In a laboratory experiment, a fermenting aqueous solution of glucose and yeast produces carbon dioxide gas and ethanol. The solution was heated by burning natural gas in a Bunsen burner to distill the ethanol that formed in the flask. During the distillation, the ethanol evaporated and then condensed in the receiving flask. The flame of the burner was kept too close to the bottom of the flask and some of the glucose decomposed into a black carbon deposit on the inside of the flask. During this experiment the following changes occurred. Which of these changes involved a physical change and not a chemical change?
1. evaporation of ethanol
2. condensation of ethanol
3. formation of a carbon deposit inside the flask
4. formation of carbon dioxide gas from glucose
5. burning of natural gas
6. formation of ethanol from glucose by yeast

Answer:

The answer to your question is: KOH

Explanation:

Formula

Molarity = # of moles / volume

Process

a. No right answer.

b. 121.45 g of KOH in 75.0 mL

MW KOH = 56 g

                                    56 g --------------------- 1 mol

                                  121.45 g -----------------   x

                                x = (121.45 x 1) / 56

                               x = 2.17 mol

M = 2.17 / 0.075

M = 29

c. 23.49 g of NH4OH in 125.0 mL

MW NH4OH = 35 g

                                   35 g  --------------------  1 mol

                               23.49 g  ---------------------   x

                                   x = (23.49 x 1) / 35 = 0.67 mol

M = 0.67 / 0.125

M = 5.36

d. 217.5 g of LiNO3 in 2.00 L

MW LiNO3 = 69 g

                                69 g ----------------------  1 mol

                              217.5 g ----------------------  x

                                 x = (217.5 x 1) / 69 = 3.15 mol

M = 3.15 / 2

M = 1.6

e. 15.25 g of Pb(C2H3O2)2 in 65.0 mL

MW Pb(C2H3O2) = 266 g

                               266 g ------------------ 1 mol

                                 15.25g ...................   x

                              x = (15.25 x 1) / 266 = 0.06 mol

M = 0.06 / 0.065

M = 0.92

Answer:

The answer to your question is letter c) Sugar burns in air to form water and carbon dioxide.

Explanation:

Exist two kinds of phenomena: physical and chemical

physical phenomena are when matter only changes its physical state, like evaporation, condensation, sublimation, etc.

chemical phenomena are when matter changes, react and form a new compound.

a) Iodine (a purple solid) becomes a purple gas.  This is a physical change, sublimation, this answer is wrong.

b) Titanium is less dense than iron.  Density is a physical property of matter, this answer is incorrect.

c) Sugar burns in air to form water and carbon dioxide.  Sugar in transform into water and carbon dioxide, this is the right answer.

d) Water boils at 100 ∘C. Evaporation is a physical change, the answer is wrong.

The statement describing the chemical property has been the burning of sugar in air to form carbon dioxide and water. Thus, option C is correct.

The property of the element has been given as the physical and chemical property.

The physical property has been defined as the one in which the chemical composition has not been changed. It has been based on the appearance of the compound.

The chemical property has been the reactivity of the compound that results in the change in the chemical composition with the formation of new products.

The following changes have been classified as:

It has been the appearance and no change in the chemical composition. Thus, it is a physical property.

It has been based on the comparative density. There has been no reaction and change in chemical composition. Thus, it is a physical property.

The burning of sugar results in the change in the chemical composition with the formation of new product. Thus, it has been a chemical property.

The boiling and freezing results in the change in state of matter. There has been no change in the chemical composition, Thus, it has been a physical change.

Hence, the statement describing the chemical property has been the burning of sugar in air to form carbon dioxide and water. Thus, option C is correct.

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Answer:

Most metals can be drawn into a wire, while nonmetals would break apart.

Explanation:

Most of the metals can be drawn into wire without breaking because their tensile strength is high. This property of metals is known as ductility.

Non metals on the other hand do not have this ability because they are brittle and tend to break apart because their tensile strength is very low.

The examples of metals which are generally used for making wires are aluminium, iron, copper etc. and rarely gold and silver are used for making wires for expensive equipments like computers.

The true statement is that most metals can be drawn into a wire, while nonmetals would break apart. Most metals are malleable and ductile, and can conduct both heat and electricity, while nonmetals are brittle and are usually poor conductors.

The correct statement among the options given is: 'Most metals can be drawn into a wire, while nonmetals would break apart.'

Most metals are malleable and ductile, meaning they can be reshaped without breaking. That's why we can draw them into wires. On the other hand, most nonmetals are brittle and would break or shatter if you tried to draw them into a wire. Similarly, while both metals and nonmetals can be thermal insulators or conductors, it is generally true that metals are good conductors of both heat and electricity, while nonmetals are poor conductors.

