in the first box draw the necessary arrows to show how the starting material undergoes a bimolecular elimination pathway. in the empty box, draw the major organic product of the reaction.

N and C

Because Lithium and Sodium belong to group 1A whereas Magnesium is from group 2A, which are S block elements and they form ionic bond.

Answer:

N and C

Explanation:

Os the right answer

The total bond energy of the reactants and products must be subtracted to obtain the energy change in the reaction \(2H_2O --- > 2H_2 + O_2\) using the provided bond energy.

Reactants:

2H-O-H (2 molecules) = 2 * (2 * O-H) = 2 * (2 * 463 kJ/mol) = 1852 kJ/mol

Products:

2H-H (2 molecules) = 2 * (2 * H-H) = 2 * (2 * 436 kJ/mol) = 1744 kJ/mol

O=O = 1 * O=O = 1 * 495 kJ/mol = 495 kJ/mol

1852 kJ/mol is the total binding energy of the reactants.

The combined binding energy of the products is 1744 kJ/mol + 495 kJ/mol, which is equal to 2239 kJ/mol.

Energy change (ΔE) = Total bond energy of the products - Total bond energy of the reactants

ΔE = 2239 kJ/mol - 1852 kJ/mol = 387 kJ/mol

So, the answer is E.

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Your question is incomplete, most probably the complete question is:

Calculate the energy change of the following reaction

based on the bond energies given.

2H2O2H2 + O2

H-H: 436kJ/mol

O=0: 495kJ/mol

O-H: 463kJ/mol

Select one:

Answer:

d) The moon s about 1/2 the size of Earth s diameter

Explanation:

The concentration of the solution will be 0.073 M.

To solve this problem, we need to use the concept of stoichiometry and the equation for the reaction given.

The balanced net ionic equation for the reaction is not given in the question, so we cannot provide a numerical answer. Please provide the balanced net ionic equation for the reaction. Once we have that, we can proceed with the calculation.

Assuming the balanced net ionic equation for the reaction is;

A + B → C + D

where A represents the substance in the solution we are trying to determine the concentration of, and B represents the titrant (0.1371 M solution), we can use the following equation to calculate the concentration of A;

M_A = (M_B x V_B) / V_A

where M_A is the concentration of A, M_B is the concentration of the titrant, V_B is the volume of titrant used, and V_A is the volume of the solution.

Substituting the given values into the equation, we get;

M_A = (0.1371 M x 21.24 mL) / 40.00 mL

M_A = 0.073 M

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Answer:

A. carbon

Explanation:

When atoms form chemical bonding then the atoms attain Noble gas configuration.

Noble gas configuration of an atom includes the fundamental image of the ultimate noble fueloline previous to that atom, observed via way of means of the configuration of the ultimate electrons.so for sodium, we make the substitution of [Ne] for the 1s22s22p6 a part of the configuration. Sodium's noble fueloline configuration becomes [Ne]3s1.

Covalent bonds, atoms percentage pairs of electrons, at the same time as in ionic bonds, electrons are absolutely transferred among atoms in order that ions are formed.During the formation of a chemical bond, the predicted end result is that the electrons will whole a noble fueloline configuration in each atoms. Typically, while atoms shape a chemical bond, the predicted end result is that the electrons.

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Explanation:

require an emergency support immediately

Calculate [OH-] and pH with [H+] = 2.9 × 10^-10 M:

Using the equation Kw = [H+][OH-], where Kw is the ion product of water:

Kw = [H+][OH-]

1.0 × 10^-14 = (2.9 × 10^-10)[OH-]

[OH-] = (1.0 × 10^-14) / (2.9 × 10^-10)

[OH-] ≈ 3.45 × 10^-5 M

To calculate the pH, we can use the equation:

pH = -log[H+]

pH = -log(2.9 × 10^-10)

pH ≈ 9.54

THEREFORE, the [OH-] is approximately 3.45 × 10^-5 M, and the pH is approximately 9.54.

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Answer:

C: 4

Explanation:

In every single covalent bond, each atom shares one electron. 1 + 1 = 2. A double bond is just two bonds so, 2 x 2 = 4.

