if the perimeter of a rectangle is 122 cm and its length is 1cm more than twice its width

Answer:

c

Explanation:

The pH at the equivalence point when 35.0 mL of a 0.200 M solution of acetic acid (CH3COOH) is titrated with 0.100 M NaOH to its end point is 4.76.

The pH at the equivalence point when 35.0 mL of a 0.200 M solution of acetic acid (CH3COOH) is titrated with 0.100 M NaOH to its end point can be calculated using the formula derived from the Henderson-Hasselbalch equation.

The balanced chemical equation for this reaction is as follows: CH3COOH + NaOH → CH3COONa + H2OSince the reaction between the acetic acid and sodium hydroxide is a 1:1 ratio, the number of moles of NaOH required to reach the equivalence point will be equal to the number of moles of CH3COOH present in the 35.0 mL solution of 0.200 M acetic acid.

This can be calculated using the following formula: moles of CH3COOH = M x V moles of CH3COOH = 0.200 M x 0.0350 L = 0.00700 mol of CH3COOHTo calculate the volume of NaOH required to reach the equivalence point, we can use the formula: moles of NaOH = moles of CH3COOHmoles of NaOH = 0.00700 mol of CH3COOHNow that we know the number of moles of NaOH, we can calculate the volume of NaOH required to reach the equivalence point using the following formula: V = n / CV = 0.00700 mol / 0.100 M = 0.0700 L = 70.0 mL.

Since we have added 70.0 mL of 0.100 M NaOH to the 35.0 mL of 0.200 M acetic acid solution, the total volume of the solution at the equivalence point is: Vtotal = 35.0 mL + 70.0 mL = 105.0 mL. Now that we have determined the volume and concentration of the NaOH solution required to reach the equivalence point, we can use the Henderson-Hasselbalch equation to calculate the pH at the equivalence point: pH = pKa + log([A-]/[HA])At the equivalence point, the concentration of CH3COOH and CH3COO- are equal.

Therefore, the concentration of [HA] and [A-] are equal, and we can simplify the equation to:pH = pKa + log(1)Since the pKa of acetic acid is 4.76, we can substitute this value into the equation and solve for pH:pH = 4.76 + log(1)pH = 4.76.

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Taking into account the reaction stoichiometry, the volume of O₂ is 7.28406 L when 28.5 g of hydrogen peroxide decomposes to form water and oxygen at 150 degrees c and 2.0 atm.

The balanced reaction is:

2 H₂O₂  → 2 H₂O + O₂

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

The molar mass of the compounds is:

By reaction stoichiometry, the following mass quantities of each compound participate in the reaction:

The following rule of three can be applied: if by reaction stoichiometry 68 grams of H₂O₂ form 1 mole of O₂, 28.5 grams of H₂O₂ form how many moles of O₂?

moles of O₂= (28.5 grams of H₂O₂×1 mole of O₂)÷68 grams of H₂O₂

moles of O₂= 0.42 grams

Then, 0.42 moles of O₂ are formed.

Ideal gases are a simplification of real gases that is done to study them more easily. It is considered to be formed by point particles, do not interact with each other and move randomly. It is also considered that the molecules of an ideal gas, in themselves, do not occupy any volume.

The pressure, P, the temperature, T, and the volume, V, of an ideal gas, are related by a simple formula called the ideal gas law:

P×V = n×R×T

Where:

In this case, you know:

Replacing in the definition of the ideal gas law:

2 atm×V = 0.42 moles×0.082 (atmL)÷(molK)× 423 K

Solving:

V = (0.42 moles×0.082 (atmL)÷(molK)× 423 K)÷ 2 atm

V= 7.28406 L

Finally, the volume of O₂ is 7.28406 L.

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Answer:

1. A

2. B

Explanation:

Answer:

9.63 L of NO

Explanation:

We'll begin by calculating the number of mole in 50.0 g of NH₄ClO₄. This can be obtained as follow:

Mass of NH₄ClO₄ = 50 g

Molar mass of NH₄ClO₄ = 14 + (4×1) + 35.5 + (16×4)

= 14 + 4 + 35.5 + 64

= 117.5 g/mol

Mole of NH₄ClO₄ =?

Mole = mass /molar mass

Mole of NH₄ClO₄ = 50/117.5

Mole of NH₄ClO₄ = 0.43 mole

Next, we shall determine the number of mole of NO produced by the reaction of 50 g (i.e 0.43 mole) of NH₄ClO₄. This can be obtained as follow:

3Al + 3NH₄ClO₄ –> Al₂O₃ + AlCl₃ + 3NO + 6H₂O

From the balanced equation above,

3 moles of NH₄ClO₄ reacted to produce 3 moles of NO.

