Which step in naming unsaturated hydrocarbons is used for alkenes but not alkynes?

Answer:

yes, 7 is the correct answer.

Answer: 7

Explanation: Just did it.

Answer:

B

Explanation:

Answer:

D.A tree

Explanation:

Answer:

a

Explanation:

Answer:

i am also positive it is A

Explanation:

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Answer:

most acids contain something called   hydrogen atoms

Explanation:

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Human activity affects Earth systems such as the atmosphere, hydrosphere, lithosphere, and biosphere, resulting in consequences such as climate change, soil erosion, and pollution. To reduce environmental impacts, individuals can conserve energy, reduce waste, use public transportation, and support sustainable practices. Governments and industries can also implement policies and technologies to promote sustainability.

Human activity can have significant impacts on Earth systems, including the atmosphere, hydrosphere, lithosphere, and biosphere. For example, the burning of fossil fuels releases greenhouse gases into the atmosphere, contributing to climate change. Deforestation can lead to soil erosion and loss of biodiversity. Pollution from industrial and agricultural activities can contaminate water sources.

To reduce environmental impacts, individuals can take actions such as conserving energy by using energy-efficient appliances, reducing waste by recycling and composting, using public transportation or carpooling to reduce emissions, and supporting sustainable practices such as organic farming. Additionally, governments and industries can implement policies and technologies that prioritize renewable energy sources, promote sustainable land use, and regulate pollution.

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Answer : The correct option is, 23.6 g

Explanation : Given,

Mass of [tex]Mg_3N_2[/tex] = 100.0 g

Mass of [tex]H_2O[/tex] = 75.0 g

Molar mass of [tex]Mg_3N_2[/tex] = 101 g/mol

Molar mass of [tex]H_2O[/tex] = 18 g/mol

First we have to calculate the moles of [tex]Mg_3N_2[/tex] and [tex]H_2O[/tex].

[tex]\text{Moles of }Mg_3N_2=\frac{\text{Given mass }Mg_3N_2}{\text{Molar mass }Mg_3N_2}[/tex]

[tex]\text{Moles of }Mg_3N_2=\frac{100.0g}{101g/mol}=0.990mol[/tex]

and,

[tex]\text{Moles of }H_2O=\frac{\text{Given mass }H_2O}{\text{Molar mass }H_2O}[/tex]

[tex]\text{Moles of }H_2O=\frac{75.0g}{18g/mol}=4.17mol[/tex]

Now we have to calculate the limiting and excess reagent.

The balanced chemical equation is:

[tex]Mg_3N_2(s)+6H_2O(l)\rightarrow 3Mg(OH)_2(aq)+2NH_3(g)[/tex]

From the balanced reaction we conclude that

As, 6 moles of [tex]H_2O[/tex] react with 1 mole of [tex]Mg_3N_2[/tex]

So, 4.17 moles of [tex]H_2O[/tex] react with [tex]\frac{4.17}{6}=0.695[/tex] moles of [tex]Mg_3N_2[/tex]

From this we conclude that, [tex]Mg_3N_2[/tex] is an excess reagent because the given moles are greater than the required moles and [tex]H_2O[/tex] is a limiting reagent and it limits the formation of product.

Now we have to calculate the moles of [tex]NH_3[/tex]

From the reaction, we conclude that

As, 6 moles of [tex]H_2O[/tex] react to give 2 moles of [tex]NH_3[/tex]

So, 4.17 moles of [tex]H_2O[/tex] react to give [tex]\frac{2}{6}\times 4.17=1.39[/tex] mole of [tex]NH_3[/tex]

Now we have to calculate the mass of [tex]NH_3[/tex]

[tex]\text{ Mass of }NH_3=\text{ Moles of }NH_3\times \text{ Molar mass of }NH_3[/tex]

Molar mass of [tex]NH_3[/tex] = 17 g/mole

[tex]\text{ Mass of }NH_3=(1.39moles)\times (17g/mole)=23.6g[/tex]

Therefore, the maximum theoretical yield of [tex]NH_3[/tex] is, 23.6 grams.

