CH₂-CH3
CH3-CH₂-CH-CH-CH₂-CH3
-CH-CH-
CH₂-CH3
What is this compound?

After the reaction is complete, no nitrogen and no hydrogen molecules remain, and 8.00 x 1014 molecules of NH3 are produced.

In the equation, nitrogen and hydrogen react at a high temperature, in the presence of a catalyst, to produce ammonia, according to the balanced chemical equation:N2(g)+3H2(g)⟶2NH3(g)The coefficients of each molecule suggest that one molecule of nitrogen reacts with three molecules of hydrogen to create two molecules of ammonia.

So, to determine how many molecules of ammonia are produced when four nitrogen and nine hydrogen molecules are present, we must first determine which of the two reactants is the limiting reactant.

To find the limiting reactant, the number of moles of each reactant present in the equation must be determined.

Calculations:
Nitrogen (N2) molecules = 4Hence, the number of moles of N2 = 4/6.02 x 1023 mol-1 = 6.64 x 10-24 mol
Hydrogen (H2) molecules = 9Hence, the number of moles of H2 = 9/6.02 x 1023 mol-1 = 1.50 x 10-23 mol

Now we have to calculate the number of moles of NH3 produced when the number of moles of nitrogen and hydrogen are known, i.e., mole ratio of N2 and H2 is 1:3.

The mole ratio of N2 to NH3 is 1:2; thus, for every 1 mole of N2 consumed, 2 moles of NH3 are produced.
The mole ratio of H2 to NH3 is 3:2; thus, for every 3 moles of H2 consumed, 2 moles of NH3 are produced.
From these mole ratios, it can be observed that the limiting reactant is nitrogen.

Calculation for NH3 production:
Nitrogen (N2) moles = 6.64 x 10-24 moles
The mole ratio of N2 to NH3 is 1:2; therefore, moles of NH3 produced is 2 × 6.64 × 10−24 = 1.33 × 10−23 moles.

Now, to determine how many molecules of NH3 are produced, we need to convert moles to molecules.
1 mole = 6.02 x 1023 molecules
Thus, 1.33 x 10-23 moles of NH3 = 8.00 x 1014 molecules of NH3 produced.

To find the amount of each reactant remaining after the reaction is complete, we must first determine how many moles of nitrogen are consumed, then how many moles of hydrogen are consumed, and then subtract these from the initial number of moles of each reactant.

The moles of nitrogen consumed = 4 moles × 1 mole/1 mole N2 × 2 mole NH3/1 mole N2 = 8 moles NH3
The moles of hydrogen consumed = 9 moles × 2 mole NH3/3 mole H2 × 2 mole NH3/1 mole N2 = 4 moles NH3
Thus, the moles of nitrogen remaining = 6.64 × 10−24 mol – 8 × 2/3 × 6.02 × 10^23 mol-1 = 5.06 × 10−24 mol
The moles of hydrogen remaining = 1.50 × 10−23 mol – 4 × 2/3 × 6.02 × 10^23 mol-1 = 8.77 × 10−24 mol

Finally, the number of molecules of each reactant remaining can be calculated as follows:
Number of N2 molecules remaining = 5.06 × 10−24 mol × 6.02 × 10^23 molecules/mol = 3.05 × 10−1 molecules ≈ 0 molecules
Number of H2 molecules remaining = 8.77 × 10−24 mol × 6.02 × 10^23 molecules/mol = 5.28 × 10−1 molecules ≈ 0 molecules.

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Answer:

See Explanation

Explanation:

There is a concept in chemistry called the denticity of  a ligand. The denticity of a ligand refers to the number of donor groups in a given ligand that can bond to a central metal atom or ion. In other words, it is the number of bonding positions available in a ligand.

Ammonia has only one bonding position(monodentate ligand); that is, the lone pair on its nitrogen atom. Hence, six ammonia ligands are required to form an octahedral complex with the nickel center.