Therefore, 0.43 mole of NH₄ClO₄ will also react to produce 0.43 mole of NO.

Finally, we shall determine the volume occupied by 0.43 mole of NO. This can be obtained as follow:

1 mole of NO = 22.4 L

Therefore,

0.43 mole of NO = 0.43 × 22.4

0.43 mole of NO = 9.63 L

Thus, 9.63 L of NO were obtained from the reaction.

The formula for phosphorous acid is H₃PO₃. It can also be written as HPO(OH)₂, which is the hydrated form of the compound.

Phosphorous acid is a diprotic acid that contains one P(III) center and two -OH groups. It is a colorless and odorless solid that is highly soluble in water. When it is dissolved in water, it can act as a reducing agent because it can easily donate electrons. The formula for phosphate is PO₄³⁻. It is a polyatomic ion that contains one central phosphorus atom and four oxygen atoms arranged in a tetrahedral structure.

Phosphate has a negative three charge and is commonly found in minerals such as apatite. The formula for phosphite is PO₃³⁻. It is a polyatomic ion that contains one central phosphorus atom and three oxygen atoms arranged in a trigonal pyramidal structure. Phosphite has a negative two charge and is commonly used as a reducing agent and a chelating agent in chemical reactions involving metal ions.

The formula for phosphorus is P. It is a chemical element that has the atomic number 15 and the symbol P. Phosphorus is a nonmetal that is essential for life and is found in DNA, RNA, and ATP. It is also used in the production of fertilizers, detergents, and other industrial chemicals.

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Zinc hydroxide, which is represented by the chemical formula Zn(OH)₂, is a basic hydroxide salt of zinc.

In a saturated solution of Zn(OH)₂, the concentration of the zinc ions and the hydroxide ions will be equal to the solubility product of Zn(OH)₂. As a result, we can calculate the pH of a saturated solution of Zn(OH)₂ by using the equation for the solubility product constant (Ksp).

The solubility product constant for Zn(OH)₂ is given as Ksp=1.8x10⁻¹⁴. This means that the product of the zinc ion concentration [Zn²⁺] and the hydroxide ion concentration [OH⁻] in a saturated solution of Zn(OH)₂ will be equal to 1.8x10⁻¹⁴.

Using this equation, we can calculate the concentration of hydroxide ions in a saturated solution of Zn(OH)₂. Since the concentration of zinc ions is equal to the concentration of hydroxide ions in a saturated solution of Zn(OH)₂, we can calculate the concentration of zinc ions as well.

[Zn²⁺][OH⁻] = 1.8x10⁻¹⁴∴ [Zn²⁺] = [OH⁻] = √(1.8x10⁻¹⁴) = 1.34x10⁻⁷ M. The pH of the solution can be determined by using the formula: pOH = -log[OH⁻] = -log(1.34x10⁻⁷) = 6.87pH = 14 - pOH = 7.13. Therefore, the pH of a saturated solution of Zn(OH)₂ is approximately 7.13.

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Answer:

Lithium has 5 elements, sulphur has 2 elements and oxygen has 4 elements

The theoretical values for ΔS and ΔG for the dissolution reaction of calcium chloride in water are approximately:

ΔS = 401.0 J/(mol·K)

ΔG = -343.6 kJ/mol

The standard molar entropy values (ΔS°) at 298 K (25°C) are as follows:

ΔS°(CaCl₂(s)) = 115.3 J/(mol·K)

ΔS°(Ca²⁺(aq)) = 72.1 J/(mol·K)

ΔS°(2Cl⁻(aq)) = 222.1 J/(mol·K)

The standard Gibbs free energy change (ΔG°) at 298 K (25°C) is given by the equation:

ΔG° = ΣnΔG°(products) - ΣnΔG°(reactants)

The standard Gibbs free energy change values (ΔG°) at 298 K (25°C) are as follows:

ΔG°(CaCl₂(s)) = -795.4 kJ/mol

ΔG°(Ca²⁺(aq)) = -544.6 kJ/mol

ΔG°(2Cl⁻(aq)) = -167.2 kJ/mol

For the dissolution reaction of CaCl₂ in water:

CaCl₂(s) → Ca²⁺(aq) + 2Cl⁻(aq)

