how was rutherfords gold foil experiment inconsistent with the plum pudding model of the atom

The condensation (dehydrated) product rather than the aldol addition (hydrated) product obtained in this experiment is due to the greater stability of the condensation product.

The aldehyde is dehydrated in the aldol condensation process to produce the β-hydroxyaldehyde which then eliminates a water molecule to form an α,β-unsaturated aldehyde or ketone. The condensation product is obtained rather than the aldol addition product in this experiment due to the greater stability of the condensation product. The condensation product is exceptionally stable due because the resonance stabilization. In the condensation product, the carbonyl group in the β position is connected to the α-carbon through a double bond. The carbon-carbon double bond is delocalized over the two carbon atoms in the compound, and this contributes to the overall stability of the compound.

Chelation effect, the carbonyl group in the β position is also involved in chelation with the metal ion. As a result, the overall stability of the compound is increased. Elimination of the water molecule: In the aldol reaction, the product of the reaction has a water molecule in it. This water molecule is eliminated during the condensation reaction, which leads to an increase in the stability of the compound.

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The substance that gives photochemical smog its brownish color is Nitrogen dioxide.

Nitrogen dioxide (NO2) is a reddish-brown irritating gas that is a prominent air pollutant. In the atmosphere, NO2 can be converted into an acid, which is one of the main components of acid deposition, when it combines with water, oxygen, and other chemicals. Nitrogen dioxide is one of the primary pollutants in urban areas.

When NO2 and other chemicals in the atmosphere come into contact with sunlight, they produce photochemical smog, which is a type of air pollution that appears as a brownish haze.

Nitrogen dioxide is formed when nitrogen oxides (NOx) react with sunlight and other atmospheric compounds. Nitrogen oxides are produced by a variety of natural and human activities. For example, NOx can be produced by vehicle exhaust, power plants, and other industrial sources.

Nitrogen dioxide has a wide range of negative health and environmental consequences. NO2 is also one of the primary constituents of acid rain, which is a type of precipitation that is acidic.

Acid rain has a significant impact on the environment and human health. When it falls to the ground, it can cause damage to plants, animals, and ecosystems. Acid rain can also cause respiratory problems in humans and other animals.

In conclusion, nitrogen dioxide is a reddish-brown irritating gas that is a significant air pollutant. Nitrogen dioxide, along with other pollutants, contributes to the formation of photochemical smog and acid rain, both of which have significant health and environmental consequences.

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meat cooking is a chemical change

Heating a meat changes its colour to brownish due to Maillard reaction

Explanation:

The heat of fusion given has units of  kJ / MOL

  so we need to find the number of moles in 70 . 0 g

    using periodic table,    mole wt for AU =196.97 g/mol

     then 70 g   is   70 g / 196.97 g/mol = .355 mole

Now to MELT the gold     .355 mole * 12.5 kJ/mol = 4.44 kJ  ( = 4440 J)

Then to HEAT the liquid to 1213 degrees C from the melting point :

  70 g  * (1213 - 1063) C * .129 J / (g C) = 1355 J

Then add together   4.44kJ  + 1355 J = 4440 J + 1355 J = 5795 J

There are approximately 11.78 grams of oxygen gas (O2) in 8.25 L at STP.

To calculate the number of grams of oxygen gas (O2) in 8.25 L, we need to use the ideal gas law which states:

PV = nRT

Where;

Assuming standard temperature and pressure (STP) conditions (0°C and 1 atm), we can use the molar volume of a gas at STP, which is 22.4 L/mol, to calculate the number of moles of oxygen gas in 8.25 L:

n = (V / V_m) = (8.25 L) / (22.4 L/mol) = 0.3683 mol

The molar mass of O2 is approximately 32 g/mol, so we can calculate the number of grams of oxygen gas in 0.3683 mol:

mass = n x molar mass = 0.3683 mol x 32 g/mol = 11.78 g

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Radiation is the mechanism of heat transfer that does not need any medium. Hence, option C is correct.

Radiation is generally defined as the energy that comes from a source and travels through the space at the speed of light. This type of energy has an electric field and a magnetic field which is associated with it, and has wave-like properties. We can also call radiation as “electromagnetic waves”.