The maximum theoretical yield of NH3 when 100.g Mg3N2 reacts with 75.0 g H2O is 23.6 g, as H2O is the limiting reactant.

To determine the maximum theoretical yield of NH3, start by calculating the number of moles for both reactants. The molar mass of Mg3N2 is 100.93 g/mol, so you have 100 g / 100.93 g/mol = 0.991 moles of Mg3N2. The molar mass of H2O is 18.02 g/mol, so you have 75 g / 18.02 g/mol = 4.16 moles of H2O.

According to the stoichiometry of the reaction, Mg3N2 reacts with 6H2O to produce 2NH3. Thus, the moles of H2O is not enough to react with all the moles of Mg3N2, making H2O the limiting reactant. This means that the reaction will stop once all the H2O is consumed.

From the reaction stoichiometry, 6 moles of H2O produce 2 moles of NH3. So, 4.16 moles of H2O will produce (2/6)*4.16 = 1.39 moles of NH3. The molar mass of NH3 is 17.03 g/mol, so the maximum theoretical yield of NH3 is 1.39 moles * 17.03 g/mol = 23.6 g.

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None of the given options are correct, and the correct answer is 174 K.

Explanation:

Mass of N = 41.6 g

Moles = [tex]$\frac{given mass}{molar mass}[/tex]

      = [tex]$\frac{41.6 g}{28 g/ mol}[/tex] = 1.5 moles

Pressure, P = 815 mm Hg = 1.07 atm

Volume, V = 20 L

R = gas constant = 0.08205 L atm mol⁻¹ K⁻¹

Temperature, T = ? K

We have to use the ideal gas equation,  

PV = nRT  

by rearranging the equation, so that the equation becomes,  

T = [tex]$\frac{PV}{nR}[/tex]

 Plugin the above values, we will get,  

T = [tex]$\frac{1.07 \times 20}{1.5 \times 0.08205}[/tex]

  = 174 K

So the temperature of the nitrogen gas is 174 K.

Final answer:

The temperature at which 41.6 grams of nitrogen exert a pressure of 815 mmHg in a 20.0L cylinder is calculated using the ideal gas law and is approximately 177 Kelvin.

Explanation:

To find the temperature at which 41.6 grams of nitrogen (N₂) will exert a pressure of 815 mmHg in a 20.0L cylinder, we need to use the ideal gas law, which is PV = nRT.

First, we convert the mass of nitrogen to moles. The molar mass of N₂ is 28.02 g/mol, so:

moles of N₂ = 41.6 g ÷ 28.02 g/mol = 1.484 moles of N₂

Using the ideal gas law:

R = 62.36 L mmHg / (mol·K)

We have:

PV = nRT

(815 mmHg)(20.0 L) = (1.484 mol)(62.36 L mmHg / mol·K)T

T = (815 mmHg × 20.0 L) / (1.484 mol × 62.36 L mmHg / mol·K)

T = 16370 mmHg·L / (92.48104 mol·L mmHg / mol·K)

T = 177 K (rounded to 3 significant figures)

The temperature at which 41.6 grams of nitrogen will exert a pressure of 815 mmHg in a 20.0L cylinder is approximately 177 Kelvin.

Each element in the periodic table has two numbers. The first is the atomic number that represents the number of protons in the nucleus. The second is the atomic weight that accounts for the average mass of the isotopes of the element.

In the periodic table, each element is represented with two numbers. The larger number, usually found on top, is the atomic number, which signifies the number of protons present in the nucleus of the atom. The second number is the atomic weight or atomic mass, which is usually found at the bottom of the element symbol. It represents the average mass of the isotopes of that element, considering their abundance. For instance, for Carbon (C), the atomic number is 6 (protons) and the atomic weight is about 12.01 (protons + neutrons).

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Answer: This unknown powder is most likely made up of ionic bond.

Explanation:

An ionic compound is defined as the compound formed due to transfer of electrons between its atoms.

As we know that like dissolves like. Therefore, an ionic compound is readily soluble in a polar solvent like water.

Hence, when an unknown white powder is added to a beaker of water and stirred. The powder disappears after a few seconds because the white powder is ionic in nature and it is made up of ionic bond.