However, ethylenediamine has two positions available for bonding to a central metal atom or ion. These are the two nitrogen atoms present in the molecule. Hence, each molecule of ethylenediamine is bidentate, bonding to the nickel using two "teeth". Hence, three ethylenediamine molecules form six bonds to the nickel center as required in an octahedral complex.

Answer:

Fresh milk has several chemical properties. It is a good source of nutrients such as carbohydrates, proteins, and fats, as well as vitamins and minerals. It is also a source of enzymes and hormones. One important enzyme found in fresh milk is lactase, which helps to digest lactose, a type of sugar found in milk. Fresh milk also contains lactic acid, which gives it a slightly sour taste. It also has a pH of around 6.5-6.7, which is slightly acidic. Milk also contains a number of antimicrobial agents, such as lactoferrin and lysozyme, which help to protect against the growth of harmful bacteria.

Explanation:BRAINLIEST PLS

Answer:

The half-life of polonium-210 is approximately 138.792 days.

Explanation:

We must remember that the decay of a radioisotope is modelled by this ordinary differential equation:

\(\frac{dm}{dt} = -\frac{m(t)}{\tau}\)

Where:

\(m(t)\) - Current mass of the isotope, measured in grams.

\(\tau\) - Time constant, measured in days.

Whose solution is:

\(m(t) = m_{o}\cdot e^{-\frac{t}{\tau} }\)

Where \(m_{o}\) is the initial mass of the isotope, measured in grams.

Our first step is to determine the value of the time constant:

\(-\frac{t}{\tau} = \ln \frac{m(t)}{m_{o}}\)

\(\tau = -\frac{t}{\ln \frac{m(t)}{m_{o}} }\)

If we know that \(\frac{m(t)}{m_{o}} = 0.016\) and \(t = 828\,days\), then the time constant of the radioisotope is:

\(\tau = -\frac{828\,days}{\ln 0.016}\)

\(\tau \approx 200.234\,days\)

And lastly we find the half-life of polonium-210 (\(t_{1/2}\)), measured in days, by using this expression:

\(t_{1/2} = \tau \cdot \ln 2\)

\(t_{1/2} = (200.234\,days)\cdot \ln 2\)

\(t_{1/2}\approx 138.792\,days\)

The half-life of polonium-210 is approximately 138.792 days.

B ) Hydrogen

as O2 helps in combustion and Fuel is the one which is going to combust and heat is required to bring fuel to the combustion temperature

Which of the following is NOT a requirement for combustion to occur?

A. Fuel

B. Hydrogen

C. Heat

D. Oxygen

Answer:-\( \bold \pink{hydrogen}\)

The four elements are oxygen for sustaining combustion, enough heat for raising the material to the ignition temperature, combustible material or fuel, and a subsequent exothermic chain reaction in the material.

No se si aun necesitas ayuda o no

The molecular formula is twice the empirical formula which is (NH₂)₂ or N₂H₄.

To determine the molecular formula of the compound, find the empirical formula first. The empirical formula gives the simplest whole number ratio of atoms present in a compound.

Assuming we have 100 g of the compound, then 87.4 g of it is nitrogen and 12.6 g of it is hydrogen:

moles of N = 87.4 g / 14.01 g/mol = 6.24 mol

moles of H = 12.6 g / 1.01 g/mol = 12.5 mol

Find the simplest whole number ratio of moles of nitrogen to moles of hydrogen. To do this, we divide both values by the smaller one (in this case, 6.24 mol):

moles of N / 6.24 = 6.24 mol / 6.24 mol = 1

moles of H / 6.24 = 12.5 mol / 6.24 mol = 2

So the empirical formula is NH₂.

To find the molecular formula, know the molecular mass of the compound

The molecular mass of the compound is given as 32.05 g/mol. The empirical formula mass of NH₂ is:

empirical formula mass = 14.01 g/mol + 2(1.01 g/mol) = 16.03 g/mol

The molecular formula mass is a multiple of the empirical formula mass, divide the molecular mass by the empirical formula mass to find the multiple:

molecular mass / empirical formula mass = 32.05 g/mol / 16.03 g/mol = 2

Therefore, the molecular formula is twice the empirical formula:

(NH₂)₂ or N₂H₄.