Generally, radiation is defined as the transfer of heat through electromagnetic waves through space. Unlike convection or conduction, in which energy produced from gases, liquids, and solids is transferred by the molecules with or without their physical movement, radiation does not need any medium (molecules or atoms). Hence, option C is correct.

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The fulminate ion has the chemical formula CNO-, and its Lewis structure can be drawn as follows:

Place the carbon atom in the center since it is the least electronegative atom among C, N, and O.

Connect the carbon atom to the nitrogen atom with a triple bond, as nitrogen is more electronegative than carbon.

Connect the nitrogen atom to the oxygen atom with a single bond since oxygen is more electronegative than nitrogen.

Add a lone pair of electrons to the oxygen atom to satisfy its octet.

Place a negative charge on the oxygen atom since it has gained an extra electron.

The Lewis structure with all atoms and bonds is as follows:

markdown

     O

     ||

C ≡ N -

     ||

     H

All atoms except for the nitrogen atom have a formal charge of 0. The nitrogen atom has a formal charge of +1 because it has four valence electrons but only three bonding electrons. The oxygen atom has a formal charge of -1 because it has six valence electrons but seven electrons around it.

The Lewis structure can also be represented by showing the possible resonance forms:

makefile

 O         O

 ||        ||

C = N  ↔  C ≡ N

 ||        ||

 H         H

In this case, the double bond is delocalized between the carbon and nitrogen atoms, and both resonance structures contribute to the overall electronic structure of the fulminate ion.

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Among the given options, the element that requires the most energy to lose one electron is option B) Ca2+.

This is because, in Ca2+, the electron is removed from an inner shell, which requires more energy than removing an electron from the outer shell. The outermost electron shell of Ca2+ is already filled with electrons, so the next electron is in an inner shell, which is tightly bound to the nucleus. Therefore, it requires more energy to remove this electron than it does to remove an electron from an outer shell.

The other options listed are:

A) Li: Lithium has a single electron in its outer shell, so it is relatively easy to remove an electron from it.

C) Si2+: Silicon has four electrons in its outer shell, so it requires less energy than Ca2+ to remove one electron.

D) P: Phosphorus has five electrons in its outer shell, so it requires less energy than Ca2+ to remove one electron.

E) Na: Sodium has a single electron in its outer shell, so it requires less energy than Ca2+ to remove one electron.

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In a neutralization reaction, the acid reacts with the base and produces salt and water. The point where the acid and base are present in stoichiometric proportions is known as the equivalence point. To find the molarity of H2SO4, we first need to consider the balanced chemical equation for the reaction between H2SO4 and KOH:

H2SO4 + 2KOH → K2SO4 + 2H2O

From this equation, we can see that 1 mole of H2SO4 reacts with 2 moles of KOH. Now, we can use the information given to calculate the moles of KOH:

moles of KOH = molarity × volume
moles of KOH = 0.540 M × 58.5 mL × (1 L / 1000 mL) = 0.03159 moles

Since 1 mole of H2SO4 reacts with 2 moles of KOH, we can find the moles of H2SO4:

moles of H2SO4 = 0.03159 moles KOH × (1 mole H2SO4 / 2 moles KOH) = 0.015795 moles

Now, we can find the molarity of H2SO4:

molarity of H2SO4 = moles of H2SO4 / volume of H2SO4
molarity of H2SO4 = 0.015795 moles / (25.00 mL × 1 L / 1000 mL) = 0.6318 M

So, the molarity of H2SO4 is approximately 0.632 M (option b).

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Approximately 402.27 grams of sodium azide (NaN₃) must decompose to fill a 55.0-gallon airbag.

The ideal gas law is a fundamental equation that describes the behavior of ideal gases under a wide range of conditions. It relates the pressure (P), volume (V), temperature (T), and number of moles of gas (n) of an ideal gas through the equation:

PV = nRT

where R is the gas constant, which has a value of 8.314 J/(mol·K) or 0.0821 L·atm/(mol·K) in SI units.

We know that the volume of the airbag is 55.0 gallons, so we need to convert this to liters using a conversion factor.

1 gallon = 3.78541 liters

Therefore, the volume of the airbag in liters is:

55.0 gallons x 3.78541 liters/gallon = 208.20 liters

Next, we need to calculate the number of moles of N₂ gas that would be produced from the decomposition of NaN₃ required to fill the airbag.