Answer : The number of moles of gas inside the car is, 105.0 mole.

Explanation :

To calculate the moles of gas we are using ideal gas equation.

[tex]PV=nRT[/tex]

where,

P = Pressure of gas = 98.5 kPa = 0.972 atm     (1 atm = 101.3 kPa)

V = Volume of gas = 2600 L

n = number of moles of gas = ?

R = Gas constant = [tex]0.0821L.atm/mol.K[/tex]

T = Temperature of gas = [tex]20^oC=273+20=293K[/tex]

Now put all the given values in above equation, we get:

[tex]0.972atm\times 2600L=n\times (0.0821L.atm/mol.K)\times 293K[/tex]

[tex]n=105.0mol[/tex]

Therefore, the number of moles of gas inside the car is, 105.0 mole.

Answer:

Zero

Explanation:a ionic compound consists of an equal number or positive and negative ions

The two processes of carbon cycle are rapid carbon exchange and the long-term cycling of carbon.

The carbon cycle consists of two interconnected processes: rapid carbon exchange among living organisms and the long-term cycling of carbon through geologic processes.

In the first process, photosynthesis consumes carbon dioxide and produces oxygen, while aerobic respiration consumes oxygen and produces carbon dioxide. These two processes play an important role in the carbon cycle.

In the second process, carbon is stored for long periods in carbon reservoirs such as the atmosphere, bodies of liquid water, ocean sediment, soil, land sediments, and the Earth's interior.

Learn more about Two processes of the carbon cycle here:

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Answer:

A sublevel is an energy level defined by quantum theory.

Explanation:

In chemistry, sublevels refer to energies associated with electrons. In physics, sublevels may also refer to energies associated with the nucleus.

Answer:e

The level of energy possessed by all of the electrons in one type of orbital.

Explanation:

I took the test.

The always true statement for the freezing of water is that the entropy change of the universe (ΔSₙₙₕₑ) is greater than zero, signaling a spontaneous process.

The statement that is always TRUE for the freezing of water is ΔSₙₙₕₑ > 0. During the freezing process, the system which is the water being frozen, undergoes a decrease in entropy (ΔS < 0) since the water molecules become more ordered. However, the entropy change of the surroundings (ΔSₙₙₕₑ) is positive because the heat rejected during freezing increases the entropy of the surroundings even more. As a result, the entropy of the universe increases (ΔSₙₙₕₑ > 0), making the overall process spontaneous as the second law of thermodynamics predicts that the entropy of the universe should increase in a spontaneous process.

Answer:

Prophase

Explanation:

During prophase, the chromosomes condense, the nucleolus disappears, and the nuclear envelope breaks down.

Answer: It should be Prophase I am 100% sure

Answer:

\large \boxed{\text{12.3 mol HCl}}  

Explanation:

We need a balanced chemical equation with moles.

            2HCl +Ca(OH)₂ ⟶ CaCl₂ + 2H₂O

n/mol:    12.3

The molar ratio is 2 mol H₂O:2 mol HCl.

[tex]\text{Moles of H$_{2}$O} = \text{12.3 mol HCl} \times \dfrac{\text{2 mol H$_{2}$O}}{\text{2 mol HCl}} = \textbf{12.3 mol HCl}\\\\\text{The reaction produces $\large \boxed{\textbf{12.3 mol HCl}}$}[/tex]

Assuming a stoichiometric relationship where 2 moles of HCl react with 1 mole of Ca(OH)₂ to produce 2 moles of H₂O, 12.3 moles of HCl would theoretically produce 12.3 moles of H₂O.