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Answer:

\(\boxed{O_2 \: ^{2-} (\sigma2s)^2(\sigma∗2s)^2(\sigma2pz)^2(π2py,π2px)^4(π∗2py,π∗2px)^4}\)

\(\boxed{O_2 \: ^{1-}(\sigma2s)^2(\sigma∗2s)^2(\sigma2pz)^2(π2py,π2px)^4{ (π∗2py)}^{2} {(π∗2px)}^{1}}\)

Explanation:

\(\sf \: Electronic \: configuration \: of \: O_2 \: ^{2-} and \: O_2 \: ^{1-}\)

Electronic configuration of any diatomic molecule can be determined using MOT(molecular orbital theory).

To know the electronic configuration of above two molecules, draw the MOT of O2 molecule.(refer the diagram)

There are 16 electrons in O2 molecule out of which Four electrons are in non bonded state. Remaining 12 electrons of 16 will be filled according to MOT, since O2 is not a S-P mixing case, in without S-P mixing case the sigma orbital(σ2pz) lies below the Pi orbital(π2px,π2py) in bonding state as you can see in the diagram, on other hand the other diatomic molecules like B2, C2 & N2 are S-P mixing case where Pi orbital lies below and sigma orbital lies above.

Now, the electronic configuration of O2 molecule is

\((\sigma2s)^2(\sigma∗2s)^2(\sigma2pz)^2(π2py,π2px)^4(π∗2py,π∗2px)^2 \)

There are two electrons unpaired electrons in MOT hence the O2 molecule is paramagnetic which contradicts VBT, Thats why MOT dominant VBT.

in case of O2^2-(peroxide linkage) the two electrons enters in the Anti Bonding of pi orbital. hence the electronic configuration of O2^2- is

\((\sigma2s)^2(\sigma∗2s)^2(\sigma2pz)^2(π2py,π2px)^4(π∗2py,π∗2px)^4\)

since the HOMO (highest occupied molecular orbital) is paired the O2^2- is diamagnetic in nature.

Coming to O2^1- (superoxide linkage) the one electron enters in the Anti Bonding of pi orbital hence the electronic configuration comes out,

\((\sigma2s)^2(\sigma∗2s)^2(\sigma2pz)^2(π2py,π2px)^4{ (π∗2py)}^{2} {(π∗2px)}^{1} \)

The HOMO of O2^1- is unpaired hence it is Paramagnetic in nature.

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The volume of oxygen gas produced by the decomposition of 3.05 g KCIO₃ according to the given equation is 1.68 liters

Let us begin by obtaining the mole of 3.05 g of KClO₃. Details below:

Mole = mass / molar mass

Mole of KClO₃ = 3.05 / 122.5

Mole of KClO₃ = 0.025 mole

Next, we shall determine the mole of of oxygen gas, O₂ produced from the reaction. Details below:

KClO₃ -> 2KCl + 3O₂

From the balanced equation above,

1 mole of KClO₃ reacted to produced 3 moles of O₂

Therefore,

0.025 mole of KClO₃ will react to produce = 0.025 × 3 = 0.075 mole of O₂

Finally, we shall obtain the volume of oxygen gas, O₂ produced. This is shown below

At STP,

1 mole of O₂ = 22.4 Liters

Therefore,

0.075 moles of O₂ = 0.075 × 22.4

0.075 moles of O₂ = 1.68 liters

Thus, the volume of oxygen gas, O₂ produced is 1.68 liters

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Answer:

Crust

Explanation:

Answer:

The crust

Explanation:

Answer:

Last one

hope it helps mvhsbshsjjak

Answer:The lungs expel the carbon dioxide and bring in new oxygen-containing air. Only when both systems are working together can oxygen and carbon dioxide be successfully exchanged between cells and environment. There are many other examples of this cooperation in your body.

Explanation:

Hope it will help

Question:

A body system is a group of organs that work together to keep the organism

alive. How does the respiratory system help to keep an organism alive?