To calculate the theoretical values of ΔS and ΔG, we use the stoichiometric coefficients of the balanced equation. The stoichiometric coefficients for the products and reactants are as follows:

n(Ca²⁺) = 1

n(Cl⁻) = 2

Calculating the values:

ΔS°(reaction) = ΣnΔS°(products) - ΣnΔS°(reactants)

= (1 * ΔS°(Ca²⁺(aq))) + (2 × ΔS°(Cl⁻(aq))) - ΔS°(CaCl₂(s))

Substituting the values:

ΔS°(reaction) = (1 × 72.1 J/(mol·K)) + (2 × 222.1 J/(mol·K)) - 115.3 J/(mol·K)

= 401.0 J/(mol·K)

ΔG°(reaction) = ΣnΔG°(products) - ΣnΔG°(reactants)

= (1 × ΔG°(Ca²⁺(aq))) + (2 × ΔG°(Cl⁻(aq))) - ΔG°(CaCl₂(s))

Substituting the values:

ΔG°(reaction) = (1 × -544.6 kJ/mol) + (2 × -167.2 kJ/mol) - (-795.4 kJ/mol)

= -343.6 kJ/mol

Therefore, the theoretical values for ΔS and ΔG for the dissolution reaction of calcium chloride in water are approximately:

ΔS = 401.0 J/(mol·K)

ΔG = -343.6 kJ/mol

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The correct answer is 5 Ni 138 56.

Explanation :

The nucleotide which has the largest nuclear binding energy per nucleon is nickel-56 (56Ni). It is important to note that nuclear binding energy per nucleon refers to the energy released when a nucleus is formed by assembling its nucleons.

The nuclear binding energy is the amount of energy required to separate an atomic nucleus into its individual nucleons. It is the sum of the energy of the individual nucleons in the nucleus. It's important to remember that when atomic nuclei are formed, they release a certain amount of energy in the process.

The nuclear binding energy per nucleon depends on the total number of nucleons present. In general, the larger the number of nucleons in an atomic nucleus, the greater the amount of nuclear binding energy per nucleon.

Therefore, among the given nucleotides, nickel-56 (56Ni) has the largest nuclear binding energy per nucleon. The amount of energy released when nickel-56 (56Ni) is formed is greater than that released by any other nuclide. The high energy released by nickel-56 (56Ni) makes it important for the process of nuclear fusion in stars.

Thus, the answer to this question is nickel-56 (56Ni).

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Answer:

terminal velcity

Explanation:

Answer:

Input Mask

Explanation:

In this scenario, the best tool for Raul to use would be an Input Mask. When dealing with Microsoft Access or any other database tool, Input Masks are a great way of validating data inputs so that they always match the desired format. In this case, Raul would need to use input mask and apply the desired format while comparing it to the order date, therefore, making sure that it is always a minimum of 2 days after before it is accepted as a valid entry in the database.

Answer:

Explanation:

Find the molar mass of H2SO4

2H = 2 * 1 = 2

S  = 1 * 32 =32

O4 = 4*16 = 64

total             98

Find the number of mols in 71.5 grams

mols = given mass / molar mass.

given mass = 71.5

molar mass = 98

mols = 71.5/98

mols = 0.7296 mols of H2SO4

Find the moles of H2O

From the Balanced equation, every mol of H2SO4 produces 2 moles of H2O

mols water = 2 * 0.7296

mols water = 1.4592

That's as far as I can take you. I have to know a great deal more to get the volume of H2O

A dilute solution of NaOH needs to be standardized in order to accurately determine its concentration. Standardization involves comparing the concentration of the NaOH solution to a known concentration of a primary standard substance.

There are several reasons why standardization is necessary. Firstly, NaOH is highly hygroscopic, meaning it readily absorbs moisture from the air. This moisture absorption can alter the concentration of the solution over time, leading to inaccurate results. By standardizing the NaOH solution, we can ensure that its concentration is accurately determined at a specific point in time. Secondly, during the manufacturing and storage process, impurities may be introduced into the NaOH solution, affecting its concentration. Standardization allows us to account for these impurities and determine the true concentration of the solution. Lastly, dilution of the NaOH solution introduces a potential for errors in the preparation process, such as inaccuracies in volumetric measurements. Standardization helps correct for these errors and provides a reliable concentration value for subsequent use in various analytical procedures.

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Answer:

From top to bottom coyote, crow, squirrel, then acorn

Explanation:

The coyote has the least amount of energy and its the biggest predator so it belongs at the top. The crows eat squirrels and the squirrels eat acorns.

