Vinegar is composed of approximately 5% acetic acid and 95% water. Which one of the following is the best classification of vinegar?A. pure substance B. element C. compound D. mixture

Answer:

Mg₃N₂ + 6H₂O  →  2NH₃  +  3Mg(OH)₂

Coefficient of water is 6 (option 3)

Explanation:

The reaction is:

Mg₃N₂ + H₂O  →  NH₃  +  Mg(OH)₂

Let's balance the reaction.

In reactant side we have 3 Mg, therefore in product side, we add 3 Mg to the hydroxide.

This change, modified the hydroxide, so now we have 6 O and 6 H, but we have in total 9 H (6 from the hydroxide + 3 from the ammonia)

As we have 2N, in reactant side, we must add 2 N to the ammonia, so now

we have 12 H in product side . We must complete with 6, the water so the H are ballanced.

In reactant side we have 6 O, therefore in product we must have 6 O (two O, in the OH but we have 3 moles, so in total we have 6 O) - BALANCED

The balance reaction is:

Mg₃N₂ + 6H₂O  →  2NH₃  +  3Mg(OH)₂

The chemical reaction of magnesium nitride with water to form ammonia and magnesium hydroxide has a coefficient of 6 for water in the balanced equation.

Preparing ammonia through the reaction of magnesium nitride with water yields ammonia and magnesium hydroxide. The balanced chemical equation for this reaction is: Mg3N2 + 6H2O → 3NH3 + 3Mg(OH)2. Thus, the coefficient of water in the balanced chemical equation is 6, which corresponds to option number 3 in your question.

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Answer:

The answer is D

Explanation:

Law of Definite Proportions states that a given compound always contain its component elements in fixed ratio (by mass) and does not depend on its source and/or method of preparation.  

If one is to explain the law of definite proportions properly, then Dalton's fourth atomic theory comes to mind which states that atoms chemically combine with other atoms in fixed, whole number ratios.

The law of definite proportions suggests that compounds always contain its component elements in fixed ratio no matter the source, for example, oxygen makes up 8/9 of the mass of the sample of pure water regardless of the source while hydrogen makes up the remaining 1/9 of the mass. This generally shows that when oxygen and hydrogen combine in the ratio 8:1, water molecule will be formed as suggested by the Dalton Atomic Theory.

The Dalton's atomic theory postulate explaining the Law of Definite Proportions is 'Atoms chemically combine with other atoms in fixed, whole-number ratios.' This principle underlies consistent elemental proportions in compounds, such as the 1:8 ratio of hydrogen to oxygen in water.

The postulate of Dalton's atomic theory that is vital to explain the observations summarized by the Law of Definite Proportions is: 'Atoms chemically combine with other atoms in fixed, whole-number ratios.'

This is crucial because the Law of Definite Proportions states that a given compound, regardless of the source or preparation method, will always consist of the same elements in the same proportion by mass.

For example, water (H2O) is always composed of 2 hydrogen atoms and 1 oxygen atom (fixed, whole-number ratio) regardless of the source. In water, the ratio of the mass of hydrogen to oxygen is always 1:8, which corroborates the Law of Definite Proportions.

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HF and CH3OH exhibit dipole-dipole forces when dissolved in water because they both can form hydrogen bonds. CaCl2 and FeBr3 display ion-dipole forces in water because they are ionic compounds.

When these substances are added to water, they exhibit different solute-solvent interactions due to their different properties.

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Answer: 2,625.3 g AlCl3

Explanation: solution attached:

First balance the chemical equation then do basic stoichiometry.