A. The respiratory system helps the organism respond to its

environment.

B. The respiratory system helps the organism absorb nutrients from

its environment.

O C. The respiratory system takes in oxygen and releases carbon

dioxide.

O D. The respiratory system carries oxygen to the organism's cells.​

Answer:

O C. The respiratory system takes in oxygen and releases carbon

dioxide.

Explanation:

Breathing uses chemical and mechanical processes to bring oxygen to every cell of the body and to get rid of carbon dioxide. Our body needs oxygen to obtain energy to fuel all our living processes. Carbon dioxide is a waste product of that process

Hope This Helps?

Answer is B

A mixture means two compounds mixed together but not atomically. For example, sand and water solution. A water with sand mixed inside is a mixture because the sand can be separated by physical means.

Water is H2O. This means it is a compound, because hydrogen and oxygen is bonded together atomically. Hydrogen however is an element, because you can't seperate it anymore (You could seperate it in the sense of protons and neutrons, but the definition of element is something you can see on the periodic table)

Compound means more than one element bonded together.

The sample must be a compound because it couldn't be seperated by physical means but can be seperated by chemical means into three pure substances (synonym of element)

The question is incomplete, the complete question is:

Nitrogen and fluorine react to form nitrogen fluoride according to the chemical equation:

\(N_2(g)+3F_2(g)\rightarrow 2NF_3(g)\)

A sample contains 19.3 g of \(N_2\) is reacted with 19.3 g of \(F_2\). Now we need to find the amount of \(NF_3\) that can be formed by the complete reactions of each of the reactants.

If all of the \(N_2\) was used up in the reaction, how many moles of \(NF_3\) would be produced?

Answer: 1.378 moles of \(NF_3\) are produced in the reaction.

Explanation:

The number of moles is defined as the ratio of the mass of a substance to its molar mass.

\(\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}\)       ......(1)

Limiting reagent is defined as the reagent which is completely consumed in the reaction and limits the formation of the product.

Excess reagent is defined as the reagent which is left behind after the completion of the reaction.

In the given chemical reaction, \(N_2\) is considered as a limiting reagent because it limits the formation of the product and it was completely consumed in the reaction.

We are given:

Mass of \(N_2\) = 19.3 g

Molar mass of \(N_2\) = 28.02 g/mol

Putting values in equation 1:

\(\text{Moles of }N_2=\frac{19.3g}{28.02g/mol}=0.689mol\)

For the given chemical reaction:

\(N_2(g)+3F_2(g)\rightarrow 2NF_3(g)\)

By the stoichiometry of the reaction:

1 mole of \(N_2\) produces 2 moles of \(NF_3\)

So, 0.689 moles of \(N_2\) will produce = \(\frac{2}{1}\times 0.689=1.378mol\) of \(NF_3\)

Hence, 1.378 moles of \(NF_3\) are produced in the reaction.

the Calorimetry relationships you can find the amount of water in the calorimeter is      m = 21.3 g

given parameters

to find

The body of water

Thermal energy is the energy stored in the body that can be transferred as heat when two or more bodies are in contact. Calorimetry is a technique where the energy is transferred between the body only in the form of heat and in this case the thermal energy of the lead is transferred to the calorimeter that reaches the equilibrium that the thematic energy of the two is equal

              Q_{ceded} = Q_{absorbed}

Lead, because it is hotter, gives up energy

              Q_{ceded} = M c_{e Pb} (T₁ - T_f)

The calorimeter that is colder absorbs the heat

              Q_{absrobed} = m c_{e H_2O} (T_f - T₀)

where M and m are the mass of lead and water, respectively, c are the specific heats, T₁ is the temperature of the hot lead, T₀ the temperature of cold water and T_f the equilibrium temperature

              M c_{ePb} (T₁ - T_f) = m c_{eH2O} (T_f - T₀)

               m = \(\frac{ M\ c_{ePb} \ (T_1 - T_f)}{c_{eH_2O} \ (T_f - T_o)}\)

let's calculate

              m = \(\frac{200 \ 0.129 (176.4-56.4)}{ 4.186 \ (56.4 -21.7)}\)

              m = 3096 / 145.25

              m = 21.3 g

Using the Calorimetry relationships you can find the amount of water in the calorimeter is:

             m = 21.3 g

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Answer:

C

Explanation:

there is no explanation needed

Answer:

The value of ionization energy (IE) decreases down the group due to the increasing size as the valence electrons are more loosely bound. Thus lowest IE in this case is of Bi as it is bottom most element.

