Hazel used 45. 7grams of nickel II nitrate Ni(NO3)2 to make a 1. 25M solution. How much water is required to make this solution?



Solve for the GFM=

There are 516.682 grams in a sample of 7.9 moles of zinc.

To determine the number of grams in a sample of 7.9 moles of zinc, we need to use the molar mass of zinc. The molar mass of zinc is 65.38 g/mol.

Therefore, to calculate the number of grams in 7.9 moles of zinc, we can multiply 7.9 moles by 65.38 g/mol. The calculation is as follows:

7.9 moles x 65.38 g/mol = 516.682 g

Therefore, there are 516.682 grams in a sample of 7.9 moles of zinc. It's important to remember to always use the molar mass of the element or compound when converting between moles and grams.

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Turtle refuges are usually created on beaches where turtles lay their eggs, hatch, and return to the sea. Therefore, beaches that are known as nesting grounds for sea turtles may be suitable for creating a turtle refuge.

In general, turtle nesting sites are characterized by sandy beaches, dunes, and undisturbed vegetation. Female sea turtles come ashore to lay their eggs on sandy beaches, and the hatchlings make their way to the ocean once they emerge from the nest.

Turtle refuges provide protection for these nesting sites, allowing the turtles to lay their eggs and for the hatchlings to safely make their way to the ocean.

It is important to note that the location of a turtle refuge should be based on careful research and consideration of a variety of factors, such as the species of turtles that inhabit the area, the presence of human and natural threats to the nesting sites, and the availability of resources and support for the conservation efforts.

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The amount of HCl produced when 57.49 grams of H₂SO4 after a chemical reaction with 98.20 grams of NaCl (in grams) is found out being  42.70 grams.

The balanced chemical equation as per the mentioned case, the reaction between H₂SO₄ and NaCl can be represented as,

H₂SO₄ + 2 NaCl -----> 2 HCl + Na₂SO₄

We are needed to use stoichiometry in the way to know the amount of HCl produced out from the given amounts of H₂SO₄ and NaCl.

Step 1: Convert the given masses of H₂SO₄ and NaCl into an amount of equivalent moles.

Molar mass of H₂SO₄ is = 98.08 g/mol

Molar mass of NaCl is 58.44 g/mol

Number of moles of H₂SO₄  = 57.49 g / 98.08 g/mol = 0.586 mol

Number of moles of NaCl = 98.20 g / 58.44 g/mol = 1.679 mol

Step 2: Now we have to balance the chemical equation to know the mole ratio for H₂SO₄ to HCl.

From the balanced equation, we observe that 1 mole of H₂SO₄ produces 2 moles of HCl. Therefore, the 0.586 moles of H₂SO₄ will be producing about 2 × 0.586 = 1.172 moles of HCl.

Lastly, Convert the moles of HCl to grams.

Molar mass of HCl = 36.46 g/mol

Mass of HCl produced = 1.172 mol × 36.46 g/mol = 42.70 g

Therefore, it can be concluded that about 57.49 grams of H₂SO₄ would be reacting with nearly 98.20 grams of NaCl in order to produce out about 42.70 grams of HCl.

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The oxidation number approach, commonly referred to as the oxidation states, keeps track of the electrons obtained during reduction and the electrons lost during oxidation.

Thus, Each atom in a charged or neutral molecule is given an oxidation number. Oxidation takes place whenever the oxidation number rises. Reduction happens when the oxidation number goes down. The total charge of a chemical is equal to the sum of all of its oxidation numbers.

 The roles of oxidation and reduction is the only foolproof method for balancing a redox equation. Then you achieve equilibrium by bringing the electron gain and loss into balance.

The oxidation numbers of all atoms are determined using the oxidation number method. The altered atoms are then multiplied by small whole numbers.

Thus, The oxidation number approach, commonly referred to as the oxidation states, keeps track of the electrons obtained during reduction and the electrons lost during oxidation.

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The type of conversion that would be required to determine how many liters 26 grams of water is would be a conversion from mass to volume. This is because grams are a unit of mass, while liters are a unit of volume. In order to make this conversion, it is necessary to know the density of water, which is approximately 1 gram per milliliter at room temperature and atmospheric pressure.

To convert 26 grams of water to liters, we need to divide the mass by the density. This gives us:

26 grams / 1 gram per milliliter = 26 milliliters
Since there are 1000 milliliters in a liter, we can further convert this to liters by dividing by 1000:
26 milliliters / 1000 = 0.026 liters

Therefore, 26 grams of water is equivalent to 0.026 liters of water.