The oxygen content of a water column can be seen to vary with depth in the image what causes oxygen levels to rise at great depths

At the deepest levels, there is frequently an increase in dissolved oxygen below the oxygen minimum layer. Since lower temperatures and higher pressure increase the solubility of dissolved gases, this bottom water is typically colder and under much greater pressure than the surrounding surface water.

What is pressure at depth ?

The relationship between pressure and depth is inversely proportional. This is a result of the larger water column pressing down on an object that is submerged. In contrast, pressure drops as items are raised and the depth is lowered. At sea level, a force of 14.6 pounds is applied to every square inch of your surface. For every 10 meters of sea depth, the pressure rises by approximately one atmosphere. The pressure will be about 500 atmospheres, or 500 times more than the pressure at sea level, at a depth of 5,000 meters.

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The dosage of 26mg can be prepared using approximately 1.625 mL of the 40mg in 2.5 mL solution.

The dosage of 22mg can be prepared using approximately 1.222 mL of the 36mg per 2 mL strength solution.

To calculate the dosage using ratio and proportion, we can set up a proportion based on the strength of the solution.

40mg in 2.5 mL solution will be used to prepare a 26mg dosage.

Let X represent the mL of the solution needed to prepare the 26mg dosage.

We can set up the proportion as follows:

40mg/2.5mL = 26mg/X mL

Cross-multiplying and solving for X, we have:

40mg * X mL = 2.5mL * 26mg

40X = 65

X = 65/40

X ≈ 1.625 mL

For the second question:

36mg per 2 mL strength solution is used to prepare 22mg.

Let Y represent the mL of the solution needed to prepare the 22mg dosage.

We can set up the proportion as follows:

36mg/2mL = 22mg/Y mL

Cross-multiplying and solving for Y, we have:

36mg * Y mL = 2mL * 22mg

36Y = 44

Y = 44/36

Y ≈ 1.222 mL

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Liquids are more compressible than solids.

In liquids there is space between the molecules, not a lot, but there is enough space to offer some compressibility. Solids are arranged in regular patterns and their molecules are almost fixed close together.

Approximately 1.693 grams of calcium will be produced when 4.7 grams of calcium chloride are completely used up in the reaction.

To determine the grams of calcium produced, we need to calculate the molar ratio between calcium chloride (CaCl2) and calcium (Ca) in the balanced chemical equation for the reaction. The balanced equation is:

2Al + 3CaCl2 → 3Ca + 2AlCl3

From the balanced equation, we can see that for every 3 moles of calcium chloride, 3 moles of calcium are produced. We need to convert the given mass of calcium chloride (4.7 grams) to moles using its molar mass.The molar mass of CaCl2 is calculated by adding the atomic masses of calcium (Ca) and chlorine (Cl). The atomic mass of calcium is 40.08 g/mol, and the atomic mass of chlorine is 35.45 g/mol.

Molar mass of CaCl2 = (40.08 g/mol) + 2(35.45 g/mol) = 110.98 g/mol

Now we can calculate the moles of calcium chloride:

Moles of CaCl2 = (mass of CaCl2) / (molar mass of CaCl2)

              = 4.7 g / 110.98 g/mol

              ≈ 0.0423 mol

Since the molar ratio between calcium chloride and calcium is 3:3, the moles of calcium produced will be equal to the moles of calcium chloride used.

Moles of Ca = 0.0423 mol

To convert moles of calcium to grams, we multiply by the molar mass of calcium:

Mass of Ca = (moles of Ca) × (molar mass of Ca)

          = 0.0423 mol × 40.08 g/mol

          ≈ 1.693 g

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ANSWER

The number of moles of Pb(SO4)2 is 1.5 moles

EXPLANATION

Given that;

The mass of Li2SO4 is 330g

Follow the steps below to find the moles of Pb(SO4)2

Step 1; Write the balanced equation of the reaction

Step 2; Find the number of moles of Li2SO4 using the below formula

Recall, that the molar mass of Li2SO4 is 109.94 g/mol

The number of moles of Li2SO4 is 3.00 moles

Step 3; Find the number of moles of Pb(SO4)2 using a stoichiometry ratio

In the above equation of the reaction, 1 mole Pb(SO4)2 reacts to give 2 moles LiSO4

Let the number of moles of Pb(SO4) be x

Therefore, the number of moles of Pb(SO4)2 is 1.5 moles

The Concentration is 0.19 mol/L i.e., also known as molarity which is calculated below.