From the balanced equation:

2 NaN₃ (s) -> 2 Na (s) + 3 N₂ (g)

We can observe that two moles of NaN₃ result in three moles of N₂. Therefore, the number of moles of N2 produced is:

moles of N2 = (2/3) x moles of NaN₃

To fill the airbag, we need enough N₂ gas to occupy a volume of 208.20 liters. One mole of any gas has a volume of 22.4 litres at standard temperature and pressure (STP).

Therefore, the number of moles of N₂ required is:

moles of N₂ = (208.20/22.4) = 9.29 moles

Now we can use the balanced equation to calculate the number of moles of NaN₃ required:

2 NaN₃ (s) -> 2 Na (s) + 3 N2 (g)

For every 3 moles of N₂ produced, we need 2 moles of NaN3. Therefore, the number of moles of NaN₃ required is:

moles of NaN₃ = (2/3) x moles of N₂ = (2/3) x 9.29 = 6.19 moles

Finally, we can use the molar mass of NaN₃ to calculate the mass required:

mass of NaN₃ = moles of NaN₃ x molar mass of NaN₃

The molar mass of NaN₃ is:

Molar mass of NaN₃ = (1 x 22.99) + (3 x 14.01) = 65.01 g/mol

Therefore, the mass of NaN₃ required to fill the airbag is:

mass of NaN₃ = 6.19 moles x 65.01 g/mol = 402.27 grams

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The restricting reactant is the reactant that is totally consumed in the reaction, thereby restricting how much item that can be shaped. To decide the restricting reactant, we want to look at how much every reactant present to the stoichiometric ratio of the reasonable chemical equation.

In this case, the decent chemical equation is:

2Al(s) + 3Cu(NO3)2(aq) → 3Cu(s) + 2Al(NO3)3(aq)

From the equation, we can see that the stoichiometric ratio of aluminum to copper(II) nitrate is 2:3. This means that for each 2 moles of aluminum, we want 3 moles of copper(II) nitrate to totally respond.

Based on the given information, aluminum is the restricting reactant because it is totally consumed in the reaction, while copper(II) nitrate remains in the solution. This is indicated by the colorless solution of aluminum nitrate shaped, which indicates that all of the copper(II) nitrate has responded with aluminum to frame copper metal and aluminum nitrate.

Therefore, the right answer is Aluminum, because it was totally consumed in the reaction.

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In a titration of a weak acid with a strong base, the concentration of the weak acid and its conjugate base are approximately equal at the halfway point of the titration, also known as the half-equivalence point.

At the beginning of the titration, the solution contains only the weak acid and its concentration is high. As the strong base is added, it reacts with the weak acid to form its conjugate base and water. The concentration of the weak acid gradually decreases while the concentration of the conjugate base increases until it reaches the halfway point.

At the halfway point, half of the weak acid has been neutralized by the strong base, and half remains in the solution. At this point, the concentrations of the weak acid and its conjugate base are approximately equal, and the pH of the solution is equal to the pKa of the weak acid. After the half-equivalence point, the concentration of the conjugate base becomes higher than the concentration of the weak acid, and the pH of the solution starts to rise more rapidly.

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A small fish eats part of a plate and then is eaten by a larger fish. The large fish is eaten by a shark. The situation described is an example of a food chain in an ecosystem.

The small fish is a primary consumer, which eats part of a plate. The larger fish is a secondary consumer, which eats the small fish. The shark is a tertiary consumer, which eats the larger fish.

This sequence of events is an example of how energy and matter flow through an ecosystem. The energy from the sun is captured by producers, such as plants, and then passed on to primary consumers, which are eaten by secondary consumers, and so on.

This transfer of energy and matter is known as a food chain or a food web, and it is an important concept in ecology.

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Answer: it’s all weak like me :(

Explanation:

The concentration of hydrogen ions (H+) and hydroxide ions in a solution determines its pH. (OH-). Svante Arrhenius, a Swedish scientist, proposed the Arrhenius model of acids and bases in 1884.

The pH that an acid will create in solution will decrease the stronger the acid is. The negative logarithm of the concentration of hydronium ions is used to determine pH.