In summary, to determine the volume of a given mass of water, we need to use the density of water as a conversion factor. This involves dividing the mass by the density to obtain the volume in milliliters, and then converting this to liters by dividing by 1000.

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The volume of the gas at 100℃ would be 4.64 liters, assuming the pressure remains constant.

We can use the combined gas law, which relates the pressure, volume, and temperature of a gas. The combined gas law formula is: (P1 x V1) / T1 = (P2 x V2) / T2. Where P is the pressure, V is the volume, and T is the temperature. The subscripts 1 and 2 refer to the initial and final states of the gas, respectively.

In this case, we know that the initial volume (V1) is 4 liters and the initial temperature (T1) is 50 ℃. We want to find the final volume (V2) when the temperature is 100℃.To solve for V2, we can rearrange the formula as follows: V2 = (P1 x V1 x T2) / (P2 x T1).We don't know the pressure, but since the problem doesn't mention any changes in pressure, we can assume that it remains constant. Therefore, we can cancel out the P1 and P2 terms.

Plugging in the known values, we get: V2 = (4 L x 373 K) / (323 K) = 4.64 L (rounded to two decimal places)Therefore, the volume of the gas at 100℃ would be 4.64 liters, assuming the pressure remains constant.

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The reaction that undergoes a condensation reaction to produce CH₃CH₂OCH₂CH₃ is the reaction is involving 2CH₃CH₂OH  which is Option D.

The reason behind this is that the reaction between these two compounds is an example of a nucleophilic substitution reaction which includes the replacement or taking over of a leaving group (in this case Br) by a nucleophile (in this case OH) . The reaction projects van SN2 reaction mechanism.

SN2 reaction mechanism refers to the  type of reaction mechanism that is very common in organic chemistry. Inside this mechanism, one bond is broken and dismantled and one bond is formed in a concerted way.

The SN2 reaction mechanism includes the nucleophilic substitution reaction of the leaving group (which generally consists of halide groups or other electron-withdrawing groups) with a nucleophile in a given organic compound .

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If the decomposition of hydrogen peroxide into water and oxygen gas is an exothermic reaction, we would expect the final temperature to be lower than the initial temperature of 28˚C.

This is because during an exothermic reaction, energy is released from the system into the surroundings in the form of heat. In other words, the energy of the products (water and oxygen) is lower than the energy of the reactants (hydrogen peroxide), and the excess energy is released into the surroundings.

As a result, the temperature of the surroundings (in this case, the container holding the reaction) will increase, while the temperature of the system (the reactants and products) will decrease. This means that the final temperature of the reaction will be lower than the initial temperature of 28˚C.

Overall, we would expect the reaction to release heat into the surroundings, causing the temperature of the surroundings to increase while the temperature of the system decreases.

The pressure of a gas is directly proportional to the number of moles of gas present, and inversely proportional to the volume of the container. Therefore, given the temperature of the gas in the tire remains constant, the pressure of the gas can be calculated using the ideal gas law:

PV = nRT

Where P is pressure, V is volume, n is number of moles, R is the ideal gas constant, and T is temperature.

In this case, the number of moles is 0.448 mol, the temperature is 28°C (or 301 K), and the volume is 7.32 l.

Plugging in all the values, we get:

P = (0.448 mol) × (8.314 L·atm·K−1·mol−1) × (301 K) / (7.32 l)

P = 4.20 atm

Therefore, the pressure of the gas in the tire is 4.20 atm.

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To solve this problem, we need to use the volume ratio from the balanced chemical equation. The ratio tells us that for every 3 liters of [tex]H_2[/tex] that reacts, 2 liters of [tex]NH_3[/tex] are produced.

In this case, we have 3.6 liters of [tex]H_2[/tex]  reacting, so we can set up a proportion:

3 L [tex]H_2[/tex]  : 2 L [tex]NH_3[/tex] = 3.6 L [tex]H_2[/tex]  : x L [tex]NH_3[/tex]

To solve for x (the amount of NH3 produced), we can cross-multiply:

3 L [tex]H_2[/tex]  * x L [tex]NH_3[/tex] = 2 L [tex]NH_3[/tex] * 3.6 L [tex]H_2[/tex]  

Simplifying, we get:

x = (2 L [tex]NH_3[/tex] * 3.6 L [tex]H_2[/tex] ) / 3 L [tex]H_2[/tex]  

x = 2.4 L [tex]NH_3[/tex]

Therefore, the answer is 2.4 liters of [tex]NH_3[/tex] produced if 3.6 liters of [tex]H_2[/tex]  reacts with an excess of [tex]N_2[/tex].