Step 1: Calculation of molarity

Molarity is  defined to be the number of moles of solute divided by volume of solution in liters

i.e.,    Molarity(M)= number of moles of solute / volume of solution ( in L )

Step 2: Calculate the moles  of KMnO4

Given,

Mass = 5.9 g

Molar mass of KMnO4 = 158.034 g/mol

we know,  moles = mass / molar mass

moles of KMnO4  = 5.9 g / 158.034 g/mol = 0.037334 mol

Step 3: Calculation of molarity

Volume of solution = 200 mL = 0.200 L  

[ because 1 L=1000 mL   so, 200 mL = ( 200 mL  ×  ( 1 L / 1000 mL) = 0.200 L ]

Since we know ,

molarity = moles of solute / volume of solution in L

molarity = 0.037334 mol /0.200 L = 0.19 mol/L        

Hence, the Concentration is 0.19 mol/L    

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Complete question:          

A Chemist Prepares A Solution Of Potassium Permanganate (KMnO4) By Measuring Out 5.9 G Of Potassium Permanganate Into A 200 ML Volumetric Flask And Filling The Flask To The Mark With Water. Calculate The Concentration In Mol/L Of The Chemist's Potassium Permanganate Solution. Round Your Answer To 2 Significant Digits.

According to the research, the correct answer is Option C. A prism splits light up into a frequency spectrum.

It is a medium endowed with transparency that is delimited by flat faces that are not parallel.

In this sense, they are usually made of glass, they are used to make a light break, reflect or refract.

Therefore, we can conclude that according to the research, a prism is a crystal where the light rays that fall on its surface reverse the direction of propagation.

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The Clausius-Clapeyron equation, which links a substance's vapour pressure to its temperature. Therefore, the liquid's heat of vaporisation is roughly 45.56 kJ/mol.

The Clausius-Clapeyron equation, which connects the change in vapour pressure to the change in temperature and the heat of vaporisation, can be used to address this issue: Hvap/R(1/T1 - 1/T2) is equal to ln(P2/P1). When the temperature rises from 22.4°C (295.55 K) to 30.7°C, the liquid's vapour pressure increases by a factor of three (303.85 K). P2/P1 = 3 T1 = 295.55 K T2 = 303.85 K is the result.

The Clausius-Clapeyron equation can be solved for by substituting these values and getting the answer: ln(3) = Hvap/R(1/295.55 - 1/303.85).

ΔHvap = -R(1/295.55 - 1/303.85)

ln(3)

Applying the gas constant R = 8.314 J/(mol K), the following equation is obtained: Hvap = -8.314 J/(mol K) (1/295.55 K - 1/303.85 K) ln (3)

Hvap equals -40.71 J/mol.

We divide this amount by 1000 to get kJ/mol:

ΔHvap = -0.0407kJ/mol

As a result, the liquid's heat of vaporisation is 0.0407 kJ/mol.

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Among the following gases SO₂ will deviate most from the ideal gas behavior. Hence, option A is correct.

A gas deviates the most from its ideal behavior at high pressure and low temperature.

Under high pressure and low temperature conditions, the gas molecules becomes closer to each other and they exert significant amount of intermolecular forces on each other.

Also under these conditions, the volume of the gas molecules becomes a significant portion of the total volume and can not be neglected.

Hence, from the above gases only SO₂ shows this property more under high pressure and low temperature and deviates more from its ideal behavior.

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Approximately 3.04 grams of magnesium would be required to react with 0.25 moles of hydrochloric acid.

To determine the mass of Mg required, we need to use the balanced chemical equation for the reaction between hydrochloric acid (HCl) and magnesium (Mg):

2HCl + Mg → MgCl2 + H2

From the balanced equation, we can see that 2 moles of HCl react with 1 mole of Mg. Therefore, if 0.25 mol of HCl reacts, we would need half of that amount, which is 0.125 mol of Mg.