Answer:

Gastric juices have a pH of 1 or 2. This would indicate numerous H+ ions and a low pH

Explanation:

Highers concentrations of [H⁺] means very low pH.

pH = - log [H⁺]

Imagine this two concentrations:

[H⁺]₁ = 0.2 M

[H⁺]₂ = 0.0006 M

[H⁺]₁ > [H⁺]₂

pH₁ = - log 0.2 → 0.70

pH₂ = - log 0.0006 → 3.22

Then pOH₁ = 14 - 0.70 = 13.30

pOH₂ = 14 - 3.22 = 10.78

[OH⁻]₁ = 10^-pOH = 5.01×10⁻¹⁴

[OH⁻]₂ = 10^-pOH = 1.66×10⁻¹¹

As pH is so low, [OH⁻] is more and more lower.

Answer:

a) 0.67 moles of O2

b) 1.34 moles H2O

c) 24.15 grams of H2O

d) 21.44 grams O2

Explanation:

Step 1: Data given

Dihydrogen dioxide = H2O2

oxygen gas = O2

Moles H2O2 = 1.34 moles

Molar mass of H2O2 = 34.01 g/mol

Step 2: The balanced equation

2H2O2 → 2H2O + O2

Step 3: Calculate moles of H2O formed

For 2 moles H2O2 we'll have 2 moles H2O produced

For 1.34 moles H2O2 we have 1.34 moles H2O produced

This is 1.34 moles * 18.02 g/mol = 24.15 grams of H2O

Step 4: Calculate moles of O2 formed

For 2 moles H2O2 we'll have 1 mol O2 produced

For 1.34 moles H2O2 we'll have 1.34 /2 = 0.67 moles of O2 produced

This is 0.67 moles * 32.00 g/mol = 21.44 grams O2

Answer:

Partia pressure N₂ → 0.975 atm

Explanation:

Let's analyse the moles fractions:

N₂ → 0.25

O₂ → 0.65

He → 0.1

Partial pressure / Total pressure = Mole fraction

Partial pressure N₂ / 3.9 atm = Mole fraction N₂

Partial pressure N₂ / 3.9 atm = 0.25

Partial pressure N₂ = 3.9 atm . 0.25 → 0.975 atm

The pressure of nitrogen in the mixture has been 0.975 atm.

Partial pressure has been defined as the pressure exerted by the gas molecules in the mixture. The partial pressure ([tex]P_A[/tex])  has been expressed as:

[tex]P_A=X_A\;\times\;P[/tex]

Where,  Mole fraction of the element A, [tex]X_{N_2}=0.25\;\rm atm[/tex]

The total pressure of the mixture, [tex]P=3.9\;\rm atm[/tex]

Substituting the values, the pressure of nitrogen ([tex]P_{\rm N_2}[/tex]),

[tex]P_{\rm N_2}=0.25\;\times\;3.9\;\rm atm\\ \textit P_{N_2}=0.975\;atm[/tex]

The pressure of nitrogen in the mixture has been 0.975 atm.

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Answer:

4. 1; 6; 2 — synthesis

Explanation:

Decomposition reaction is defined as the reaction in which a single large substance breaks down into two or more smaller substances.

[tex]AB\rightarrow A+B[/tex]

Single displacement reaction is defined as the reaction in which more reactive element displaces a less reactive element from its chemical reaction.

The reactivity of metal is determined by a series known as reactivity series. The metals lying above in the series are more reactive than the metals which lie below in the series.

[tex]A+BC\rightarrow AC+B[/tex]

Synthesis reaction is defined as the reaction in which smaller substances combine in their elemental state to form a larger substance.

[tex]A+B\rightarrow AB[/tex]

The unbalanced combustion reaction is shown below as:-

[tex]P_4+Ca\rightarrow Ca_3P_2[/tex]

On the left hand side,  

There are 4 phosphorus atoms and 1 calcium atom

On the right hand side,  

There are 2 phosphorus atoms and 3 calcium atoms

Thus,  

Right side, [tex]Ca_3P_2[/tex] must be multiplied by 2 to balance phosphorus.

Left side, [tex]Ca[/tex] is multiplied by 6 so to balance the whole reaction.