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Answer:

The answer to your question is the first option

Explanation:

Just remember that to balance using this method,

first look for the elements that change their oxidation number, and

later count the number of electrons that changed,

later identify which element oxidazes and which reduces and

finally cross the number of electrons that change in each semireaction and write these numbers in the main reaction.

               2Cr⁺³ (aq) + 6Cl⁻ (aq) ⇒ 2Cr(s) + 3Cl₂ (g)

                              2                  Cr                 2

                              6                  Cl                  6

Answer:

The answer is the first option

Explanation:

Just took the test

Have a great day

Answer:

The pH is 4.76 (option C)

Explanation:

pH of a solution = TO BE DETERMNED

[sodium acetate] = 1M   ;   [acetic acid] = 1M

K = [H+] [A-] / [HA] 

K = [H+] [1] / [1] 

K = H  

pH = pK

⇒ now pH is equal to pK

⇒ The value of pK is given which is 4.76

⇒ This means the value of the pH is also 4.76

Answer:

The pH is 4.76 (option C)

Explanation:

Explanation:

pH of a solution = TO BE DETERMNED

[sodium acetate] = 1M   ;   [acetic acid] = 1M

Answer: The Oxygen will have a partial negative charge, and the hydrogen will have a partial positive charge.

Explanation:

Electronegativity is the tendency of an atom to attract a pair of electrons when forming a chemical bond. The more electronegative atom will attract the electrons more, and will have a partial negative charge, because the electrons are negatively charged. The less electronegative atom will have the electrons the other atom attracted further away from it, so it will have a partial positive charge.

Oxygen is more electronegative than hydrogen. Oxygen has a nuclear charge of 16 protons (positively charged), whereas hydrogen only has 1. As a result, the pull these 16 protons produce on the electrons will be stronger than the pull only 1 proton produces, and the electrons will be closer to the Oxygen atom.

Answer:

Most exothermic

Kl

KBr

KCl

KF

Most endothermic

Explanation:

There is the presence of the same cation in the given salts, so only anion has to be compared.

The charge density of the anion decreases from the fluoride to the iodide as size increases from fluoride to iodide. Fluoride has highest charge density because of the smallest radius in halogen family. Also, potassium fluoride would have highest lattice enthalpy because there will be greater force of attraction between them. The trend for the lattice enthalpy is:

KF>KCl>KBr>KI

Since more energy to split KF , so it will be most endothermic and so on.

So trend is:

KF is most endothermic and KI being most exothermic.

Most exothermic

Kl

KBr

KCl

KF

Most endothermic

The size of ions in an ionic compound impacts internuclear distance and lattice energy, which in turn affect the compound's enthalpy of solution. Larger ions have less lattice energy, and are less exothermic when dissolved. In a comparison of KF, KI, KBr, and KCl, KF should be most exothermic and KI, most endothermic.

In an ionic compound, the size of the ion influences the distance between the nuclei of adjacent ions, known as the internuclear distance. This relation affects the lattice energy, or the energy required to separate the ions in an ionic compound. Larger ions have a greater distance between them and thus have less lattice energy and are less exothermic when dissolved.

Given the compounds KF, KI, KBr, and KCl, their ion sizes (from fluorine to iodine) decrease moving across the periodic table. Therefore, KF should be the most exothermic and KI should be the most endothermic. Consequently, the sequence from most exothermic to most endothermic should be KF > KCl > KBr > KI.

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Answer:

C. 1.3 mol

Explanation:

PV = nRT

where P is absolute pressure,

V is volume,

n is number of moles,

R is universal gas constant,

and T is absolute temperature.

Given:

P = 121.59 kPa

V = 31 L

T = 360 K

R = 8.3145 L kPa / mol / K

Find: n

n = PV / (RT)

n = (121.59 kPa × 31 L) / (8.3145 L kPa / mol / K × 360 K)

n = (3769.29 L kPa) / (2993.22 L kPa / mol)

n = 1.26 mol

Round to two significant figures, there are 1.3 moles of gas.

Answer:

1propyl,3Ethyl,3methyl pentane

a) mass = 4.69gms b) mass = 5.5gms c) mass = 5.15gms d) mass = 5.94 gms.

Part A: Ba(s)+Cl₂(g)⇄BaCl₂(s)

Ba= 137

so,moles of Ba= 3.09g /137=0.02255 moles

so that the moles of BaCl₂

so mass= 0.02255x(137 +35.5x2)=4.69gms

Part B: CaO(s)+CO₂(g)⇄CaCO₃(s)

molar mass of Cao=40+16=56

moles=3.09/56=0.055

so ,moles of CaCO₃= 0.055

so mass= 0.055x(100)=5.5gms

Part C: 2Mg(s)+O₂(g)⇄2MgO(s)

Mg= 24 gms per mole

so ,no. of moles= 3.09 /24=0.128

so same no. of moles for MgO= 0,.128

weight=0.128x40=5.15gms

Part D: 4Al(s)+3O₂(g)⇄2Al₂O₃(s)

the molar mass of Al= 26

so,no.of moles = 3.09/26=0.1188

4moles of Al gives 2 moles of Al₂O₃

so, 0.1188 will give 0.0594 moles of Al₂O₃

weight= (26x2 +16x3) x0.0594=5.94 gms

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In the chemical reactions given, the mass of the product formed from 3.68g of the underlined reactant varies based on stoichiometry ranging from 2.98g to 3.68g for different reactions.