To calculate the mass of Mg required, we need to multiply the number of moles of Mg by its molar mass. The molar mass of Mg is given as 24.31 g/mol. Therefore, the mass of Mg required can be calculated as follows:

Mass of Mg = Number of moles of Mg × Molar mass of Mg

Mass of Mg = 0.125 mol × 24.31 g/mol

Mass of Mg = 3.04 g

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Answer:

observation

Explanation:

Observation: copper carbonate is a green solid and product CuO is a black solid. Hence, green color disappears, and black color appears. (a) copper nitrate. (b) copper carbonate.

Answer;

Water 1.0 g/mL 100°C colorless liquid

Explanation:

thats the answer

Answer:

ethanol

Explanation:

just did it in study island

Answer:

En el grupo de los no metales se incluyen los halógenos​ (flúor, cloro, bromo, yodo, astato y téneso), que tienen 7 electrones en su última capa de valencia y los gases nobles (helio, neón, argón, kriptón, xenón, radón), que tienen 8 electrones en su última capa (excepto el helio, que tiene 2).

Explanation:

halógenos

Answer:

1,4

Explanation:

Chemical disequilibrium is likely to be present in any system where the forward and reverse reactions are not in balance.

This can occur in a variety of situations, such as when the reactants are not present in the correct proportions, when the reaction conditions are not ideal, or when there are external factors affecting the reaction. For example, in a chemical reaction where one product is constantly being removed from the system, the reaction may never reach equilibrium.

Similarly, in a reaction where the temperature or pressure is constantly changing, the equilibrium may shift in one direction, leading to a chemical disequilibrium. Ultimately, chemical disequilibrium occurs when a reaction is not able to maintain a stable equilibrium state. Chemical disequilibrium is likely to be present in environments where reactions are ongoing and not yet in a stable state. These situations can be found in systems experiencing changes in temperature, pressure, or concentrations of reactants and products. Examples include volcanic areas, hydrothermal vents, or chemical industries where continuous production or consumption of reactants occurs. The presence of chemical disequilibrium provides opportunities for further reactions to take place, leading to new products and potential energy releases. Understanding these environments can offer insights into various natural processes and technological applications.

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Answer:

a.

\([H _{3}O {}^{ + } ] = 4.23 \times {10}^{ - 3} M\)

b.

\([OH {}^{ - } ] = \frac{kw}{[H {}^{ + } ]} \\ [OH {}^{ - } ] = \frac{1 \times {10}^{ - 14} }{4.23 \times {10}^{ - 3} } \\ [OH {}^{ - } ] = 2.36 \times {10}^{ - 12} M\)

c.

\(pH = - log[H {}^{ + } ] \\ pH = - log(4.23 \times {10}^{ - 3} ) \\ pH = 2.37\)

d.

\(pOH = - log[OH {}^{ - } ] \\ = - log(2.36 \times {10}^{ - 12} ) \\ = 11.63\)

Answer:

Where are the answer choices

?

Carbon tetrachloride (CCl4) can be produced when excess chlorine reacts with methane (CH4) in the presence of light. This reaction is a substitution reaction known as chlorination. Here's a step-by-step explanation of how carbon tetrachloride is formed:

In the presence of light, methane (CH4) and chlorine (Cl2) undergo a substitution reaction. One of the chlorine atoms in Cl2 is substituted for a hydrogen atom in CH4, resulting in the formation of chloromethane (CH3Cl) and hydrogen chloride (HCl).

The chloromethane (CH3Cl) formed in the first step continues to react with chlorine (Cl2) in a similar substitution reaction. Another chlorine atom substitutes a hydrogen atom in chloromethane, leading to the formation of dichloromethane (CH2Cl2).

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The heat of combustion of ethane (C2H6) in kilojoules per mole can be determined by subtracting the sum of the enthalpies of formation of the products from the sum of the enthalpies of formation of the reactants.

The enthalpy of formation is the change in enthalpy when one mole of a compound is formed from its constituent elements in their standard states. By referring to the table of thermodynamic properties, the enthalpies of formation for ethane (C2H6), carbon dioxide (CO2), and water (H2O) can be obtained.

The heat of combustion of ethane can be calculated using the following equation:

ΔHcomb = ΣΔHf(products) - ΣΔHf(reactants)

For the combustion of ethane, the reaction equation is:

C2H6 + 3.5O2 → 2CO2 + 3H2O

Using the enthalpies of formation from the table, the heat of combustion of ethane can be calculated.

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