Thus, the balanced reaction is:-

[tex]P_4+6Ca\rightarrow 2Ca_3P_2[/tex]

Thus, answer:- 4. 1; 6; 2 — synthesis

Answer: B

Double replacement reaction

Explanation:

Answer:

224 grams of O₂

Explanation:

This is the reaction:

2 C₂H₆ (g) + 7 O₂(g) → 4 CO₂ (g) + 6 H₂O (g)

2 moles of ethene react with 7 moles of oxygen.

Let's convert the ethene's mass into moles (mass / molar mass)

60 g / 30 g/m = 2 mol

So, if 2 moles of ethene must react with 7 moles of O₂ and we have 2 moles, obviously we would need 7 moles of oyxgen.

Let's convert the moles to mass ( mol . molar mass)

7 m . 32 g/m = 224 grams

Answer: Mass of O2 is 224g

Explanation:

From the equation of the reaction, Ethane to oxygen is 2 to 7

While the molar masses respectively gives 30 and 32 g/mol

2 moles of methane gives 7 moles of O2;

60g/30=2moles for methane gives x/32 for O2;

Cross multiplying yields

7 x 2 = 2 x mass of O2/32

14 = 2x/32

Final answer gives 224 grams of oxygen

Answer:

(a). Biological fixation

(b). Fixation by lightning

Explanation:

Gaseous nitrogen in the atmosphere has to be converted or "fixed" into a suitable form before it can be utilised by living organisms.

There two main ways of nitrogen fixation are

(a). Biological fixation: Majority (approximately 90%) of nitrogen fixation is carried out by bacteria. Bacterias such as Cyanobacteria transforms nitrogen into ammonium and ammonia : N2 + 3 H2 → 2 NH3. The produced ammonia can then be taken in directly by plants and /or the conversion products of ammonium and ammonia may further react in the process of nitrification.

(b). Fixation by lightning: Lightning energy causes the combination nitrogen (N2) and water (H2O) forming nitrates (NO3) and ammonia (NH3) . Rain water dissolves the formed nitrates and ammonia and the solution is drained into the ground, where they can be reached by plants plant roots for consumption.

Biological nitrogen fixation and lightning are the major natural processes responsible for converting atmospheric nitrogen to useable forms.

Nitrogen gas goes into the soil from the atmosphere, and nitrogen fixing bacteria convert this nitrogen to ammonium ions (NH4+), which can be used by plants.

Whereas, Lightning converts atmospheric nitrogen into ammonia and nitrate (NO3) that comes to the soil with the help of rainfall.

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Answer:

C₃H₈  +  5O₂  →  3CO₂  +  4H₂O

Option D.

Explanation:

This is a combustion reaction, where a compound reacts with oxygen to produce CO₂ and water.

You have to look at the reactants and the products.

C₃H₈  +  O₂  →  CO₂  +  H₂O

To balance you must have the same atoms of each elements in both sides.

Actually we have 3 C, 8 H and 2 O in reactant side and 1 C, 3 O and 2H in product side.

We can add 4 to water to have 8 H in product side to balance the H with reactants but we modified the amount of oxygens. Now, we have 4 O in water and 2 O from CO₂ (6 in total).

In reactant side, we have 3 C, therefore we add 3 to CO₂ and now, we have 3 C on both sides and 8 H in both sides, so, as in product side we have 10 O, 6 from CO₂ and 4 from water, we must add a 5 to balance in reactant side.  The balance equation will be:

C₃H₈  +  5O₂  →  3CO₂  +  4H₂O

Answer:

B. 0.075 m (NH4)3PO4

Explanation:

Our strategy here is to recall the van´t Hoff factor, i, for the colligative properties of electrolyte solutions which appears as the consequence that electrolytes disociate completely in their solutions in water.

Thus in this problem we need to determine i and then realize the one with the lowest freezing point will have the biggest  i ( all the concentrations are equal) since

ΔTf = i m Kf

Substance  van´t Hoff factor

Li I                             2

(NH4)3PO4              4

NaIO4                       2

KCN                          2

KNO2                       2

The correct answer is B. 0.075 m (NH4)3PO4

The aqueous solution with the lowest freezing point is 0.075 m (NH4)3PO4 because it dissociates into the highest number of particles, leading to the greatest freezing point depression.