(1)The densities of the two rubbing alcohol samples may not be identical. (2)The density of the rubber stopper should not be reported based on the density determined from only one piece. (a) Due to the procedural error of water splashing out when adding the rubber stopper, the experimentally determined density of the stopper would be erroneously low. (b) If the top of an unknown object remains above the water surface, the calculated volume would be too low, as it does not account for the portion of the object above the water level.

The densities of rubbing alcohol samples may differ due to variations in the concentration or impurities present in each sample. Differences in the manufacturing process or storage conditions can result in slight variations in concentration, which can impact the density. Additionally, impurities present in the samples can affect their densities, as different impurities have different molecular masses and structures.

When sharing the rubber stopper, the experimentally determined density of the individual pieces should not be reported as the density of the entire stopper. Instead, the densities determined by both partners should be added together to obtain the total density of the original stopper. This is because cutting the stopper into two pieces alters its overall volume, and reporting the density based on only one piece would not provide an accurate representation of the original stopper's density.

(a) If water splashes out when adding the rubber stopper to the graduated cylinder, the displaced water volume would be erroneously low. This would result in a lower overall density calculation for the stopper since density is calculated by dividing mass by volume. Therefore, the experimentally determined density of the stopper would be erroneously low.

(b) If the top of an unknown object remains above the water surface, the calculated volume would be too low. The volume of an object should include its entire submerged portion to obtain an accurate measurement. As the portion above the water surface is not accounted for, the calculated volume would underestimate the actual volume, leading to a calculated object volume that is too low.

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Answer:

radio waves

Explanation:

the answer is simple, radio waves. it is radio waves because when you look at the diagram the waves below Radio are very long. if you look at the waves under gamma ray, they are very short. radio is the longest wave while gamma is the shortest. if you are still confused it also says longer wavelength and low frequency( meaning it is safe) right under the wavelength.

Answer:

Depending on the different angles the sun reaches the earth at, the amount of the suns ray may differ per angle. Smaller, more concentrated areas of the suns rays would result in warmer temperatures while areas where sunlight is spread out may have colder temperatures.

Answer:

Physics is a natural science that involves the study of matter and its motion through space and time, along with related concepts such as energy and force. More broadly, it is the study of nature in an attempt to understand how the universe behaves.

Explanation:

The ∆H° for the reaction  [tex]1/2 Mg_3N_2(s) + 3H_2O(l)[/tex]→[tex]1/2 Mg(OH)_2 (s) + NH_3(g)[/tex] is approximately -1372.54 kJ/mol

To calculate the ∆H° for the reaction[tex]1/2 Mg_3N_2(s) + 3H_2O(l)[/tex] → [tex]1/2 Mg(OH)_2 (s) + NH_3(g)[/tex], we need to use the given information that 3.4 kJ of energy are released when excess water is added to 0.50 g of Mg3N2(s).

First, let's calculate the moles of [tex]Mg_3N_2[/tex](s):

Molar mass of [tex]Mg_3N_2[/tex] = 3 * molar mass of Mg + 2 * molar mass of N

Molar mass of [tex]Mg_3N_2[/tex] = 3 * 24.31 g/mol + 2 * 14.01 g/mol = 100.95 g/mol

Moles of [tex]Mg_3N_2[/tex](s) = Mass / Molar mass

Moles of [tex]Mg_3N_2[/tex](s) = 0.50 g / 100.95 g/mol = 0.004955 mol

Next, we can determine the ∆H° per mole of [tex]Mg_3N_2[/tex](s):

∆H° per mole = Energy released / Moles of [tex]Mg_3N_2[/tex](s)

∆H° per mole = -3.4 kJ / 0.004955 mol = -686.27 kJ/mol

Since the balanced equation shows that only half a mole of [tex]Mg_3N_2[/tex](s) is involved, we multiply the ∆H° per mole by 2:

∆H° = 2 * ∆H° per mole

∆H° = 2 * (-686.27 kJ/mol) = -1372.54 kJ/mol

Therefore, the ∆H° for the reaction  [tex]1/2 Mg_3N_2(s) + 3H_2O(l)[/tex]→[tex]1/2 Mg(OH)_2 (s) + NH_3(g)[/tex] is approximately -1372.54 kJ/mol.

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A. [tex]HC_{2} O^{-} _{4[/tex] (oxalate ion) acts as a base by accepting a proton from [tex]HS^{-}[/tex] (hydrosulfide ion) to form [tex]H_{2}C_{2} O_{4}[/tex] (oxalic acid).