Explanation:

If a H₂ sample has a diffusion rate of 955 m/s, 5.95 is the rate of a Cl2 sample at the same temperature.

Graham's law states that a gas's rate of diffusion or effusion is inversely proportional to its molar mass squared. The Formula can be written as follows. M1 denotes the molar mass of gas. 1. M2 denotes the molar mass of gas. 2. Rate1 is the rate of the first gas's effusion.

It supports in the separation of gases with varying densities. It aids in the separation of certain element isotopes. It aids in determining the molecular weight of an unknown gas by utilizing effusion rates.

According to Grahm's law of diffusion

rate (gas A) × √molar mass(gas A) = rate(gas B) × √molar mass (gas B)

For H₂ gas and Cl₂ gas

r H₂ / r Cl₂ = √molar mass of Cl₂ / molar mass of H₂

= √70.90 / 2

= √35.45

= 5.95

Thus, If a H₂ sample has a diffusion rate of 955 m/s, 5.95 is the rate of a Cl2 sample at the same temperature.

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Answer:

The cell potential for the given galvanic cell is 0.188 V.

Explanation:

To calculate the cell potential, we can use the Nernst equation:

Ecell = E°cell - (RT/nF)ln(Q)

where E°cell is the standard cell potential, R is the gas constant (8.314 J/mol·K), T is the temperature in Kelvin (25°C = 298 K), n is the number of moles of electrons transferred (in this case, n = 2), F is the Faraday constant (96,485 C/mol), and Q is the reaction quotient.

First, we need to write the half-reactions and their standard reduction potentials:

Sn4+(aq) + 2e- → Sn2+(aq) E°red = 0.15 V

Fe3+(aq) + e- → Fe2+(aq) E°red = 0.77 V

The overall reaction is the sum of the half-reactions:

Sn2+(aq) + 2Fe3+(aq) → Sn4+(aq) + 2Fe2+(aq)

The reaction quotient Q can be expressed as:

Q = [Sn4+][Fe2+]^2 / [Sn2+][Fe3+]^2

Substituting the given concentrations, we get:

Q = (0.00655)(0.01139)^2 / (0.0624)(0.0437)^2 = 0.209

Now we can calculate the cell potential:

Ecell = 0.15 V + 0.0592 V log([Fe2+]^2/[Fe3+]) + 0.0592 V log([Sn4+]/[Sn2+])

= 0.15 V + 0.0592 V log(0.01139^2/0.0437^2) + 0.0592 V log(0.00655/0.0624)

= 0.188 V

Therefore, the cell potential for the given galvanic cell is 0.188 V.

The cell potential for the given galvanic cell in which the given reaction occurs at 25 °C is 0.188 V.

To find the cell potential, we take the Nernst equation:

Ecell = E°cell - (RT/nF)ln(Q)

In which R is the gas constant (8.314 J/mol·K) and E° cell is the standard cell potential.

T temperature in Kelvin (25°C = 298 K), and n is the number of moles of electrons transferred (n = 2), Q is the reaction quotient and F is the Faraday constant (96,485 C/mol).

