Why can't an atom's electrons ever be located between orbits?

1.28atm

According to Boyle's law

P1V1 = P2V2

where

P is the pressure

V is the volume

Given the following

P1 = 2atm

V1 = 3.2L

V2 = 5L

Required

Final pressure P2

Substitute

P2 = P1V1/V2

P2 = 2*3.2/5

P2 = 6.4/5

P2 = 1.28atm

Hence the pressure in atm of the expanded gas sample

The answer is "a mix of alveolar air and dead space air."

Expired air has a greater oxygen content than alveolar air because it is a mix of alveolar air and dead space air.

Expired air is the air that is breathed out after breathing in oxygen.

Alveolar air, on the other hand, is the air that is in the lungs, specifically in the alveoli.

Dead space air is the air that is not involved in gas exchange, or the air that is in the trachea, bronchi, and bronchioles that does not reach the alveoli.

The answer is "a mix of alveolar air and dead space air."

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Answer:

variable

Explanation:

The approximate molar concentration of Na+ ions can be determined by considering the concentration of a sodium-containing compound or the concentration of Na+ in a solution is 1M

The molar concentration of Na+ ions can vary depending on the context. If you have a specific sodium-containing compound, you can determine the molar concentration of Na+ ions by considering its formula and the stoichiometry of the compound. For example, if you have a 1 M solution of sodium chloride (NaCl), the molar concentration of Na+ ions would be 1 M.

In a more general sense, if you have a solution containing sodium ions (Na+), you can determine the approximate molar concentration of Na+ ions by measuring the concentration of a sodium-containing compound or using analytical techniques such as ion-selective electrodes or spectrophotometry.

It's important to note that the molar concentration of Na+ ions can vary depending on the specific solution or compound being considered. Therefore, it is necessary to specify the particular context or compound to obtain a more accurate determination of the molar concentration of Na+ ions.

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The Complete question is

what is the approximate molar concetrations of Na ions in NaCl?

Answer:

maybe, but id rather do automotive stuff, thats my second option.

Explanation:

The number of moles of NaHC2H3O2 produced is 15.90 mol. In conclusion, 15.90 moles of NaHC2H3O2 will be produced in the given chemical reaction.

The balanced equation given is,Na2CO3 + Ca(HC2H3O2)2 → 2NaHC2H3O2 + CaCO3The limiting reagent is Ca(HC2H3O2)2

.Number of moles of Na2CO3 given = 7.95 molesNumber of moles of Ca(HC2H3O2)2 given = 9.20 molesMoles of NaHC2H3O2 produced = ?Molar ratio of Ca(HC2H3O2)2 and NaHC2H3O2 is 1:2

Number of moles of NaHC2H3O2 produced can be calculated as follows:Step 1Number of moles of Ca(HC2H3O2)2 needed to react with Na2CO3 can be calculated as follows

:Na2CO3 + Ca(HC2H3O2)2 → 2NaHC2H3O2 + CaCO3Number of moles of Ca(HC2H3O2)2 = 7.95 moles Na2CO3 × 1 mol Ca(HC2H3O2)2/1 mol Na2CO3= 7.95 moles

Step 2To calculate the number of moles of NaHC2H3O2 produced, use the mole ratio between Ca(HC2H3O2)2 and NaHC2H3O2Number of moles of NaHC2H3O2 = 7.95 mol Ca(HC2H3O2)2 × 2 mol NaHC2H3O2/1 mol Ca(HC2H3O2)2= 15.90 mol NaHC2H3O2

Therefore, 15.90 moles of NaHC2H3O2 will be produced.

The given balanced chemical equation is Na2CO3 + Ca(HC2H3O2)2 → 2NaHC2H3O2 + CaCO3. The limiting reagent is Ca(HC2H3O2)2. We are given 7.95 moles of Na2CO3 and 9.20 moles of Ca(HC2H3O2)2.

To find the moles of NaHC2H3O2 produced, we need to first find the number of moles of Ca(HC2H3O2)2. Then, we can use the mole ratio between Ca(HC2H3O2)2 and NaHC2H3O2 to find the number of moles of NaHC2H3O2 produced.