B. [tex]HC_{2} O^{-} _{4[/tex] (oxalate ion) acts as an acid by donating a proton to [tex]HS^{-}[/tex](hydrosulfide ion) to form [tex]C_{2} O^{-} _{4[/tex] (oxalate ion).

A. At the point when [tex]HC_{2} O^{-} _{4[/tex] goes about as a base, it acknowledges a proton ([tex]H^{+}[/tex]) from [tex]HS^{-}[/tex], which goes about as a corrosive. The condition can be addressed as:

[tex]HC_{2} O^{-} _{4[/tex]+ [tex]HS^{-}[/tex] → [tex]H_{2}C_{2} O_{4}[/tex] +[tex]S^{-} _{2}[/tex]

In this response,[tex]HC_{2} O^{-} _{4[/tex] goes about as a base by tolerating a proton from the corrosive [tex]HS^{-}[/tex], shaping the impartial particle [tex]H_{2}C_{2} O_{4}[/tex] (oxalic corrosive) and the form base [tex]S^{-} _{2}[/tex].

B. At the point when [tex]HC_{2} O^{-} _{4[/tex] goes about as a corrosive, it gives a proton ([tex]H^{+}[/tex]) to [tex]HS^{-}[/tex], which goes about as a base. The condition can be addressed as:

[tex]HC_{2} O^{-} _{4[/tex] +[tex]HS^{-}[/tex] → [tex]HC_{2} O^{-} _{4[/tex]+ [tex]H_{2} S[/tex]

In this response, [tex]HC_{2} O^{-} _{4[/tex]goes about as a corrosive by giving a proton to the base [tex]HS^{-}[/tex], bringing about the development of the form base [tex]HC_{2} O^{-} _{4[/tex](oxalate particle) and the unbiased atom [tex]H_{2} S[/tex] (hydrogen sulfide).

In the two cases, [tex]HC_{2} O^{-} _{4[/tex] displays its amphoteric nature by having the option to go about as both a corrosive and a base, contingent upon the idea of the responding species.

[tex]HS^{-}[/tex], thus, exhibits its capacity to go about as a corrosive while responding with [tex]HC_{2} O^{-} _{4[/tex] as a base and as a base while responding with [tex]HC_{2} O^{-} _{4[/tex] as a corrosive.

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The chemical formula of the gas is Option c, Helium.

We need to take into account the molar masses and the root mean square (RMS) speeds of various gases in order to ascertain the chemical formula of the gas that escapes through the pinhole 2.65 times quicker than N₂ gas.

The following equation describes how a gas's molar mass and RMS speed are related:

RMS velocity = 1/√(molar mass)

The following ratio may be established since the provided gas leaves 2.65 times more quickly than N₂ gas:

RMS speed of the given gas / RMS speed of N₂ gas = 2.65

Now, let's compare the molar masses of the options provided:

a. Ne (Neon) has a molar mass of approximately 20 g/mol.

b. O₂ (Oxygen) has a molar mass of approximately 32 g/mol.

c. He (Helium) has a molar mass of approximately 4 g/mol.

d. Ar (Argon) has a molar mass of approximately 40 g/mol.

Since the ratio of RMS speeds is greater than 1, the molar mass of the given gas must be less than that of N₂ gas. Among the options, the only gas with a molar mass significantly lower than N₂ gas is Helium (He) with a molar mass of approximately 4 g/mol.

Therefore, the chemical formula of the gas is Option C, Helium.

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Answer:

A- Before the mechanic left, the molecules were moving away from each other. When she returned, they were moving around each other.

Explanation:

Brainliest?

The mass of oxygen gas in the unknown mixture is approximately 5.868 g. The mass of ethane gas in the unknown mixture is approximately 0.812 g. The mass percent of oxygen gas in the unknown mixture is approximately 71.83%.

To solve this problem, we need to determine the masses of oxygen gas and ethane gas in the unknown mixture, as well as the mass percent of oxygen gas.