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The solution has a Molarity of approx 0.01575 M.

To calculate the molarity of a solution, we use the formula:

Molarity (M) = moles of solute ÷ volume of solution in liters

First, we need to convert the volume of the solution from milliliters to liters:

Volume of solution = 400 mL = 400/1000 L = 0.4 L

Next, we need to calculate the moles of solute:

moles of solute = 6.3 x [tex]10^{-3[/tex] mol

Substituting these values into the formula, we get:

Molarity (M) = 6.3 x[tex]10^{-3[/tex] mol ÷ 0.4 L = 0.01575 M

Therefore, the molarity of the solution is 0.01575 M.

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Answer:   Elements and compounds are both examples of pure substances.

Explanation:

The volume at standard pressure will be 293 mL.

To find the volume of gas at standard pressure, we need to use the ideal gas law, which states that PV = nRT, where P is pressure, V is volume, n is the number of moles, R is the gas constant, and T is the temperature.

Since the temperature remains constant, we can rearrange the equation to solve for the volume at standard pressure:

(P₁V₁) / P₂ = V₂

Where P₁ is the initial pressure, V₁ is the initial volume, P₂ is the final pressure (standard pressure), and V₂ is the final volume (what we're solving for).

Plugging in the given values, we get:

(112 kPa)(259 mL) / (1 atm) = V₂

Simplifying and converting units of pressure and volume, we get:

(112000 Pa)(0.259 L) / (1.01325 × 10⁵ Pa) = V₂

Solving for V₂, we get:

V₂ = 0.293 L = 293 mL

Rounding to 3 significant figures, we get that the volume at standard pressure will be 293 mL.

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Answer:

0.108L HCl

Explanation:

5.32 g zinc * 1 mol zinc/65.38g zinc * 2 mol HCl/1 mol zinc * L HCl/1.5 mol HCl = 0.108L HCl

The boiling point of the solution prepared by dissolving 2.50 g of biphenyl in 85.0 g of benzene is 80.58 °C.

The boiling point elevation of the solution can be determined using the equation ΔTb = Kb x m, where ΔTb represents the boiling point elevation, Kb is the boiling point elevation constant (for benzene, Kb = 2.53 °C/m), and m denotes the molality of the solution.

To calculate the molality, we first need to find the number of moles of biphenyl in the solution. By dividing the given mass of biphenyl (2.50 g) by its molar mass (154 g/mol), we obtain 0.0162 mol.

Next, we can determine the molality by dividing the moles of solute by the mass of the solvent in kilograms. Given that the mass of the solvent is 85.0 g (0.085 kg), the molality is calculated as 0.0162 mol / 0.085 kg = 0.191 mol/kg.

Substituting this molality into the equation, we have ΔTb = 2.53 °C/m x 0.191 mol/kg = 0.484 °C.

This indicates that the boiling point of the solution is raised by 0.484 °C compared to the boiling point of pure benzene, which is 80.1 °C.

Therefore, the boiling point of the solution, prepared by dissolving 2.50 g of biphenyl in 85.0 g of benzene, is 80.58 °C.

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Answer:

0.08 atm

Explanation:

The pressure change of a gas at constant volume can be determined using the ideal gas law:

PV = nRT

Where P is the pressure, V is the volume, n is the number of moles, R is the gas constant, and T is the temperature in Kelvin.

Since the volume is constant, we can simplify the ideal gas law to:

P = (nRT) / V

The number of moles and the gas constant are constant for a given sample of gas, so we can further simplify to:

P1 / T1 = P2 / T2

Where P1 and T1 are the initial pressure and temperature, and P2 and T2 are the final pressure and temperature.

Plugging in the given values:

P1 = 2.50 atm

T1 = 30.0 + 273.15 = 303.15 K

T2 = 40.0 + 273.15 = 313.15 K

P2 = (P1 * T2) / T1

P2 = (2.50 atm * 313.15 K) / 303.15 K

P2 = 2.58 atm

Therefore, the pressure change when a constant volume of gas at 2.50 atm is heated from 30.0 °C to 40.0 °C is 0.08 atm (2.58 atm - 2.50 atm).

Answer:

Explanation: 0.08

The least effective choice of color would be green color. Hence option a is correct.

The plants absorb all different wavelength lights of the visible light spectra but the only color that is not absorbed and reflected back is green color light.

