) ion.

5 0
3 years ago
Read 2 more answers
If high tide occurs at 6:00 am, when will the next high tide occur?
Zepler [3.9K]
High tides occur 12 hours and 2 minutes apart do it would be at 6:25 pm
8 0
2 years ago
Read 2 more answers
Can someone help me
Veseljchak [2.6K]

Answer:

Is it D?

Explanation:

3 0
3 years ago
What is the Law of conservation of mass? If one was given the mass of all the products, would it be possible to find the missing
DaniilM [7]
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.
5 0
3 years ago
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