The Arrhenius theory states that an acid is a chemical that releases an H+ ion when dissolved in water. It raises the amount of H+ ions present in the solution. A chemical that ionises the OH- ion is the base.

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When a proton is removed from the -OH group, the remaining oxygen ion can act as a nucleophile and attack the adjacent carbon atom, forming a cyclic ether. The rate at which this reaction occurs depends on the stability of the intermediate carbocation that is formed during the reaction.

In general, the stability of a carbocation depends on the number of alkyl groups attached to the positively charged carbon atom. More alkyl groups increase the stability of the carbocation, making the reaction more favorable and rapid.

Thus, in the pair of compounds, the one with more alkyl groups attached to the carbon atom adjacent to the -OH group would form a cyclic ether more rapidly. For example, in the pair of compounds 2-methyl-1-butanol and 1-butanol, 2-methyl-1-butanol would form a cyclic ether more rapidly as the intermediate carbocation formed during the reaction is more stable due to the presence of an additional methyl group.

Similarly, in the pair of compounds 2-methyl-2-butanol and 2-butanol, 2-methyl-2-butanol would form a cyclic ether more rapidly due to the presence of two methyl groups attached to the adjacent carbon atom, which increases the stability of the intermediate carbocation formed during the reaction.

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a. the number of moles of carbon monoxide is  39.21875 mol CO

b. the pressure of CO in a 1.00 L container at 5000°C is 178,426 atm.

c. the volume occupied by 39.21875 moles of CO at standard pressure (101.3 kPa) and 5000°C is 17,706 L.

The given chemical equation is incorrect as it shows the production of carbon monoxide (CO) which is not produced in the reaction of TNT. The correct equation for the decomposition of TNT is:

2 C7H5N3O6 -> 3 N2 + 5 H2O + 7 CO

a. Calculate the number of moles of carbon monoxide produced if 2550 grams of TNT decomposes according to the equation above.

Molar mass of TNT = (2 x 12.01) + (7 x 1.01) + (3 x 14.01) + (6 x 16.00) = 227.13 g/mol

Number of moles of TNT = 2550 g / 227.13 g/mol = 11.225 mol

From the balanced equation, 7 moles of CO are produced for every 2 moles of TNT. Therefore, the number of moles of CO produced will be:

11.225 mol TNT x (7 mol CO / 2 mol TNT) = 39.21875 mol CO

b. In a 1.00 L container, what would be the pressure of this many moles of CO at 5000°C?

We can use the Ideal Gas Law to determine the pressure of CO at 5000°C:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.

Since the volume is given as 1.00 L, we can convert the temperature to Kelvin:

5000°C + 273.15 = 5273.15 K

The gas constant is R = 0.08206 L•atm/(mol•K).

Substituting the values into the Ideal Gas Law and solving for P:

P = nRT/V = (39.21875 mol)(0.08206 L•atm/(mol•K))(5273.15 K)/1.00 L = 178,426 atm

Therefore, the pressure of CO in a 1.00 L container at 5000°C is 178,426 atm.

c. What volume would be occupied by this number of moles at standard pressure (101.3 kPa) and 5000°C?

To determine the volume occupied by 39.21875 moles of CO at standard pressure and 5000°C, we can use the Ideal Gas Law again, but this time with the pressure and temperature given in standard units:

P = 101.3 kPa = 1.00 atm

T = 5000°C + 273.15 = 5273.15 K

Substituting these values and solving for V:

V = nRT/P = (39.21875 mol)(0.08206 L•atm/(mol•K))(5273.15 K)/(1.00 atm) = 17,706 L

Therefore, the volume occupied by 39.21875 moles of CO at standard pressure (101.3 kPa) and 5000°C is 17,706 L.

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Since the molar mass of the unknown gas is less than that of nitrogen or carbon dioxide, it is likely a lighter gas such as helium (He) or hydrogen (H₂).

Effusion rate of a gas is inversely proportional to the square root of its molar mass and therefore, we use Graham's law of effusion to determine the molar mass of unknown gas.

Let molar mass of CO be M₁ and molar mass of the unknown gas be M₂.