The subject question is related to the calculation of the mass of products in a chemical reaction using stoichiometry. Here is how you can calculate the mass for each reaction:

Part A: Ba(s)+Cl₂(g) → BaCl₂(s)
Since one mole of Ba produces one mole of BaCl2, we calculate the molar mass of BaCl2 (208.23 g/mol) and find that 3.68g of Ba will yield 3.68g of BaCl2.

Part B: CaO(s)+CO₂(g) → CaCO₃(s)
In this reaction, one mole of CaO reacts to form one mole of CaCO3. We know the molar mass of CaCo3 is 100.1 g/mol. Using stoichiometry, we calculate the mass to be 3.68g of CaCO3.

Part C: 2Mg(s)+O₂(g) → 2MgO(s)
Here, 2 moles of Mg yield 2 moles of MgO. Given that the molar mass of MgO is 40.3 g/mol, we find that 3.68g of Mg will yield 3.68g of MgO.

Part D: 4Al(s)+3O₂(g) → 2Al₂O₃(s)
In this case, 4 moles of Al yields 2 moles of Al2O3. Considering the molar ratio, we find that 3.68g of Al will produce 2.98 g of Al2O3.

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Explanation:

Atomic number of barium is 56 and its electronic configuration is [tex][Xe]6s^{2}[/tex].

Since, barium is a group 2 metal so in order to attain stability it will readily lose two electrons. Hence, barium will acquire a +2 charge and forms [tex]Ba^{2+}[/tex] ion.

On the other hand, chlorine is a group 17 element and its electronic distribution is 2, 8, 7. Hence, to attain stability it will gain one electron and forms [tex]Cl^{-}[/tex] ion.

Thus, we can conclude that charge on barium ion is +2 and charge on chlorine ion is -1.

Barium (Ba) is a second gathering component in s - the block of the occasional table. Every element in the second group always displays 2+ charge as cations. As a result, the Ba cation in BaCl2 has a 2+ charge as well. Chlorine and barium make up the inorganic salt barium chloride.

They c form an ionic bond since barium (Ba) is a metal and chlorine (Cl) is a nonmetal. An essential electrolyte found in all body fluids, chloride ion is a chlorine anion that is responsible for maintaining acid-base balance, transmitting nerve impulses, and regulating fluid in and out of cells.

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Answer:

a)  Lead

b) Below

Explanation:

a) ₂₁₀ Po⁸⁴ ⇒ α + ₂₀₈Pb⁸²

b) Acids are extremely corrosive substances, so they must be cleaned soon as possible because they can damage not only the furniture but also clothes and skin of the laboratory workers.

Before cleaning the polluted area with water, acids must be clean with towels in order to reduce the amount of acid.

The reaction between the acids and water are very explosive, they are exothermic reactions, that means that they increase the temperature of the area polluted and it can cause more damage. That's why the area must be cleaned with towel before add water.

Answer:

The gas argon does not reach a state of vibrational excitation when infrared radiation strikes this gas.

Explanation:

The dry atmosphere is composed almost entirely of nitrogen (in a volumetric mixing ratio of 78.1%) and oxygen (20.9%), plus a series of oligogases such as argon (0.93%), helium and gases of greenhouse effect such as carbon dioxide (0.035%) and ozone. In addition, the atmosphere contains water vapor in very variable amounts (about 1%) and aerosols.

Greenhouse gases or greenhouse gases are the gaseous components of the atmosphere, both natural and anthropogenic, that absorb and emit radiation at certain wavelengths of the infrared radiation spectrum emitted by the Earth's surface, the atmosphere and clouds . In the Earth's atmosphere, the main greenhouse gases (GHG) are water vapor (H2O), carbon dioxide (CO2), nitrous oxide (N2O), methane (CH4) and ozone (O3 ). There is also in the atmosphere a series of greenhouse gases (GHG) created entirely by humans, such as halocarbons (compounds containing chlorine, bromine or fluorine and carbon, these compounds can act as potent greenhouse gases in the atmosphere and they are also one of the causes of the depletion of the ozone layer in the atmosphere) regulated by the Montreal Protocol. In addition to CO2, N2O and CH4, the Kyoto Protocol sets standards regarding sulfur hexafluoride (SF6), hydrofluorocarbons (HFCs) and perfluorocarbons (PFCs).