To find the aqueous solution with the lowest freezing point, we need to determine the effective concentration of solute particles after dissociation. Freezing point depression is larger for solutions with a higher number of dissolved particles. Therefore, we must consider the van't Hoff factor (i), which is the number of particles a compound dissociates into in solution. For example, LiI (i=2), NaIO4 (i=1), and KCN (i=2) will produce fewer particles than (NH4)3PO4, which will dissociate into four particles (i=4).

Given that the molal concentrations (m) are the same, the solution with the highest van't Hoff factor will have the highest concentration of particles and therefore, the lowest freezing point. Hence, solution B, 0.075 m (NH4)3PO4, with an effective concentration of 0.3 m (0.075 m × 4), will have the lowest freezing point.

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Answer:

sorry i cant read sideways

Explanation:

Answer: The final pressure in the vessel will be 0.965 atm

Explanation:

To calculate the number of moles, we use the equation:

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

Given mass of phosphorus trichloride = 20.0 g

Molar mass of phosphorus trichloride = 137.3 g/mol

Putting values in equation 1, we get:

[tex]\text{Moles of phosphorus trichloride}=\frac{20.0g}{137.3g/mol}=0.146mol[/tex]

Given mass of oxygen gas = 3.15 g

Molar mass of oxygen gas = 32 g/mol

Putting values in equation 1, we get:

[tex]\text{Moles of oxygen gas}=\frac{3.15g}{32g/mol}=0.098mol[/tex]

The chemical equation for the reaction of phosphorus trichloride and oxygen gas follows:

[tex]2PCl_3+O_2\rightarrow 2POCl_3[/tex]

By Stoichiometry of the reaction:

2 moles of phosphorus trichloride reacts with 1 mole of oxygen gas

So, 0.146 moles of phosphorus trichloride will react with = [tex]\frac{1}{2}\times 0.146=0.073mol[/tex] of oxygen gas

As, given amount of oxygen gas is more than the required amount. So, it is considered as an excess reagent.

Thus, phosphorus trichloride is considered as a limiting reagent because it limits the formation of product.

By Stoichiometry of the reaction:

2 moles of phosphorus trichloride produces 2 moles of [tex]POCl_3[/tex]

So, 0.146 moles of phosphorus trichloride will produce = [tex]\frac{2}{2}\times 0.146=0.146mol[/tex] of [tex]POCl_3[/tex]

To calculate the pressure of the vessel, we use the equation given by ideal gas follows:

[tex]PV=nRT[/tex]

where,

P = pressure of the vessel = ?

V = Volume of the vessel = 6.00 L

T = Temperature of the vessel = [tex]210^oC=[210+273]K=483K[/tex]

R = Gas constant = [tex]0.0821\text{ L. atm }mol^{-1}K^{-1}[/tex]

n = number of moles = 0.146 moles

Putting values in above equation, we get:

[tex]P\times 6.00L=0.146mol\times 0.0821\text{ L atm }mol^{-1}K^{-1}\times 483K\\\\P=\frac{0.146\times 0.0821\times 483}{6.00}=0.965atm[/tex]

Hence, the final pressure in the vessel will be 0.965 atm

Answer:

The final pressure in the vessel is 1.13 atm

Explanation:

Step 1: Data given

Volume of the vessel = 6.00 L

Mass of PCl3 = 20.0 grams

Mass of O2 = 3.15 grams

Temperature = 15.0 °C

The vessel is heated to 210°C

Molar mass of PCl3 = 137.33 g/mol

Step 2: The balanced equation

2PCl3 + O2 → 2POCl3

Step 3: Calculate moles PCl3

MolesPCl3 = mass PCl3 / molar mass PCl3

Moles PCl3 = 20.0 grams / 137.33 g/mol

Moles PCl3 =0.146 moles PCl3

Step 4: Calculate moles O2

Moles O2 = 3.15 grams/ 32.0 g/mol

Moles O2 = 0.0984 moles O2

Step 5: Calculate the limiting reactant

PCl3 is the limiting reactant. It will completely be consumed(0.146 moles). So at completion there is no PCl3 remaining.