The principal pigment in photosynthesis, chlorophyll, reflects green light and significantly absorbs red and blue light. Chloroplasts, which house the chlorophyll in plants, are where photosynthesis occurs.

The plant's green colour is a reflection of the green light. Violet and orange (chlorophyll a) and blue and yellow (chlorophyll b) are the colours that are most readily absorbed. Therefore, green colour light would be least effective for the production of sugar and fruit in this tomato plant.

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The statement that reflects a central theme of the atomists is: Atomists would agree that a butterfly and a caterpillar exist as a collection of atoms, but their atoms are organized differently.

Atomists believe that everything in the universe is composed of small, indivisible particles called atoms. They assert that the properties of objects, like a butterfly and a caterpillar, are determined by the arrangement and organization of these atoms.

While a butterfly and a caterpillar may share similar atoms, their unique characteristics are due to the differences in how these atoms are arranged within each organism.

This perspective acknowledges the transformation from a caterpillar to a butterfly as a process of reorganization of atoms, rather than the creation or destruction of matter.

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The pressure of a gas is 1.2 atm at 300k.  the pressure  at 250k if the gas is in a rigid container is 1.0 atm.

To solve this problem, we can use the combined gas law, which states that:

(P1 * V1) / (T1) = (P2 * V2) / (T2)

where P1 is the initial pressure, V1 is the initial volume (which is constant since the gas is in a rigid container), T1 is the initial temperature, P2 is the final pressure (what we're trying to find), V2 is the final volume (also constant), and T2 is the final temperature.

We can rearrange the equation to solve for P2:

P2 = (P1 * V1 * T2) / (V2 * T1)

Plugging in the given values, we get:

P2 = (1.2 atm * V1 * 250K) / (V2 * 300K)

Since the container is rigid, V1 = V2, so we can cancel those terms:

P2 = (1.2 atm * 250K) / 300K

Simplifying:

P2 = 1.0 atm

Therefore, the pressure of the gas at 250K in a rigid container is 1.0 atm.

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In the electrowinning process, the energy applied using 5 mol of IR photons with a wavelength of 32 nm is 1.863 MJ.

1. Convert wavelength to energy using the equation: E = (hc)/λ, where h is Planck's constant (6.626×10⁻³⁴ Js), c is the speed of light (3×10⁸ m/s), and λ is the wavelength (32 nm = 32×10⁻⁹ m).

2. Calculate the energy of one IR photon: E = (6.626×10⁻³⁴ Js × 3×10⁸ m/s) / (32×10⁻⁹ m) = 6.184×10⁻¹⁹ J.

3. Determine the energy for 5 moles of IR photons: Total energy = 6.184×10⁻¹⁹ J × 5 × 6.022×10²³ photons/mol = 1.863×10⁶ J.

4. Convert energy to megajoules: 1.863×10⁶ J = 1.863 MJ.

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Answer:

Carbon and silicon are both in Group 14 of the periodic table, which means they have similar electronic configurations and therefore similar bonding properties. However, the difference in melting and sublimation temperatures of their oxides, silicon oxide and solid carbon dioxide, respectively, can be attributed to differences in their structure and bonding.

Silicon oxide (SiO2) has a giant covalent structure, in which each silicon atom is covalently bonded to four oxygen atoms and each oxygen atom is covalently bonded to two silicon atoms. This gives rise to a three-dimensional network of strong covalent bonds, which requires a large amount of energy to be broken. Therefore, silicon oxide has a high melting point of 2440°C because a lot of energy is required to overcome the strong covalent bonds and melt the solid.

On the other hand, solid carbon dioxide (CO2) has a molecular structure, in which each carbon atom is double bonded to two oxygen atoms. The carbon dioxide molecules are held together by weak intermolecular forces, such as Van der Waals forces, which are much weaker than the strong covalent bonds present in silicon oxide. As a result, solid carbon dioxide can sublime at -70°C, without melting into a liquid, because the intermolecular forces can be overcome by relatively low energy input.

In summary, the difference in melting and sublimation temperatures of silicon oxide and solid carbon dioxide can be explained by the difference in their bonding types and structures. Silicon oxide has a giant covalent structure with strong covalent bonds that require a large amount of energy to break, resulting in a high melting point. Solid carbon dioxide has a molecular structure held together by weak intermolecular forces, which can be overcome by relatively low energy input, resulting in a low sublimation point.

Answer:

A chemical formula tells us the number of atoms of each element in a compound.

Explanation:

Explanation:

formula shows

At standard temperature and pressure (STP), 1 mole of any gas occupies 22.4 L of volume. Therefore, 8.19 L of gas at STP represents 0.364 moles and 21.7 L of gas at STP represents 0.969 moles.