The question is about determining how many moles of H₂O will be produced from 12.3 moles of HCl reacting with Ca(OH)₂. To solve this, it's essential to know the chemical reaction involved. Unfortunately, the reaction between HCl and Ca(OH)₂, which typically forms CaCl₂ and H₂O, is not provided in full detail in the question. However, knowing that HCl reacts with base like Ca(OH)₂ to produce water and a salt, and typically in stoichiometric reactions involving a strong acid like HCl and a strong base like Ca(OH)₂, the ratio often is 2 moles of HCl react with 1 mole of Ca(OH)₂ to produce 2 moles of water (as a simplified approximation). While an exact reaction equation is necessary for a precise answer, if we assume the reaction follows a simple stoichiometry of 2HCl + Ca(OH)₂ → 2H₂O + CaCl₂, then for every 2 moles of HCl, 2 moles of H₂O are produced. Therefore, if 12.3 moles of HCl react completely with an adequate amount of Ca(OH)₂, they would produce 12.3 moles of H₂O, assuming the reaction goes to completion and all the HCl is used.

Answer:

29.3 atm

Explanation:

We need to use the Ideal Gas Law to solve this problem: PV = nRT, where P is pressure, V is volume, n is moles, R is the gas constant, and T is the temperature in Kelvin.

Here, volume is V = 500 mL = 0.500 L; moles is n = 0.60 mol; R is 0.08206 atm/(mol * K); and temperature is T = 25 + 273 = 298 K. Plug these into the equation to solve for P:

P * (0.500 L) = (0.60 mol) * (0.08206 atm/mol * K) * (298 K)

P ≈ 29.3 atm

Hope this helps!

Answer:

the osmolarity of the 0.85% NaCl solution is approximately equal to 300 mosmol/L.

Explanation:

Molarity= number of moles/volume of the solution in liters

volume of the solution= 100 mL

1 L= 1000 mL

100 mL= 100/1000=0.1 L

molar mass of NaCl= 58.44 g/mol

number of moles= mass in gram/gram molecular mass

= 0.85/58.44

= 0.01455

molarity= number of moles/volume of the solution in liters

= 0.01455 / 0.1

= 0.1455 M

1 M= 1000 mM

so 0.1455 M = 0.1455 × 1000

= 145.5 mM

Osmolarity is the concentration of solutes in the solution.

NaCl dissociates to Na+ and Cl-

so osmolarity of 145.5 mM NaCl= 2 × 145.5

= 291 mosmol/L

Therefore, we conclude that the osmolarity of the 0.85% NaCl solution is approximately equal to 300 mosmol/L.

Answer:

The muscle cell need to use most entry in a typical day

The cells that use most of the energy in a typical day are the cells of the brain, the cells of the heart, the cells of the lungs, the muscle cells, etc., and all the involuntary cells use the energy in a typical day because they do so spontaneously.

The body is made up of many different types of cells, some of which are voluntarily active and work while others are involuntarily work and always do their job. Even when a person is not doing much physical activity during the day, the cells of the heart (cardiac cells), brain, lungs, and other organs are constantly functioning and require continuous energy. When more physical work is done in a typical day, muscle cells or skeletal muscles require more energy and use more ATP to complete the work.

Hence The cells that use most of the energy in a typical day are the cells of the brain, the cells of the heart, the cells of the lungs, the muscle cells, etc.

Learn more about the cells here.

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Answer:

D

Explanation:

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Ammonium hydroxide, a weak base, according to the Arrhenius definition, gives up some of its OH- ions in solution.

Ammonium hydroxide is considered a weak base according to the Arrhenius definition beacause it dissociates in water to some extent and produces hydroxide ions (OH-). So, the correct choice in this case is (D) 'gives up some of its OH in solution'. It doesn't receive most of its H+ in solution, which makes options A and B incorrect, and it does not receive most of its OH- ions instead it donates them in the solution, making option C incorrect as well.

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Answer:

violet

Explanation:

Violet has the shortest wavelength at 380 nanometers

The correct option is 1 i.e, Violet light has the shortest wavelength in the visible spectrum at approximately 380-450 nm and carries the most energy. Red light has the longest wavelength, about 620-750 nm, and the least energy.

The visible light spectrum consists of a range of colors that our eyes perceive as different wavelengths. Of these colors, violet light has the shortest wavelength, approximately 380-450 nanometers (nm). Because it has the shortest wavelength, violet light also carries the most energy. On the other end of the spectrum, red light has the longest wavelength, about 620-750 nm, and thus carries the least energy. To remember the order of colors from longest to shortest wavelength, you can use the mnemonic ROY G BIV, which stands for Red, Orange, Yellow, Green, Blue, Indigo, and Violet.