O2 is in excess. There will react 0.146/2 = 0.073 moles. There will remain 0.0984 - 0.073 = 0.0254 moles O2

Step 6: Calculate moles POCl3

For 2 moles PCl3 we need 1 mol O2 to produce 2 moles POCl3

For 0.146 moles PCl3 we'll have 0.146 moles POCl3

Step 7: Calculate final pressure

p*V = n*R*T

p = (n*R*T)/V

⇒ with n = the number of moles = 0.146 moles of POCl3 produced + 0.0254 moles O2 remaining = 0.1714 moles gas

⇒ with R = the gas constant = 0.08206 L*atm/mol*K

⇒with T = the temperature = 210 +273 = 483 Kelvin

⇒ with V = the volume = 6.00 L

p = (0.1714 *0.08206 * 483) / 6.00

p = 1.13 atm

The final pressure in the vessel is 1.13 atm

Answer: only H2O is a compound

Explanation:

Answer:

The value of Kp is 4

Explanation:

Step 1: Data given

The initial pressure of N2 = 1 atm

The initial pressure of  H2 = 2 atm

Temperature = 200 °C

At equilibnrium, the toal pressure is 2 atm

Step 2: The balanced equation

N2(g) + 3H2(g) → 2NH3(g)

Step 3: The initial pressures

N2 = 1.0 atm

H2 = 2.0 atm

NH3 = 0 atm

Step 4: The partial pressures at equilibrium

For 1 mol N2 we need 3 moles H2 to produce 2 moles NH3

There will react X moles of N2,

There will react 3X moles of H2

There will be produced 2X moles NH3

The partial pressure of N2 at the equilibrium is (1.0 -X)atm

The partial pressure of H2 at the equilibrium is (2.0 - 3X)atm

The partial pressure of NH3 at the equilibrium is 2X

The total pressure at the equilibrium = 2.0 atm

The total pressure = pN2 + pH2 +pNH3 = 2.0 atm

2.0 atm = (1.0-X) + (2.0 - 3X) + 2X

2.0 =3.0 -2X

X = 0.50

The partial pressure of N2 at the equilibrium is (1.0 -0.50) = 0.50 atm

The partial pressure of H2 at the equilibrium is (2.0 - 3*0.5) = 0.50 atm

The partial pressure of NH3 at the equilibrium is 2*0.5 = 1.0 atm

Step 5: Calculate Kp

Kp = pNH3 / (pN2)*(pH2)

Kp = 1.0 / (0.5*0.5)

Kp = 4

The value of Kp is 4

Answer:

1. Reduce

2. Oxidize

3. Oxidize

4. Reduce

5. Oxidize

6. Reduce

Explanation:

Answer:

1. Reduce, Oxidize

2.Oxidize, reduce

3.Reduce, Oxidize

Explanation:

Answer:

covalent bond

Explanation:

Covalent bond -

It is the type of interaction observed between two species , which share the electrons in order to attain stability , is referred to as covalent bond.

The shared electrons are referred to as the bonding pairs or the shared pairs .

Stability and completion of the octet is the driving force for the formation covalent bond.

The molecules of the organic compound usually shows this type bonding .

Like the bonds between - carbon , oxygen and hydrogen are covalent bonds.

Answer:

Na+ is the most plentiful positively charged ion outside the cell, while K+ is the most plentiful inside.

Explanation:

Sodium ion and potassium ion play an important role in cellular metabolism. Na+ ion present in extracellular fluid while K+ ion is present in intracellular fluid.