Firstly, write the half-reactions and then their standard reduction potentials:

Sn⁴⁺(aq) + 2e⁻  → Sn²⁺(aq) E°red = 0.15 V

Fe³⁺(aq) + e⁻ → Fe²⁺(aq) E°red = 0.77 V

The overall reaction is the sum of the half-reactions:

Sn²⁺(aq) + 2Fe³⁺(aq) → Sn⁴⁺(aq) + 2Fe²⁺(aq)

The Q reaction quotient can be written as:

Q = [Sn⁴⁺][Fe²⁺]² ÷ [Sn²⁺][Fe²⁺]²

Substituting the given concentrations, we observe:

Q = (0.00655)(0.01139)² ÷ (0.0624)(0.0437)² = 0.209

Next, we can find the cell potential:

Ecell = 0.15 V + 0.0592 V log([Fe²⁺]²/[Fe³⁺]) + 0.0592 V log([Sn⁴⁺]/[Sn²⁺])

= 0.15 V + 0.0592 V log(0.01139²÷0.0437²) + 0.0592 V log(0.00655÷0.0624)

= 0.188 V

Thus, the cell potential for the given galvanic cell is 0.188 V.

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This representation suggests that the element is phosphorus (P) with a mass number of 30, which is incorrect. The correct mass number for phosphorus is approximately 30.97. The incorrect representation for a neutral atom is 36Li

To determine the correct representation for a neutral atom, we need to consider the atomic number (Z) and mass number (A) of the element. The atomic number represents the number of protons in the nucleus, while the mass number represents the sum of protons and neutrons.

Let's analyze the given representations:

36Li:

This representation suggests that the element is lithium (Li) with a mass number of 36, which is incorrect. The correct mass number for lithium is approximately 6.94.

613C:

This representation suggests that the element is carbon (C) with a mass number of 13, which is correct. Carbon has different isotopes, and 13C represents one of its stable isotopes.

3063Cu:

This representation suggests that the element is copper (Cu) with a mass number of 63, which is correct. Copper has different isotopes, and 63Cu represents one of its stable isotopes.

1530P:

This representation suggests that the element is phosphorus (P) with a mass number of 30, which is incorrect. The correct mass number for phosphorus is approximately 30.97.

Therefore, the incorrect representation for a neutral atom is 36Li, as it does not match the known properties of lithium.

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Neon is the tenth element with a total of 10 electrons. So, the correct atom is neon.

The volume of carbon dioxide produced is approximately (d) 11.9 liters.

To determine the amount of carbon dioxide (C\(O_2\)) produced when 37.8 grams of carbon disulfide (C\(S_2\)) reacts with excess oxygen gas (\(O_2\)), we need to use stoichiometry and the given balanced chemical equation:

C\(S_2\)(l) + 3\(O_2\)(g) → C\(O_2\)(g) + 2S\(O_2\)(g)

First, we calculate the number of moles of C\(S_2\) using its molar mass:

Molar mass of (C\(S_2\)) = 12.01 g/mol (C) + 32.07 g/mol (S) × 2 = 76.14 g/mol

Number of moles of (C\(S_2\)) = mass / molar mass = 37.8 g / 76.14 g/mol ≈ 0.496 mol

From the balanced equation, we can see that the stoichiometric ratio between (C\(S_2\)) and C\(O_2\) is 1:1. Therefore, the number of moles of C\(O_2\) produced will also be 0.496 mol.

Now we can use the ideal gas law to calculate the volume of C\(O_2\) at the given temperature and pressure. The ideal gas law equation is:

PV = nRT

where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant (0.0821 L·atm/mol·K), and T is the temperature in Kelvin.

Converting the temperature from Celsius to Kelvin:

T(K) = 28.85°C + 273.15 = 302 K

Using the ideal gas law:

V = nRT / P = (0.496 mol) × (0.0821 L·atm/mol·K) × (302 K) / (1.02 atm) ≈ 11.9 L

The correct answer is 11.9 liters.

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Answer:

Explanation:

The subscripts in a formula determine the ratio of the moles of each element in the compound. To convert this formula to the empirical formula, divide each subscript by 2. This is similar to reducing a fraction to its lowest denominator.

Answer:polonium

Explanation:

.........

The correct answer is B. 8 molecules \(SO_3\). Option B

In the given reaction:

S(s) + \(O_2\)(g) → \(SO_3\)(g)

The stoichiometric coefficient in front of the \(SO_3\)molecule is 8, which indicates that 8 molecules of \(SO_3\)are formed as a product. This coefficient represents the ratio of the number of molecules involved in the reaction.