0.027 moles of [tex]H_{2} S_{} 0_{4}[/tex] if  there are 1.64x[tex]10^{22}[/tex] molecules of [tex]H_{2} S_{} O_{4}[/tex]

Explanation:

Data given:

number of molecules of [tex]H_{2} S_{} 0_{4}[/tex] = 1.64 X [tex]10^{22}[/tex]

Atomic weight of the sulphuric acid = 98.07 grams/mole

We know that 1 mole of sulphuric acid has 6.022 x [tex]10^{23}[/tex] (Avagadro number) molecules.

so number of moles present in 1.64 X [tex]10^{22}[/tex]   molecules is given by:

so to get moles we will use

number of moles = [tex]\frac{number of molecules given}{avagadro number}[/tex]

number of moles = [tex]\frac{1.64 X 10^{22} }{6.022 X 10^{23} }[/tex]

number of moles = 0.027 moles

So, 1.64 X [tex]10^{22}[/tex]  molecules will be there in 0.027 moles of sulphuric acid.

Answer:

Your answer is Energy

Answer:

i hate my life  PERIODT

Explanation:

WHY AM I HERE :/

Answer : The number of moles of [tex]NaCl[/tex] formed are, 0.69 moles.

Explanation : Given,

Moles of [tex]CaCl_2[/tex] = 0.345 mol

Now we have to calculate the moles of [tex]NaCl[/tex]

The balanced chemical equation is:

[tex]1Na_2CO_2(aq)+1CaCl_2(aq)\rightarrow 1CaCO_3(s)+2NaCl(aq)[/tex]

From the balanced reaction, we conclude that

As, 1 mole of [tex]CaCl_2[/tex] react to give 2 moles of [tex]NaCl[/tex]

So, 0.345 mole of [tex]CaCl_2[/tex] react to give [tex]2\times 0.345=0.69[/tex] mole of [tex]NaCl[/tex]

Therefore, the number of moles of [tex]NaCl[/tex] formed are, 0.69 moles.

1 Na₂CO₃(aq) + 1 CaCl₂(aq) → 1 CaCO₃(s) + 2 NaCl(aq) = 0.690 moles.

If 0.345 moles of calcium chloride (CaCl₂) react, it will produce 0.690 moles of sodium chloride (NaCl) based on the balanced chemical equation provided.

0.345 moles CaCl₂ × 2 moles NaCl / 1 mole CaCl₂ = 0.690 moles NaCl

So, 0.345 moles of calcium chloride will produce 0.690 moles of sodium chloride.

Correct question is: Calculate the number of moles of sodium chloride (NaCl) formed if 0.345 moles of calcium chloride (CaCl2) react.
1 Na2CO3 (aq) + 1 CaCl2 (aq) – 1 CaCO3 (s) + 2 NaCl (aq) = ________ Moles ?

Answer : One mole of an ideal gas  occupies a volume of 22.4  liters at STP.

Explanation :

As we know that 1 mole of substance occupies 22.4 liter volume of gas at STP conditions.

STP stands for standard temperature and pressure condition.

At STP, pressure is 1 atm and temperature is 273 K.

By using STP conditions, we get the volume of 22.47 liter.

Hnece, the one mole of an ideal gas  occupies a volume of 22.4  liters at STP.

The bromine percentage is 49.42 %

Explanation:

Mass of AgBr precipitated =   0.31 g

Molecular weight of AgBr =  187.77 g mol - 1

moles of AgBr =   0.31 g by 187.77 g mol - 1 =   0.0016509 moles

moles of Br ion =  0.0016509 moles

Mass of Br ion =   0.0016509 moles into 79.904 g mol - 1 =  0.1319 g

The Total mass of compound = 0.2669 g

Percentage of bromine = 0.1319 by 0.2669 = 49.42 percent

Hence the bromine percentage is 49.42 %

Answer:

dihydrogen dioxide, hydrogen dioxide, hydrogen oxide, oxydol, peroxide, H2O