Sodium ions are necessary for:

generation of nerve impulse

Heart activities

electrolyte balance

High or low concentration of sodium affects health.

Potassium ions are necessary for:

fluid and electrolyte balance

Na+ ion present in extracellular fluid while K+ ion is present in intracellular fluid.

Therefore, Na+ ion present in extracellular fluid while K+ ion is present in intracellular fluid.

The correct statement is that Na+ is the most plentiful positively charged ion outside the cell, while K+ is more plentiful inside, due to the function of the sodium-potassium pump in the plasma membrane of cells.

The statement that is true among the given options is: Na+ is the most plentiful positively charged ion outside the cell, while K+ is the most plentiful inside. This arrangement is made possible through a process called the sodium-potassium pump, which is part of the plasma membrane of cells. The pump uses ATP to move 3 Na+ out of the cell and 2 K+ into the cell, which helps maintain the cell's resting potential. Therefore, outside of the cells, there is a higher concentration of Na+ ions, while inside the cells, K+ ions are more plentiful.

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Answer:

A. increases

Explanation:

According to the Gay-Lussac's law:-

Thus, at constant volume and number of moles, Pressure of the gas is directly proportional to the temperature of  the gas.

P ∝ T

Also,  it can be written as:-

[tex]\frac {P_1}{T_1}=\frac {P_2}{T_2}[/tex]

Thus, if the temperature is increased, the pressure exerted by the gas also increases.

Answer:

The correct answer is option b.

Explanation:

Average atomic mass of an element is defined as the sum of masses of each isotope each multiplied by their natural fractional abundance.

Formula used to calculate average atomic mass follows:

[tex]\text{Average atomic mass }=\sum_{i=1}^n\text{(Atomic mass of an isotopes)}_i\times \text{(Fractional abundance})_i[/tex] .....(1)

We are given:

Mass of isotope X-28 = 27.979 amu

Percentage abundance of isotope X-28 = 92.21%

Fractional abundance of isotope X-28 = 0.9221

Mass of isotope X-29 = 28.976 amu

Percentage abundance of isotope X-29 = 4.70%

Fractional abundance of isotope X-29 = 0.047

Mass of isotope X-30= 29.974 amu

Percentage abundance of isotope X-30 = 3.09%

Fractional abundance of isotope X-30 = 0.0309

Putting values in equation 1, we get:

[tex]\text{Average atomic mass of X}=\sum[(27.979 amu\times 0.9221)+(28.976 amu\times 0.047)+(29.974 amu\times 0.0309)][/tex]

[tex]\text{Average atomic mass of X}=28.09 amu[/tex]

The atomic weight of X is 28.09 amu.

The atomic weight of element X is calculated by considering the masses and abundances of its isotopes. By multiplying each isotope's mass by its abundance and summing up the products, the atomic weight of X can be determined to be 28.985 amu. Closest option to answer is option a.

The atomic weight of an element is calculated by taking into account the masses and abundances of its isotopes. In this case, element X exists in three isotopic forms with different masses and abundances. To calculate the atomic weight of X, we multiply the mass of each isotope by its abundance and sum up the products.

(27.979 amu * 0.9221) = 25.699 amu

(28.976 amu * 0.047) = 1.361 amu

(29.974 amu * 0.0309) = 0.925 amu

Summing up the products:

25.699 amu + 1.361 amu + 0.925 amu = 28.985 amu

Therefore, the atomic weight of X is 28.985 amu.