The number of moles of NaHC2H3O2 produced is 15.90 mol. In conclusion, 15.90 moles of NaHC2H3O2 will be produced in the given chemical reaction.

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Answer: The rate at which a vibration occurs that constitutes a wave, either in a material (as in sound waves), or in an electromagnetic field (as in radio waves and light), usually measured per second. Also it is measured in Hertz.

Explanation:

Answer frequency is the number of occurrences of a repeating event per unit of time. Frequency is measured in Hertz. Unit frequency is measured as the number of wave cycles that occur in one second.

The unit of frequency measurement is hertz

Explanation:

Answer:

they are more likely to get sick from the same disease

Black-footed ferrets are the most endangered mammal of North America. The problem that most black-footed ferrets today are closely related because they are more likely to get sick from the same diseases.

An endangered species are the species that can become extinct in the future, either worldwide.

The problem of the  black-footed ferrets today are closely related is that they are more likely to get sick from the same diseases.

Thus, the correct option is C.

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Answer: Diisobutylaluminum hydride (DIBALH) is a reducing agent that can reduce esters to aldehydes or 2' alcohols to ketones. Therefore, the correct answer is (A) ester to aldehyde and (C) 2' alcohol to ketone.

DIBALH is not capable of converting carboxylic acid to ester or ester to a carboxylic acid, nor can it oxidize an aldehyde to a carboxylic acid.

Explanation: Diisobutylaluminum hydride (DIBALH) is a reducing agent that can reduce esters to aldehydes or 2' alcohols to ketones. Therefore, the correct answer is (A) ester to aldehyde and (C) 2' alcohol to ketone.

DIBALH is not capable of converting carboxylic acid to ester or ester to a carboxylic acid, nor can it oxidize an aldehyde to a carboxylic acid.

Answer:

true.................

Answer:

the answer is true hope it helps

Answer:

Explanation:

The balanced chemical equation for the reaction in which water (H2O) is broken down into hydrogen gas (H2) and oxygen gas (O2) is:

2 H2O → 2 H2 + O2

According to the stoichiometry of this equation, for every 2 moles of water that react, 1 mole of oxygen gas is consumed. Therefore, to determine how many moles of oxygen gas were consumed, we need to find how many moles of water reacted.

Since we know that 0.25 moles of water were produced, we can assume that the same number of moles of water reacted, which means that:

0.25 moles H2O reacted

Using the stoichiometry of the balanced equation, we can see that for every 2 moles of water that react, 1 mole of oxygen gas is consumed. Therefore, the number of moles of oxygen gas consumed can be calculated as:

0.25 moles H2O x (1 mole O2 / 2 moles H2O) = 0.125 moles O2

Finally, we can use the ideal gas law, PV = nRT, to calculate the volume of oxygen gas consumed, assuming standard temperature and pressure (STP) of 0°C (273 K) and 1 atmosphere (1 atm):

V = nRT/P

V = (0.125 mol)(0.0821 L·atm/mol·K)(273 K)/(1 atm)

V = 2.7 L

Therefore, 2.7 liters of oxygen gas were consumed in the reaction.The balanced chemical equation for the reaction in which water (H2O) is broken down into hydrogen gas (H2) and oxygen gas (O2) is:

2 H2O → 2 H2 + O2

According to the stoichiometry of this equation, for every 2 moles of water that react, 1 mole of oxygen gas is consumed. Therefore, to determine how many moles of oxygen gas were consumed, we need to find how many moles of water reacted.

Since we know that 0.25 moles of water were produced, we can assume that the same number of moles of water reacted, which means that:

0.25 moles H2O reacted

Using the stoichiometry of the balanced equation, we can see that for every 2 moles of water that react, 1 mole of oxygen gas is consumed. Therefore, the number of moles of oxygen gas consumed can be calculated as:

0.25 moles H2O x (1 mole O2 / 2 moles H2O) = 0.125 moles O2

Finally, we can use the ideal gas law, PV = nRT, to calculate the volume of oxygen gas consumed, assuming standard temperature and pressure (STP) of 0°C (273 K) and 1 atmosphere (1 atm):

V = nRT/P

V = (0.125 mol)(0.0821 L·atm/mol·K)(273 K)/(1 atm)

V = 2.7 L

Therefore, 2.7 liters of oxygen gas were consumed in the reaction.