The difference between argon and greenhouse gases such as CO2 is that the individual atoms in the argon do not have free bonds and therefore do not vibrate. As a consequence, it does not reach a state of vibrational excitation when infrared radiation strikes this gas.

Argon doesn't contribute to global warming because it's chemically inert, meaning it doesn't react with other substances or absorb heat. This is unlike carbon dioxide, a greenhouse gas that absorbs and traps heat, leading to global warming.

The explanation for why argon does not contribute to global warming, despite its relative abundance in the atmosphere, lies in its chemical nature. Unlike carbon dioxide (CO2), argon (Ar) is chemically inert, meaning it does not easily react with other elements or compounds. This property is due to its full set of electrons in its outermost shell, giving it a stable configuration.

Global warming is primarily caused by certain gases, notably CO2, that are capable of absorbing and trapping heat in the Earth's atmosphere, a phenomenon known as the greenhouse effect. When sunlight enters the Earth's atmosphere, some of it is reflected back into space, and some is absorbed by these greenhouse gases and re-emitted in all directions, warming the Earth's surface. However, argon does not participate in these interactions due to its chemical inertness. Even though it is 27 times more abundant than CO2, it does not absorb the Sun's heat and therefore does not contribute to global warming.

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Answer: The number of valence electrons in sulfur atom are 6.

Explanation:

The isotopic representation of sulfur atom is [tex]_{16}^{32}\textrm{S}[/tex]

Valence electrons are defined as the electrons that are present in the outer most orbital of an atom. Electrons present in the orbitals having highest principle quantum number are termed as valence electrons.

Sulfur is the 16th element of the periodic table having 16 electrons.

Electronic configuration of sulfur atom is [tex]1s^22s^22p^63s^23p^4[/tex]

The number of valence electrons present in sulfur atom are 2 + 4 = 6

Hence, the number of valence electrons in sulfur atom are 6.

Answer:

The answer to your question is: sugar melting point: 186°C

Explanation:

I think that Donna did an excellent suggestion. If we heat a substance till it melts, we are obtaining the melting point. This point is the temperature at which a solid changes from solid to liquid and is specific for every substance. That means that the melting point of sugar is different from the melting point of salt, etc. So, they could distinguish among the substance they have the one that is sugar.

For example:            sugar                  table salt      

Melting point            186°C                    801°C

The combustion reaction that can be identified is Al₂S₃ + 2Al + 3S and  represents the combustion of aluminum sulfide (Al₂S₃), a compound of aluminum and sulfur.

Aluminum sulfide (Al₂S₃) reacts with oxygen (O₂) from the air to form aluminum oxide (Al₂O₃) and sulfur dioxide (SO₂). Aluminum oxide (Al₂O₃) is a white, solid compound that is often formed as a byproduct of aluminum smelting. which has found applications in various industrial applications, such as ceramics, pigments, and refractories.

Sulfur dioxide (SO₂) is a colorless gas with a pungent odor and is a major air pollutant that can cause respiratory problems and acid rain. Heat is released during the combustion reaction, which can be harnessed for various purposes, such as generating electricity or powering industrial processes.

Answer:

4.18 g

Explanation:

The formula for the calculation of moles is shown below:

[tex]moles = \frac{Mass\ taken}{Molar\ mass}[/tex]

Given: For Li

Given mass = 2.50 g

Molar mass of Li  = 6.94 g/mol

Moles of Li  = 2.50 g / 6.94 g/mol = 0.3602 moles

Given: For [tex]N_2[/tex]

Given mass = 2.50 g

Molar mass of [tex]N_2[/tex] = 28.02 g/mol

Moles of [tex]N_2[/tex] = 2.50 g / 28.02 g/mol = 0.08924 moles

According to the given reaction:

[tex]6Li+N_2\rightarrow 2Li_3N[/tex]

6 moles of Li react with 1 mole of [tex]N_2[/tex]

1 mole of Li react with 1/6 mole of [tex]N_2[/tex]

0.3602 mole of Li react with [tex]\frac {1}{6}\times 0.3602[/tex] mole of [tex]N_2[/tex]

Moles of [tex]N_2[/tex] that will react = 0.06 moles

Available moles of [tex]N_2[/tex] = 0.08924 moles

[tex]N_2[/tex] is in large excess. (0.08924 > 0.06)

Limiting reagent is the one which is present in small amount. Thus,

Li is limiting reagent.