According to Graham's law of effusion: (rate of CO) / (rate of unknown gas) = √(M₂ / M₁)

So, (30.50 / 32.60) = √(M₂ / M₁)

(30.50 / 32.60)² = M₂ / M₁

M₂ = M₁ * (30.50 / 32.60)²

= 28 * (30.50 / 32.60)²

M2 = 25.4 g/mol

Therefore,  molar mass of the unknown gas is approximately 25.4 g/mol. Molar mass of nitrogen (N₂) is approximately 28 g/mol, and molar mass of carbon dioxide (CO₂) is approximately 44 g/mol. Since the molar mass of the unknown gas is less than that of nitrogen or carbon dioxide, it is likely a lighter gas such as helium (He) or hydrogen (H₂).

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Answer:

The mass of lithium hypochlorite are 34.7 grams.

Explanation:

Moles of = 0.594 g. Molar mass of = 58.4 g/mol.

NqrB and NqrC are the two subunits of Na-NQR which can be separated by gel filtration but not by ion exchange chromatography.

The sodium-dependent NADH-quinone oxidoreductase (Na-NQR) is a membrane-bound enzyme complex found in bacteria that participates in the electron transport chain. It consists of six subunits: NqrA, NqrB, NqrC, NqrD, NqrE, and NqrF.

we need to consider the properties of the subunits and the mechanisms of the separation techniques. Gel filtration separates molecules based on their size, while ion exchange chromatography separates molecules based on their charge.

Based on this information, we can infer that the two subunits that can be separated by gel filtration but not by ion exchange chromatography are those that have similar sizes but different charges. Among the six subunits of Na-NQR, NqrB and NqrC are the two subunits that have similar molecular weights (~45 kDa) but different charges.

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In glycolysis, ATP is consumed in the reaction producing fructose-1,6-bisphosphate, which is a crucial intermediate in the pathway and is required for the further breakdown of glucose to pyruvate. The correct answer is option: B.

Glycolysis is the process by which glucose is broken down into two molecules of pyruvate, which is a key step in cellular respiration. The process occurs in ten steps and involves the conversion of glucose to two molecules of pyruvate, with the concomitant production of ATP and NADH . During the third step of glycolysis, the enzyme phosphofructokinase catalyzes the conversion of fructose-6-phosphate to fructose-1,6-bisphosphate, consuming one molecule of ATP in the process. Option: B is correct.

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The solution has a molality of 1.921 mol/kg.

The number of moles of solute dissolved in one kilogram of solvent is known as the molality, which serves as a measurement of a solution's concentration.

We must first count the moles of calcium chloride (CaCl₂) present in the solution. CaCl₂ has a molar mass of 111 g/mol.

Number of moles of CaCl₂ = 96 g / 111 g/mol = 0.8649 mol.

The kilogram mass of the solvent (water) must then be calculated. The density of water, 1 g/mL, allows us to translate the amount of water provided in milliliters (mL) to kilograms (kg).

 Mass of water = 450 mL x 1 g/mL = 450 g = 0.45 kg

We can now determine the solution's molality:

Molality = moles of solute / mass of solvent in kg

Molality = 0.8649 mol / 0.45 kg = 1.921 mol/kg

As a result, the solution has a molality of 1.921 mol/kg.

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3.33 grams of magnesium were utilized, and the same amount of magnesium chloride was generated.

One mole of magnesium interacts with two moles of hydrochloric acid to form one mole of magnesium chloride and one mole of hydrogen gas, as shown by the equation.

mass / molar mass equals moles of HCl.

The formula for HCl is 10.0 g/36.46 g/mol (molar mass of HCl)

HCl equals 0.274 moles per unit.

Mg = 0.274 moles and 2 moles of Mg are equal to 0.137 moles.

When 0.137 moles of HCl are added, the mass of magnesium needed is:

Mg mass is calculated as Mg moles times Mg molar mass.

Mg's mass is 3.33 g.

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When filling a burette for a titration, adjust the burette so that the tip is located slightly below the level of the meniscus, preferably over a sink. Then, use a funnel to add the titrant into the burette. The titrant should be filled above the 0.00 mL line.

A burette is a laboratory equipment that is used to dispense known volumes of liquid in experimental procedures. It is usually made of glass and has a long, cylindrical shape with a stopcock at the bottom to control the flow of liquid.