2.3352 g of PbCl₂ are formed when 50. 0 ml of 0. 336 m KCl react with pb(no3)2.

The balanced equation for the above double displacement reaction is as follows;

2KCl + Pb(NO₃)₂ ---> PbCl₂ + 2KNO₃

Stoichiometry of KCl to PbCl₂ is 2:1

This means that 2 mol of KCl would react with every 1 mol of PbCl₂

The molarity of KCl = 0. 336 M

in 1 L of KCl, there are mol

Therefore in  50. 0 ml of KCl, there are=  \(\frac{0. 336 * 50}{1000}\)

Number of KCl moles reacted = 0.0168 mol

according to stoichiometry

number of PbCl₂ moles formed =  1/2 x number of KCl moles reacted

Therefore number of PbCl₂ moles formed = 0.0168 mol/2 = 0.0084 mol

molar mass of PbCl₂ = 278 g/mol

mass of PbCl₂ formed = 278 g/mol x 0.0084 mol = 2.3352 g

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The graph shows that as mass increases, kinetic energy increases exponentially. This means that as the mass of an object increases, the kinetic energy increases by a larger and larger amount.

This can be seen by the upward sloping line on the graph. This can be seen in the graph by the steepness of the line, which shows that the increase in kinetic energy is growing faster and faster as the mass increases. Additionally, the graph shows that the rate of increase in kinetic energy is greater for lower masses than for higher masses, which indicates an exponential increase. This can be seen by the upward sloping line on the graph.

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When talking about physical properties of matter, a substance could change its state or form, but the substance is not changed into a new substance. In other words, the composition of matter is not changed. Physical properties are used to describe and classify matter. Three examples of physical properties of matter are density, color, and boiling point.

Physical properties of matter are characteristics that can be observed or measured without changing the substance into a new substance. These properties help us describe and classify different types of matter. When a substance undergoes a change in its physical state or form, such as melting, freezing, evaporating, or condensing, its physical properties can change, but the composition of the substance remains the same.

For example, when ice melts into liquid water, the state of the substance changes from solid to liquid, but it is still composed of the same water molecules. Similarly, when a substance changes its color or boiling point, it is still the same substance, just with different observable properties.

Three examples of physical properties of matter are:

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Answer:

50 kJ

Explanation:

Activation energy is the energy to go from reactants at 150  to   200 kJ

 = 50 kJ

As the temperature increases the water vapor concentration also increases. this leads to further warming because as the evaporation rate increases and the water water vapor is greenhouse gas.

When the temperature increases the rate of the evaporation increases and the concentration of the water vapor in the air increases because the water vapor is the greenhouse gas. when the temperature decreases then the water vapor will condense and form liquid.

Thus, As the temperature increases the water vapor concentration also increases. this leads to further warming because as the evaporation rate increases and the  water water vapor is greenhouse gas.

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When a bottle of soda is opened, it undergoes a fascinating phenomenon where carbon dioxide gas (CO2) is released, resulting in the formation of bubbles.

Carbon dioxide is responsible for the carbonation of soda and is typically dissolved in the beverage under high pressure during the bottling process.

The carbon dioxide gas is introduced to the soda under pressure, causing it to dissolve in the water or syrup used to make the drink.

This dissolution forms carbonic acid (H2CO3), which is the chemical compound responsible for giving soda its tangy and bubbly taste.

The high-pressure environment inside the bottle helps retain the gas in the liquid.

However, when the bottle is opened, the pressure inside suddenly drops, leading to the liberation of the dissolved carbon dioxide gas.

As a result, the carbon dioxide bubbles up and escapes from the liquid, creating the fizz and bubbles that we observe when opening a bottle of soda.