The formation of the product is governed by the limiting reagent. So,

6 moles of Li gives 2 mole of [tex]Li_3N[/tex]

1 mole of Li gives 2/6 mole of [tex]Li_3N[/tex]

0.3602 mole of Li react with [tex]\frac {2}{6}\times 0.3602[/tex] mole of [tex]Li_3N[/tex]

Moles of [tex]Li_3N[/tex] = 0.12

Molar mass of [tex]Li_3N[/tex] = 34.83 g/mol

Mass of [tex]Li_3N[/tex] = Moles × Molar mass = 0.12 × 34.83 g = 4.18 g

Theoretical yield = 4.18 g

Answer:

The balanced chemical equation for the reaction is:

6 Li + N2 → 2 Li3N

From the equation, we can see that 6 moles of Li react with 1 mole of N2 to produce 2 moles of Li3N. We can use this information and the molar masses of the elements to calculate the theoretical yield of Li3N:

Molar mass of Li: 6.94 g/mol

Molar mass of N2: 28.02 g/mol

Molar mass of Li3N: 34.83 g/mol

First, we need to calculate the number of moles of Li in the reaction:

2.50 g Li × (1 mol Li/6.94 g Li) = 0.360 mol Li

Next, we need to calculate the limiting reagent in the reaction. Since we have 0.360 moles of Li, and 1 mole of N2 is needed for every 6 moles of Li, we have:

0.360 mol Li × (1 mol N2/6 mol Li) = 0.0600 mol N2

Therefore, N2 is the limiting reagent in the reaction. We can now calculate the theoretical yield of Li3N:

0.0600 mol N2 × (2 mol Li3N/1 mol N2) × (34.83 g Li3N/1 mol Li3N) = 4.74 g Li3N

Therefore, the theoretical yield of Li3N is 4.74 g.

The maximum amount of tetraphosphorus (P4) that can be produced from 1.0 kg of 75% pure phosphorite is approximately 149.69 grams, considering the reaction with silicon dioxide and carbon in excess.

The student has asked about the amount of tetraphosphorus (P4) that can be produced from 1.0 kg of phosphorite, which is 75% calcium phosphate (Ca3(PO4)2) by mass, assuming an excess of the other reactants. In the industrial preparation of phosphorus, calcium phosphate is chemically reduced to form tetra phosphorus, which has several applications, including the manufacture of fertilizers, pesticides, and special alloys.

The first step is to calculate the mass of pure Ca3(PO4)2 available in the 1.0 kg of phosphorite. Since the phosphorite sample is 75% Ca3(PO4)2, this means there is 0.75 kg (or 750 g) of Ca3(PO4)2 present. Using the molar mass of Ca3(PO4)2 (310.18 g/mol) and the stoichiometry of the reaction, we find the corresponding moles of P4 produced.

For every 2 moles of Ca3(PO4)2 used, 1 mole of P4 is formed. Therefore, we calculate (750 g / 310.18 g/mol) / 2 = 1.208 mol of P4. To find the mass, we multiply the moles of P4 by its molar mass (123.89 g/mol), resulting in 149.69 g of P4 produced from 1.0 kg of phosphorite.

Answer:

Option b, Irreversible hydrocolloid impression material

Explanation:

Irreversible is used as an impression material to take impression from edentulous jaws. It is also used in wound healing and drug delivery.

Alginate is a natural polymer found in cell wall of brown seaweed.

Its monomers are β-D-mannuronate and α-L-guluronate.

In association with Ca2+, it forms gel. It is hydrophilic in nature.

The nucleus of an atom, discovered by Hans Geiger and Ernest Marsden in 1911 during the Gold Foil Experiment, accounts for most of the atom's mass but very little of its size. Although it contains the majority of the atom's mass, the nucleus is much smaller in size compared to the full atom.

In 1911, Hans Geiger and Ernest Marsden, under the supervision of Ernest Rutherford, conducted an experiment which is now commonly known as the Gold Foil Experiment. This experiment led to the pivotal discovery of the nucleus in atoms. In terms of size and mass, the nucleus of an atom accounts for most of the atom's mass but very little of its size (option D). The nucleus, although it contains nearly all of an atom's mass due to its protons and neutrons, is very small compared to the full size of the atom. The vast majority of the size of an atom is accounted for by the orbit of its electrons, which are extremely lightweight.

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Answer:

The borane reagent acts as a Lewis acid because it is electron-deficient.

Explanation:

The borane reagent is electron-deficient because it does not have a complete octet. Thus, it is electrophilic and accepts donation of the electrons from the alkene.

The electron deficiency of borane makes it electrophilic, driving its reactivity in the hydroboration reaction. Its eagerness to acquire electrons from the alkene initiates the process, enabling the formation of a C-B bond, which is essential in organic synthesis and serves as the basis for various chemical transformations.

The electron-deficient nature of the borane reagent plays a pivotal role in the hydroboration reaction, as it renders the borane electrophilic, ready to accept electron pairs from the alkene. This unique characteristic of borane can be attributed to its incomplete electron configuration, particularly the lack of a complete octet in its valence shell.