Let's start by calculating the mass of water produced;

Mass of water = 1.48 g

Since water is composed of hydrogen and oxygen in a 2:1 ratio, the molar mass of water is:

Molar mass of water = 2(1.00784 g/mol) + 15.999 g/mol = 18.015 g/mol

Now we can calculate the number of moles of water produced;

Number of moles of water = Mass of water/Molar mass of water

= 1.48 g / 18.015 g/mol

≈ 0.082 mol

From balanced chemical equation for the combustion of ethane;

C₂H₆ + 7/2 O₂ → 2 CO₂ + 3 H₂O

We can see that 1 mole of ethane produces 3 moles of water. Therefore, the number of moles of ethane can be calculated as;

Number of moles of ethane = (Number of moles of water) / 3

≈ 0.082 mol / 3

≈ 0.027 mol

The molar mass of ethane (C₂H₆) is;

Molar mass of ethane = 2(12.011 g/mol) + 6(1.00784 g/mol)

= 30.0708 g/mol

Finally, we can calculate the mass of ethane;

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

≈ 0.027 mol × 30.0708 g/mol

≈ 0.812 g

Now, to determine the mass of oxygen gas, we subtract the mass of ethane and water from the total mass of the unknown mixture:

Mass of oxygen gas = Total mass of unknown mixture - Mass of ethane - Mass of water

= 8.16 g - 0.812 g - 1.48 g

≈ 5.868 g

Finally, we can calculate the mass percent of oxygen gas in the unknown mixture;

Mass percent of oxygen gas = (Mass of oxygen gas / Total mass of unknown mixture) × 100%

= (5.868 g / 8.16 g) × 100%

≈ 71.83%

Therefore;

The mass of oxygen gas in the unknown mixture is approximately 5.868 g.

The mass of ethane gas in the unknown mixture is approximately 0.812 g.

The mass percent of oxygen gas in the unknown mixture is approximately 71.83%.

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Answer:

a

Explanation:

Answer:

1150g

Explanation:

The equation for producing sulphur dioxide is [tex]S + O_{2} ==> SO_{2}[/tex]

Looking at the ratios, you need 1 mole of sulphur for every 1 mole of sulphur dioxide

Sulphur dioxide has a molar mass of 32 + (2 x 16) = 64g

2.30 x 1000 = 2300

2300 / 64 = 35.9375

35.9375 x 32 = 1150g of sulphur

Answer:

4.9 atm

Explanation:

Given:

Total pressure = 7.0 atm

(Total number of moles)=[ (1.5 mol arg) + (3.5 mol co2) ]

= 5 moles

Let Partial pressure of CO2 gas = P(CO2)

✓✓partial pressure of CO2 can be calculated using below expresion.

P(CO2) / Total pressure = (moles of CO2 gas) / Total number of moles

✓✓ Let us substitute the values into the above expresion.

[P(CO2) / 7.0 atm ] = [3.5 mol / 5 moles]

P(CO2)= [7 atm × 3.5 moles] / [5 moles]

= 4.9 atm

Hence, the partial pressure of CO2 is 4.9 atm

Answer:

Partial pressure of CO₂ = 4.9 atm

Explanation:

From the question given above, the following data were obtained:

Mole of Ar = 1.5 moles

Mole of CO₂ = 3.5 moles

Total pressure (Pₜ) = 7.0 atm

Partial pressure of CO₂ =?

Next, we shall determine the mole fraction of CO2. This can be obtained as follow:

Mole of Ar = 1.5 moles

Mole of CO₂ = 3.5 moles

Total mole = 1.5 + 3.5

Total mole = 5 mole

Mole fraction of CO₂ = mole of CO₂ / total mole

Mole fraction of CO₂ = 3.5 / 5

Mole fraction of CO₂ = 0.7

Finally, we shall determine the partial pressure of CO₂. This can be obtained as follow:

Total pressure (Pₜ) = 7.0 atm

Mole fraction of CO₂ = 0.7

Partial pressure of CO₂ =?

Partial pressure of CO₂ = mole fraction of CO₂ × total pressure

Partial pressure of CO₂ = 0.7 × 7

Partial pressure of CO₂ = 4.9 atm

Equilibrium in a chemical reaction is reached when the rates of the forward and reverse reactions become equal. For a reversible reaction, the equilibrium constant is the ratio of the concentrations of the products to the concentrations of the reactants at equilibrium.

The following variables need to remain constant for an equilibrium constant and position to remain constant:

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The required correct answer is option D) Te.

An atom of Tellurium (Te) has 52 electrons and its electron configuration is 1s22s22p63s23p64s23d104p65s24d105p4. It has six electrons in its outermost shell and it requires two more electrons to complete its octet. Upon gaining two electrons, the electron configuration of Te will become 1s22s22p63s23p64s23d104p65s24d105p6.Te (Tellurium) is a chemical element with an atomic number of 52. It is a rare, silvery-white metalloid that is widely used in various industries. The majority of tellurium is used in alloys and as an additive to copper, steel, and lead to increase their strength and durability. It's also used in the production of solar panels and other electronic devices.

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