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Answer:

72.53% is the yield of CrCl3

Explanation:

Given

Reaction:

Cr2O3(s) + 3 CCl4(l) → 2 CrCl3(s) + 3 COCl2(aq)

CCl4 is in excess and 17.6g  Cr2O3 present

The reaction yields 26.6g of CrCl3

To Find:

% yields of the reaction

Also given

Molar mass of CrCl3 = 158.35g/mol

Molar mass of Cr2O3 = 152.00 g/mol

By the stoichiometry of the reaction

1 mole of Cr2O3 gives  2 moles of CrCl3

0r

1 x1 52 g of Cr2O3 gives 2x 158.35 g of CrCl3

= 1 52 g of Cr2O3 gives 316.70 g of CrCl3

    17.6 g of Cr2O3 gives  (17.6÷152) × 316.70 g CrCl3

= 36.67 g CrCl3

but actual yield is only 26.6g

so % yield is (26.6 ÷÷ 36.67) × 100

= 72.53% is the yield of CrCl3

Final answer:

To calculate the percent yield, the number of moles of chromium(III) oxide used was first determined, which was then used to find the theoretical yield of chromium chloride. The actual yield of chromium chloride is compared to this theoretical yield to find that the percent yield of the reaction is approximately 72.48%.

Explanation:

The student asked to calculate the percent yield of a chemical reaction involving chromium(III) oxide (Cr2O3) and carbon tetrachloride (CCl4). To find the percent yield, we need to compare the actual yield to the theoretical yield. First, we calculate the number of moles of Cr2O3 that react. With a molar mass of 152.00 g/mol, 17.6 g of Cr2O3 is equivalent to 0.1158 moles. According to the stoichiometry of the balanced equation, 1 mole of Cr2O3 produces 2 moles of CrCl3, which suggests that 0.1158 moles of Cr2O3 would yield 0.2316 moles of CrCl3. Using the molar mass of CrCl3 (158.35 g/mol), the theoretical yield of CrCl3 can be found as 0.2316 moles × 158.35 g/mol = 36.7 g.

Now, we calculate the percent yield using the actual yield (26.6 g) and the theoretical yield (36.7 g).

Percent Yield = (Actual Yield / Theoretical Yield) × 100 = (26.6 g / 36.7 g) × 100 ≈ 72.48%

Therefore, the percent yield of chromium chloride in the reaction is approximately 72.48%.

Answer:

The answer to your question is a heterogeneous mixture

Explanation:

The Matter is classified as Pure substances and Mixtures

Pure substances are elements or compounds which are not mixed with more substances.

Mixtures are several elements or compounds together, mixtures can be homogeneous or heterogeneous.

Homogeneous mixtures are when the different components can be identified.

Heterogeneous mixtures are when the different components can be identified just by looking at the mixture.

In concrete we can identify the different components like gravel, sand, crushed rocks, etc, so concrete is a heterogeneous mixture.

Answer:

He have higher pressure at room temperature.

Explanation:

It is given that both the gases are kept in 5 L chambers.

Therefore, volume is constant.

Also, they both are at room temperature, so temperature is also constant.

Now, number of moles of [tex]O_2[/tex] = [tex]\dfrac{Given\ mass}{Molecular \ mass}=\dfrac{5}{32}=0.16\ mol.[/tex]

Also, number of moles of He =[tex]\dfrac{Given\ mass}{Molecular \ mass}=\dfrac{5}{4}=1.25\ mol.[/tex]

Now, according to GAS LAW,

[tex]PV=nRT[/tex]  ( all terms have their usual meaning).

In this case, V, R and T are constant.

So, pressure is directly proportional to n i.e number of moles.

So, moles of He is more than moles of [tex]O_2[/tex].

Therefore, He have higher pressure at room temperature.

Hence , this is the required solution.

The gas that has a higher pressure is He.

Number of moles of oxygen gas = 5.00 g /32 g/mol = 0.156 moles

From PV = nRT

P = ?

V = 5 L

n =  0.156 moles

T = 25 + 273 = 298 K

R = 0.082 atmLK-1mol-1

P = nRT/V

P =  0.156 moles × 0.082 atmLK-1mol-1 × 298 K/5 L

P = 0.76 atm

Number of moles of He = 5/4 g/mol = 1.25 moles

P = ?