Borane (B2H6) is electron-deficient because boron, the central atom in borane, possesses only three valence electrons. This is in contrast to the octet rule, a fundamental principle in chemistry, which suggests that atoms tend to acquire a stable electron configuration, often characterized by eight electrons in their valence shell. Due to its deficiency of valence electrons, boron is left "wanting" more electrons to complete its octet.

The electron deficiency makes borane an electrophile, which is a species that is electron-hungry and seeks to gain additional electrons to achieve a stable electron configuration. In the hydroboration reaction, borane acts as an electrophile by accepting a pair of electrons from the pi bond of the alkene. This electron transfer results in the formation of a new carbon-boron (C-B) sigma (σ) bond, marking the initiation of the hydroboration process.

The electrophilic nature of borane, driven by its electron deficiency, allows it to participate in chemical reactions with nucleophiles, such as alkenes, where electron-rich species readily donate electron pairs. The resulting organoboron compound serves as a versatile intermediate for subsequent transformations in organic synthesis.

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Answer:

The average atomic mass of M is 181.33 g/mol.

Explanation:

First off we need to know the reaction that takes place. The balanced reaction of M₂S₃(s) is:

The important section for this problem is this:

**Thus, the number of moles of M in M₂S₃ is equal to the number of moles of M in 2MO₂.

The decrease in mass means that M₂S₃ reacted and produced MO₂, thus the mass of MO₂ is 3.280-0.228=3.052 g

Now let's say x is the atomic weight of M, and write the molecular weights (Mw) of those two compounds:

Mw of M₂S₃= 2x + 96 g/mol

Mw of MO₂= x + 32 g/mol

Now we determine the moles of each compound, using the formula [ moles = mass / molecular weight ]:

Moles of M₂S₃= [tex]\frac{3.280g}{2x+96g/mol}[/tex]

Moles of MO₂=  [tex]\frac{3.052g}{x+32g/mol}[/tex]

Using the equivalence marked by asterisks, we're left with (note that the second denominator is multiplied by 2 because of the reaction coefficients):

[tex]\frac{3.280g}{2x+96g/mol}=\frac{3.052g}{2x+64g/mol}[/tex]

We solve for x:

[tex]\frac{3.280g}{3.052g}=\frac{2x+96g/mol}{2x+64g/mol[tex]1.075*(2x+64g/mol)=2x+96g/mol\\2.150x+68.8g/mol=2x+96g/mol\\0.150x=27.2g/mol\\x=181.33g/mol[/tex]}[/tex]

Thus, the average atomic mass of M is 181.33 g/mol.

The average atomic mass of M was calculated from the mass loss during the conversion of M2S3 to MO2. It was found by comparing the moles of sulfur lost to the moles of M present and then calculating the mass per mole of M, yielding a value of 642.53 g/mol.

To determine the average atomic mass of M from the conversion of M2S3 to MO2, we begin by understanding that the loss of mass is due to the conversion of sulfur (S) in M2S3 to sulfur dioxide (SO2) in air. Given that the mass decrease is 0.228 g, this corresponds to the mass of sulfur that was converted to SO2.

Since the molar mass of sulfur is 32 g/mol, we can find the moles of sulfur that were lost:
0.228 g / 32 g/mol = 0.007125 mol of sulfur lost. Because the compound is M2S3, the loss of three moles of sulfur corresponds to two moles of M being present. Using the moles of sulfur lost, we can set up a proportion to find the moles of M:

3 moles of S : 2 moles of M
0.007125 moles of S : X moles of M

This gives us X = (2/3) * 0.007125 moles of M = 0.00475 moles of M.

The original mass of M2S3 was 3.280 g. After heating and the loss of sulfur, the remaining mass corresponds to M in the compound MO2. Therefore, we subtract the mass of sulfur lost from the original mass to find the mass of M:

Mass of M = 3.280 g - 0.228 g = 3.052 g

Finally, we can calculate the average atomic mass of M:

Average atomic mass of M = 3.052 g / 0.00475 mol = 642.53 g/mol (rounded to two decimal points)

Answer:

The question to your answer is: V2 = 78.75 l  non if the options given

Explanation:

Data

V1 = 35 l

T1 = 20 °C

T2 = 45°C

V2 = ?

Formula

V1 / T1 = V2 / T2

Clear V2 from the equation

V2 = V1T2/T1

Substitution

V2 = (35)(45) / (20)

V2 = 78.75 l

Answer:

The new volume of the balloon is 78.75 L

Explanation:

Charles's law relates the volume and temperature of an ideal gas, to a constant pressure, therefore we must use that ratio to calculate the final temperature, according to the data provided:

Vinitial = 35 L

Tinitial = 20ºC

Vfinal = ?