Burettes are commonly used in titration experiments to accurately measure the volume of the titrant added to the sample. Adjust the burette so that the tip is located slightly below the level of the meniscus, preferably over a sink. This is to prevent the loss of any of the titrant that may overflow. Using a funnel, carefully add the titrant into the burette. Make sure to pour the titrant slowly to avoid splashing or spilling any of it. The titrant should be filled above the 0.00 mL line.

This allows the initial volume of the titrant to be measured accurately before titration commences. If there are air bubbles present, they should be removed by gently tapping the burette.

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The mole fraction of salt in a solution of saltwater with a molality of 3.24 m is 0.764.

Molality is a measure of concentration used in chemistry. Molality is a measure of the amount of solute dissolved in a certain quantity of solvent, usually measured in moles per kilogram. Mole fraction is a measure of the amount of solute present in a solution. The mole fraction of a component in a solution is given by the number of moles of that component divided by the total number of moles of all the components present in the solution.

Mole fraction can be calculated using the following formula:

Xsolute = nsolute / ntotal

where, Xsolute = mole fraction of the solute, n solute = number of moles of the solute, n total = total number of moles of all the components in the solution

Given that the molality of saltwater is 3.24 m. This means that 3.24 moles of salt are present in 1 kg of water. Therefore, the total number of moles of all the components present in the solution is:

n total = 3.24 + 1.00 = 4.24 moles. The mole fraction of salt in the solution is given by:

nsolute / ntotal = 3.24 / 4.24 = 0.764

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0.500 moles of N₂O₅ contain roughly 3.011 x 10²³ molecules.

To determine the number of molecules in 0.500 moles of N₂O₅, we first need to know the Avogadro's number, which is 6.022 x 10²³ molecules per mole.

We can use this conversion factor to calculate the number of molecules as follows:

Number of molecules = (0.500 moles N₂O₅) x (6.022 x 10²³ molecules per mole)

Number of molecules = 3.011 x 10²³ molecules

Therefore, there are approximately 3.011 x 10²³ molecules in 0.500 moles of N₂O₅.

This calculation is useful in various applications, such as in chemical reactions, where it is important to know the number of reactant molecules present in a given amount of substance.

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We must utilize Avogadro's constant to compute the number of molecules in 0.500 mole of N2O5. The number of particles in a material and its mass are related by the proportionality constant known as Avogadro's constant.

The number of particles per mole that make up Avogadro's constant is 6.022 x 1023. We must multiply the number of moles by Avogadro's constant to determine the number of molecules in 0.500 moles of N2O5: = 0.500 mole x 6.022 x 1023 molecules/mole = number of molecules 3.011 x 1023 molecules are the total number. As a result, one mole of N2O5 contains around 3.011 x 1023 molecules. It is crucial to remember that the quantity of a material, measured in moles, is proportional to the number of molecules in a sample. constant allows us to convert between the number of molecules and the amount of substance in a sample.

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The repeat unit of the addition polymer that can be formed from Pent-4-enoic acid is shown below:

      H    H

      |      |

H₂- C = C-C(CH₂)₂COOH

       |     |

      H    H

Since polymer molecules are much larger than most other molecules, the concept of a repeat unit is used when drawing a displayed formula.

When creating one, change the monomer's double bond to a single bond in the repeat unit, and add a bond to each end of the repeat unit. At the end, put the letter n in subscript after the brackets (n represents a very large number of the repeating unit)

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2.50 g of the molecule has 0.135 moles of nitrogen. Atomic number 7 and the letter N both identify nitrogen as a chemical element.

A compound must have another element or components to make up the remaining 24.0% of its mass if it contains 76.0% nitrogen by mass.

Calculating the mass of nitrogen in 2.50 g of the molecule is necessary before determining how many moles of nitrogen are present there:

Nitrogen mass is equal to 76.0% x 2.50 g, or 1.90 g.

Then, we can translate the mass of nitrogen into moles using its molar mass:

1 mol N equals 14.01 g N.

N in moles per 2.50 g is calculated as 1.90 g / 14.01 g/mol = 0.135 mol.

Consequently, 2.50 g of the molecule has 0.135 moles of nitrogen.

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Answer:

0.56 mi/hr

Explanation:

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