V = 5 L

n = 1.25 moles

T = 25 + 273 = 298 K

R = 0.082 atmLK-1mol-1

P = nRT/V

P =1.25 moles × 0.082 atmLK-1mol-1 × 298 K/5 L

P = 6.11 atm

The gas that has a higher pressure is He.

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Answer:

HA +  KOH  →  KA  +  H₂O

Explanation:

The unknown solid acid in water can release its proton as this:

HA  +  H₂O  →  H₃O⁺  +  A⁻

As we have the anion A⁻, when it bonded to the cation K⁺, salt can be generated, so the reaction of HA and KOH must be a neutralization one, where you form water and a salt

HA +  KOH  →  KA  +  H₂O

It is a neutralization reaction because H⁺ from the acid and OH⁻ from the base can be neutralized as water

Answer:

Explanation:

Because most of the volume occupied by the substance is empty space.

Answer:

Option 5. 21.7 %

Explanation:

Let's think the reaction:

2Al (s) + 6HCl (l) → 3H₂ (g) + AlCl₃ (aq)

We have the data of hydrogen, we formed so let's apply the Ideal Gases Law equation to solve the amount of gas.

P . V = n . R . T

1.03 atm . 1.53L = n . 0.082 L.atm . 298K

(1.03 atm . 1.53L) / (0.082 L.atm . 298K) = n → 0.0645 moles of H₂

In the reaction, 3 moles of H₂ are produced by 2 moles of Al. Let's determine, how many moles of Al produced, the 0.0645 moles of H₂.

3 moles of H₂ were produced by 2 moles of Al

Then, 0.0645 moles of H₂ would be produced by (0.0645 .2)/3 = 0.043 moles.

If we convert the moles to mass, we can know the mass of Al in the alloy. (mol . molar mass)

0.043 m . 26.98 g/mol = 1.16 g

As the sample had a mass of 5.34 g, let's determine the % of Al.

(1.16 g / 5.34 g) . 100 = 21.7%

Answer:

Proton: m= 1.6726x10⁻²⁷ kg

Neutron: m= 1.6749x10⁻²⁷ kg

Electron: m= 9.1164x10⁻³¹ kg

Explanation:

We can calculate the mass of a proton, neutron, and electron using the following data:

mass of proton: 1.00728 amu

mass of neutron: 1.00867 amu

mass of electron: 5.49x10⁻⁴ amu

1 amu = 1.66054x10⁻²⁷ kg

Now, the mass of a proton, neutron, and electron in kilograms can be calculated using the next relation:

[tex] m = 1.66054 \cdot 10^{-27} \frac{kg}{amu} \cdot particle's mass (amu) [/tex]

For the proton:

[tex] m = 1.66054 \cdot 10^{-27} \frac{kg}{amu} \cdot 1.00728 amu = 1.6726 \cdot 10^{-27} kg [/tex]

For the neutron:    

[tex] m = 1.66054 \cdot 10^{-27} \frac{kg}{amu} \cdot 1.00867 amu = 1.6749 \cdot 10^{-27} kg [/tex]

For the electron:

[tex] m = 1.66054 \cdot 10^{-27} \frac{kg}{amu} \cdot 5.49x10⁻⁴ amu = 9.1164 \cdot 10^{-31} kg [/tex]    

I hope it helps you!

The masses of proton, neutron, and electron are approximately 1.6726 x 10-27 kg, 1.6749 x 10-27 kg and 9.109 x 10-31 kg, respectively. This is calculated by multiplying each particle's mass in Atomic Mass Units by the factor 1.66054 × 10-27 kg/amu.

To calculate the mass of a proton, neutron, and electron in kilograms, we must know their masses in Atomic Mass Units (amu). We know that 1 amu = 1.66054 × 10

-27 kg. Using this we can get the masses as:

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Answer: B. Rusting of the metal is a chemical change.

Explanation: Rusting is considered a chemical change since it involves a change in the composition of iron through oxidation. Since there is a presence of oxygen and moisture it weakens the bonds of iron molecules to react and form iron oxide another substance in the chemical process.