Option A (8 atoms \(SO_3\)) is incorrect because it only mentions the number of atoms, not molecules. The stoichiometric coefficient does not represent the number of atoms, but rather the number of molecules.

Option C (80.07g \(SO_3\)) is incorrect because it mentions a specific mass. The stoichiometric coefficient does not directly represent the mass of the substance, but rather the relative amount of molecules involved in the reaction.

Option D (32 \(SO_3\)) is incorrect because it mentions a specific volume. The stoichiometric coefficient does not directly represent the volume of the substance, but rather the relative amount of molecules involved in the reaction.

Therefore, the correct way to describe the \(SO_3\)component in the reaction is option B: 8 molecules \(SO_3\). This represents the ratio of the number of molecules of \(SO_3\)that are produced in the reaction.

Option B

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Students put solid butter and solid water on a table. The air temperature around the table is 20°C. After two hours, The butter will remain a solid, and the water will become a liquid. Therefore, option B is correct.

A state of matter is one of the various forms that matter can take. In everyday life, four states of matter are visible: solid, liquid, gas, and plasma.

On a table, students placed solid butter and solid water. The temperature of the air around the table is 20°C. The butter will remain solid after two hours, while the water will become liquid.

Thus, option B is correct.

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Your question is incomplete, most probably your question was

The pictures show butter and water in solid states. The melting point of each substance is shown.

Students put solid butter and solid water on a table. The air temperature around the table is 20°C.

A. The butter and water will both become liquids.

B. The butter will remain a solid, and the water will become a liquid.

C. The butter and water will both remain solids.

D. The butter will become a liquid, and the water will remain a solid.

Answer:

there are approximately 0.004118 moles in 0.1 g of magnesium.

Explanation:

The molar mass of magnesium is approximately 24.31 g/mol. To calculate the number of moles in 0.1 g of magnesium, we can use the following formula:

Number of moles = Mass / Molar mass

Number of moles = 0.1 g / 24.31 g/mol

Number of moles = 0.004118 mol (rounded to 3 significant figures)

Therefore, there are approximately 0.004118 moles in 0.1 g of magnesium.

Answer:

Explanation:

To calculate the number of moles of magnesium in 0.1 g of magnesium, we first need to determine the molar mass of magnesium. The molar mass of magnesium is 24.31 g/mol.

Using this information, we can use the following formula to calculate the number of moles of magnesium:

moles of magnesium = mass of magnesium / molar mass of magnesium

moles of magnesium = 0.1 g / 24.31 g/mol

moles of magnesium ≈ 0.00412 mol

Therefore, there are approximately 0.00412 moles of magnesium in 0.1 g of magnesium.

ANSWER

Option A

EXPLANATION

Base is a substance that will reacts with an acid that to produce salt and water only.

Base is also a substance that produce hydroxide ions in an aqueous solution.

Below are the properties of a base

1. A base has a pH value greater than 7

2. A base is slippery to touch

3. A base has the ability to release hydroxide ions in aqueous solution.

4. A base has the ability to dissolve fats and oils.

Hence, base does not have sour taste which make option A the correct answer

Therefore, the correct answer is option A

Answer:

3. d

4. c

5. i

6. h

7. a

8. g

9. j

10. b

11. e

12. f

Explanation:

The oxygen gas is non polar because there is no interaction between the molecules of the gas.

A diatomic molecule is one that has only two atoms in it. These atoms are usually atoms of the same element in the majority of the cases that we encounter. Given the fact that the both atoms belong to the same substance, the electronegativity difference between the atoms is zero.

Given that the electronegativity difference between the atoms is zero, there is little or no interaction between the molecules of the substance. Thus the very weak intermolecular interaction is coming from the fact that there is no kind of interaction between the molecules.

Thus oxygen gas is covalent and the molecules do not interact with each other because the bond is nonpolar.

Learn more about diatomic molecules:https://brainly.com/question/11815815

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