Tfinal = 45ºC

Vfinal = (Vinitial x Tfinal)/Tinitial = (35 L x 45ºC)/20ºC = 78.75 L

Answer:

According to decreasing viscosity = pentanol > pentanal > pentane.

surface tension =  pentanol > pentanal > pentane.

Boiling point = pentanol > pentanal > pentane.

Explanation:

pentane (CH3CH2CH2CH2CH3), pentanol (CH3CH2CH2CH2CH2OH), and pentanal (CH3CH2CH2CH2CHO) in order of decreasing viscosity, surface tension, and boiling point. They all have same sequence in which they are in order hydrogen bonding > dipole dipole interactions > van der waals dispersion forces.

Surface tension is the property of  liquid's surface that resist the force and caused by the unbalance forces. Viscosity is related to  liquid's  resistance to being moved. This is caused by the friction between molecules and Branching decreasing the boiling point.

The boiling point of the compounds pentane (C2H6), pentanol (C3H8), and pentanal (C4H10) decreases in order of pentane > pentanol > pentanal.

The boiling point of a substance is the temperature at which it changes from a liquid to a gas at a specific pressure. It is a characteristic physical property unique to each substance and depends on intermolecular forces. At the boiling point, the vapor pressure of the liquid equals the atmospheric pressure, allowing bubbles of vapor to form throughout the liquid. Water, for instance, boils at 100 degrees Celsius (212 degrees Fahrenheit) at sea level.

Thus, as per the given elements, they can be orderly arranged as - C2H6 < C3H8 < C4H10. All of these compounds are nonpolar and only have London dispersion forces: the larger the molecule, the larger the dispersion forces and the higher the boiling point.

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Answer:

The answer to your question is: Alkyl halide

Explanation:

Ether: is a functional group in which an oxygen is attached to two alkyl or aryl groups.

                   R ---  O --- R'        

Alcohol: is a functional group which has one or more hydroxyl group in its structure.

                  R ---- OH

Alkyl halide: is a group in which one or two hydrogens are replaced by halogens.

                  R --- X      X = halogen

Carbonyl group: is a structure in which one carbon is double-bounded to one oxygen

                       R --- C = O

                                |

                               R'    

Answer:

Alkyl halide is the right answer

Answer:

There is used 201,655 grams CaCl2 and 448,845 grams of water (H2O)

Explanation:

w% = m(CaCl2) / m(total) x 100%

-> (m(Cacl2) = m(total) x w% ) / 100 %  

-> m(CaCl2) = (650,5g x 31%) / 100%  = 201,655g

Total mass : m(total) = m(CaCl2) + m(H2O)

-> m(H2O) = m(total) - m(CaCl2)

->m(H2O) = 650,5g - 201,655g  = 448,845g

Answer : The molecular formula of a compound is, [tex]CHCl_3[/tex]

Solution :

If percentage are given then we are taking total mass is 100 grams.

So, the mass of each element is equal to the percentage given.

Mass of C = 0.1006 g

Mass of H = 0.0084 g

Mass of Cl = 0.8910 g

Molar mass of C = 12 g/mole

Molar mass of H = 1 g/mole

Molar mass of Cl = 35.5 g/mole

Step 1 : convert given masses into moles.

Moles of C = [tex]\frac{\text{ given mass of C}}{\text{ molar mass of C}}= \frac{0.1006g}{12g/mole}=0.0084moles[/tex]

Moles of H = [tex]\frac{\text{ given mass of H}}{\text{ molar mass of H}}= \frac{0.0084g}{1g/mole}=0.0084moles[/tex]

Moles of Cl = [tex]\frac{\text{ given mass of Cl}}{\text{ molar mass of Cl}}= \frac{0.8910g}{35.5g/mole}=0.0251moles[/tex]

Step 2 : For the mole ratio, divide each value of moles by the smallest number of moles calculated.

For C = [tex]\frac{0.0084}{0.0084}=1[/tex]

For H = [tex]\frac{0.0084}{0.0084}=1[/tex]

For Cl = [tex]\frac{0.0251}{0.0084}=2.98\approx 3[/tex]

The ratio of C : H : Cl = 1 : 1 : 3

The mole ratio of the element is represented by subscripts in empirical formula.

The Empirical formula = [tex]C_1H_1Cl_3=CHCl_3[/tex]

The empirical formula weight = 1(12) + 1(1) + 3(35.5) = 119.5 gram/eq

Now we have to calculate the molecular formula of the compound.

Formula used :

[tex]n=\frac{\text{Molecular formula}}{\text{Empirical formula weight}}[/tex]

[tex]n=\frac{119.6}{119.5}=1[/tex]

Molecular formula = [tex](CHCl_3)_n=(CHCl_3)_1=CHCl_3[/tex]

Therefore, the molecular of the compound is, [tex]CHCl_3[/tex]

The molecular formula of the compound is C4H2Cl4 (carbon tetrachloride).