This effervescent reaction is a result of the equilibrium between dissolved carbon dioxide and carbonic acid being disturbed by the sudden decrease in pressure.

The released carbon dioxide forms gas bubbles, which rapidly rise to the surface and escape into the surrounding air.

The effervescence and bubbling of soda upon opening is a delightful and refreshing experience that adds to the enjoyment of this popular carbonated beverage.

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Answer:

Huh? I guess it's

Explanation:

Answer:

Benzophenone will show absorption at 1720 cm-1, while benzaldehyde will show absorptions at 1600 and 1650 cm-1. Additionally, benzophenone will show absorption at 1865 cm1 and benzaldehyde will show absorptions at 2820 and 2720 cm1.

These absorption peaks can be used to distinguish between the two compounds using IR spectroscopy.

Benzophenone has a carbonyl group and shows an absorption peak at 1720 cm1, which corresponds to the C=O stretching frequency. Benzaldehyde has an aldehyde group and shows absorption peaks at 1600 and 1650 cm-1, which correspond to the C=C stretching frequency and the C-H bending frequency, respectively.

Additionally, benzophenone has a phenyl ring, which gives a peak at 1865 cm1, and benzaldehyde has a C-H stretching, giving peaks at 2820 and 2720 cm1.

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Actually the main difference:

Homogeneous mixture is a mixture consisting of constituent substances that are mixed evenly.  As a result, each part of the mixture has the same properties

 In contrast to heterogeneous mixtures where the constituent substances are not mixed evenly.  Thus, there are parts of the mixture that have different properties.

Differences between Homogeneous and Heterogeneous Mixtures in detail

1. Differences Between Homogeneous and Heterogeneous Mixtures Based on Their Definitions

Homogeneous is a mixture that is uniform in all its parts and forms a single phase.  An example of a homogeneous mixture is air.  In addition, homogeneous mixtures can also be commonly referred to as solutions.

Meanwhile, heterogeneous mixture is a mixture that is not similar or not uniform, and the formation of two or more phases, as well as the existence of a clear boundary between the phases.  Examples of heterogeneous mixtures include oil and water, a mixture of lime and sand, then a mixture of iron powder and carbon, and many others.

2. Differences Between Homogeneous and Heterogeneous Mixtures Based on Their Characteristics

The characteristics of this homogeneous mixture are in the form of constituent particles that cannot be distinguished from one another, have almost the same color, and have a similar taste.  Not only that, substances that have been mixed have the same ratio, have the same concentration level, and are in the form of solids, gases, and liquids.

And this mixture cannot be separated, if you use a mechanical method, but you can separate it when you use a more difficult method.  The example of such separation is similar to that of distillation.  That is one of the differences between homogeneous and heterogeneous mixtures based on their characteristics.

3. Difference between Homogeneous and Heterogeneous Mixtures Based on Their Properties

The nature of this homogeneous mixture has the property that if every part of a homogeneous mixture is often the same, both in terms of color, taste, and comparison.  An example of the nature of the homogeneous mixture is a spoonful of sugar dissolved in water.

While the nature of a heterogeneous mixture is a mixture of two or more substances, which have properties, the constituent substances are not the same or the alias is not uniform.  So that the two mixed substances can still be distinguished by the particles.

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brittle metal would experience this type of failure

Glass, ceramic, graphite, and some alloys with very low plasticity are examples of brittle materials. In these materials, cracks can start without plastic deformation and quickly progress to brittle breakage. It is a steel-gray, lightweight metal called beryllium. It is also highly brittle, which means that it fractures easily when under stress but does not typically distort before it does so (similar to glass or ceramic). Beryllium is a naturally occurring element found in over 100 different minerals and has a wide range of modern-day applications. Cast iron has a rough feel and is more brittle because it includes 2% to 3.5% carbon. Despite being made of alloyed metals, carbon steel lacks other alloying components, hence despite being an alloy, it is not classified as an alloy.

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Answer:

c

Explanation:

Answer:

Nitrogen is an inert gas — meaning it doesn't chemically react with other gases — and it isn't toxic. But breathing pure nitrogen is deadly. That's because the gas displaces oxygen in the lungs. Unconsciousness can occur within one or two breaths, according to the U.S. Chemical Safety and Hazard Investigation Board.

Answer:

because it is an insert gas and it is very dangerous for ear and our nose

Spill-cleaning materials should never be reused because of the risk of contamination. This indicates that items like absorbents and cleaning supplies need to be stored and packaged for disposal of hazardous waste.

Different cleaning techniques are used depending on the type of soil that was spilled. These are the necessary steps in liquid spill cleanup Surround the area:

1. Once the area has been covered with the absorbent material, cover the whole spill.

2. Put all the material in a plastic bag that has been scooped up and collected.

3. Put every bagged piece of trash into a sturdy trash can and organize it there.

4. It is beneficial to use of soap, water, and cleaning agent to disinfect the region.

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Answer

The freezing point o the solution = 273.714153 K

The boiling point of the solution= 373.1955328 K

Explanation

Given:

Mass of glucose = 5.00 g

Volume of water = 72.8 g

What to find:

The freezing point and the boiling point of the solution.

Step-by-step solution:

Note: (Freezing point of water = 273K, Kf for water =1.87K kg/mol, atomic weight C = 12, H = 1, O = 16).

The freezing point of the solution:

The molecular weight of glucose C6H12O6 = 6(12) + 12(1) + 6(16) = 180 g/mol

The number of moles of glucose = (Mass of glucose/Molecular weight) = 5.00 g/180.0 g/mol = 0.0278 moles

Mass of water = 72.8 g = 0.0728 kg

So molality of glucose = (Moles o glcsose/Volume of solution) = 0.0278 mol/0.0728 kg = 0.3819 mol/kg

The depression in the freezing point, ∆T = Kf x molality = 1.87 K kg/mol x 0.3819 mol/kg = 0.714153 K

Since the freezing point of water = 273 K

Therefore, the freezing point of the solution= 273 K + 0.714153 K = 273.714153K

The boiling point of the solution:

∆T = i x m x Kb

∆T = change in temperature i.e boiling point elevation

i = van't Hoff factor = 1 for glucose since it does not ionize or dissociate. It is a single particle.

m = molality = moles solut/kg solvent = 0.0278 mol/0.0728 kg = 0.3819 mol/kg

Kb = boiling poin constant = 0.512 K kg/mol

∆T = 1 x 0.3819 mol/kg x 0.512 K kg/mol

∆T = 0.1955328 K

Since the freezing point of water = 373 K

Therefore, the boiling point of the solution = 373 K + 0.1955328 K = 373.1955328 K

La(OH)3 precipitates at a pH of approximately 7.21 in this acidic solution when treated with NaOH.

To determine the pH at which La(OH)3 precipitates in an acidic solution containing 0.017 M La3+ treated with NaOH, we can follow these steps:

1. Write the balanced chemical equation for the reaction:
La3+ + 3OH- → La(OH)3 (s)

2. Write the solubility product (Ksp) expression for La(OH)3:
Ksp = [La3+][OH-]^3
Given that Ksp for La(OH)3 is 2×10^-21.

3. Calculate the concentration of OH- ions needed to precipitate La(OH)3:
[OH-] = (Ksp / [La3+])^(1/3)
[OH-] = (2×10^-21 / 0.017)^(1/3)
[OH-] ≈ 1.62×10^-7 M

4. Determine the pOH:
pOH = -log([OH-])
pOH = -log(1.62×10^-7) = -(log 1.62 +(-7*log10)) = -(0.209 +(-7*1)) = -(0.209-7) = -(-6.791) = 6.791
pOH ≈ 6.79

5. Calculate the pH:
pH = 14 - pOH
pH ≈ 14 - 6.79
pH ≈ 7.21

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The Ancient Egyptians used simple sundials and divided days into smaller parts, and it has been suggested that as early as 1,500BC, they divided the interval between sunrise and sunset into 12 parts. ... Known as a clepsydra, it uses a flow of water to measure time.