To find the molecular formula of the compound, we need to determine the empirical formula first. The empirical formula represents the simplest whole number ratio of the elements present in a compound. We can calculate the empirical formula by converting the percentages of the elements to moles and finding the mole ratios.

In this case, the compound contains 10.06% carbon, 89.10% chlorine, and 0.84% hydrogen. Assuming a 100g sample, we have 10.06g of carbon, 89.10g of chlorine, and 0.84g of hydrogen. Converting these masses to moles, we find that the mole ratio is approximately 0.835 moles of carbon, 2.517 moles of chlorine, and 0.835 moles of hydrogen.

The molecular formula can then be determined by comparing the experimental molar mass (119.6 g/mol) with the empirical formula mass. Given that the empirical formula mass is 2*(12.01g/mol) + 35.45g/mol + 2*(1.01g/mol) = 62.02 g/mol, we can divide the experimental molar mass by the empirical formula mass to find the whole number ratio. The ratio is approximately 1.93, which can be rounded to 2.

Therefore, the molecular formula of the compound is C4H2Cl4 (carbon tetrachloride).

Answer:

First of all you need to know that chemical properties are those who are determined by chemical tests and are related to the reactivity of chemical substances. In those statements you have 4 reactions, except on "conducts electricity". That is a physical property.

Explanation:

A chemical reaction is a way in which the atoms of the elements regroup to form new substances.

Final answer:

Conducts electricity is a physical property and not a chemical property. Chemical properties are those that can only be observed when a substance undergoes a chemical change to become a different substance.

Explanation:

Among the options provided, the only feature that is not a chemical property is conducts electricity, as this is a physical property related to the substance's ability to allow the passage of electric current, which can be observed without changing the identity of the substance. Chemical properties, on the other hand, involve the substance's ability to undergo a chemical change. For example, reacting with oxygen to produce a white flame, turning green when dissolved in water, giving off brown fumes when treated with nitric acid, and reacting with chlorine are all indicative of chemical changes because they result in the formation of new substances with different compositions.

Answer:

The answer to your question is:  C2 = 0.0004 M

Explanation:

Data

pH = 2.5; V = 1.0 L

V2 = 8.0 L  C2 = ?

Formula

C1V1 = C2V2

C2 = C1V1 / V2

pH = -log[H⁺]

Process

[H⁺] = antilog -pH

[H⁺] = antilog (-2.5)

[H⁺] = 0.003 M = C1

Finally

                          (0.003)(1 l) = C2(8)

                           C2 = 0.003 / 8

                           C2 = 0.0004 M

Answer : The value of [tex]K_c[/tex] at this temperature is 0.0184

Explanation : Given,

Concentration of [tex]HI[/tex] at equilibrium = [tex]3.51\times 10^{-3}M[/tex]

Concentration of [tex]H_2[/tex] at equilibrium = [tex]4.76\times 10^{-4}M[/tex]

Concentration of [tex]I_2[/tex] at equilibrium = [tex]4.76\times 10^{-4}M[/tex]

The given equilibrium reaction is,

[tex]2HI(g)\rightleftharpoons H_2(g)+I_2(g)[/tex]

The expression of [tex]Kc[/tex] will be,

[tex]K_c=\frac{[H_2][I_2]}{[HI]^2}[/tex]

Now put all the given values in this expression, we get:

[tex]K_c=\frac{(4.76\times 10^{-4})\times (4.76\times 10^{-4})}{(3.51\times 10^{-3})^2}[/tex]

[tex]K_c=0.0184[/tex]

Therefore, the value of [tex]K_c[/tex] at this temperature is 0.0184

Final answer:

The equilibrium constant, Kc, for the decomposition of gaseous hydrogen iodide into hydrogen and iodine at 425°C, given the concentrations at equilibrium, is calculated as 1.84×10⁻².

Explanation:

The question asks about the calculation of the equilibrium constant, Kc, for the decomposition of hydrogen iodide into hydrogen and iodine at 425°C. The provided concentrations at equilibrium are [HI] = 3.51×10⁻³ M, [H₂]= 4.76×10⁻⁴ M, and [I₂]= 4.76×10⁻⁴ M.

To find Kc, we use the expression Kc = [H₂][I₂]/[HI]². Plugging in the given values:

Kc = (4.76×10⁻⁴ M)×(4.76×10⁻⁴ M) / (3.51×10⁻³ M)²

Kc = (2.26×10⁻⁷ M²) / (1.23×10⁻⁵ M²)

Kc = 1.84×10⁻²

To express Kc to three significant digits, Kc = 1.84×10⁻².