Moles are a unit of measurement for the amount of matter present in an object. The number of moles in an object is proportional to the amount of matter present, and it is calculated by dividing the mass of an object by its molar mass. The molar mass of a substance is its molecular mass expressed in grams.

At STP, the number of moles of a gas in a given volume can be calculated by dividing the volume of the gas (in liters) by 22.4. This is because 1 mole of any gas occupies 22.4 L of volume at STP. Therefore, by dividing the volume of the gas by 22.4, the number of moles of gas is obtained.

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The enthalpy change when 2.50 kg of Glauber's salt solidifies is 605.28 kJ.

To calculate the enthalpy change when 2.50 kg of Glauber's salt (sodium sulfate decahydrate, Na2SO4·10H2O) solidifies, you can follow these steps:

1. Convert the mass of Glauber's salt to moles:
2.50 kg = 2500 g
Molar mass of Na2SO4·10H2O = (2×23) + (32) + (4×16) + (10×(2+16)) = 46 + 32 + 64 + 180 = 322 g/mol
Moles of Glauber's salt = 2500 g / 322 g/mol = 7.76 mol

2. Multiply the moles by the energy released per mole:
Energy released = 7.76 mol × 78.0 kJ/mol = 605.28 kJ

The enthalpy change when 2.50 kg of Glauber's salt solidifies is 605.28 kJ.

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The volume of the same gas is 320 L.

Use the combined gas law to solve for the final volume of the gas:

(P1V1/T1) = (P2V2/T2)

Substituting the given values, we get:

Solving for V2, we get:

Therefore, the volume of the gas at the new conditions is 320 L.

The combined gas law relates the pressure, volume, and temperature of a gas in a closed system. It states that the product of pressure and volume divided by the temperature is a constant for a given mass of gas in a closed system undergoing changes in pressure, volume, and temperature. Mathematically, the combined gas law can be represented as:

Where P₁ and V₁ are the initial pressure and volume, T₁ is the initial temperature, P₂ and V₂ are the final pressure and volume, and T₂ is the final temperature. This equation is useful in predicting the behavior of gases when the conditions of pressure, volume, and temperature are changed. The combined gas law is a combination of Boyle's law, Charles's law, and Gay-Lussac's law, and it can be derived from the ideal gas law.

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There are several definitions of acids and bases, and each definition provides a unique perspective on their properties and behaviors.

Arrhenius Definition:

According to the Arrhenius definition, an acid is a substance that dissociates in water to form hydrogen ions (H+), while a base is a substance that dissociates in water to form hydroxide ions (OH-).

For example, hydrochloric acid (HCl) dissociates in water to form H+ and Cl- ions:

HCl → H+ + Cl-

On the other hand, sodium hydroxide (NaOH) dissociates in water to form Na+ and OH- ions:

NaOH → Na+ + OH-

Characteristics for identification:

Acids typically have a sour taste and can cause a burning sensation on the skin. Bases have a bitter taste and can feel slippery to the touch. They also typically have a higher pH value (greater than 7) in aqueous solutions.

Bronsted-Lowry Definition:

According to the Bronsted-Lowry definition, an acid is a substance that donates a proton (H+) to another molecule or ion, while a base is a substance that accepts a proton (H+) from another molecule or ion.

In this reaction, acetic acid is the acid because it donates a proton, while water is the base because it accepts a proton.

Characteristics for identification:

Acids and bases in the Bronsted-Lowry sense are identified by the presence or absence of a hydrogen ion. An acid must contain a hydrogen ion that can be donated to a base, while a base must have an available lone pair of electrons to accept a hydrogen ion.

Lewis Definition:

According to the Lewis definition, an acid is a substance that accepts a pair of electrons, while a base is a substance that donates a pair of electrons.

In this reaction, boron trifluoride is the acid because it accepts a pair of electrons, while ammonia is the base because it donates a pair of electrons.

Characteristics for identification:

Acids and bases in the Lewis sense are identified by their electron-pair accepting or donating abilities. An acid must be able to accept a pair of electrons, while a base must be able to donate a pair of electrons.

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Correct Question:

Explain the different definitions of acid and base. Give an example of each and the characteristics of your identification.

0.0228 mol/kg is the molality of a solution containing 4. 0 grams of NaCl dissolved in 3000 grams of water.

To calculate the molality of a solution, we need to first convert the mass of the solute (NaCl) to moles and then divide by the mass of the solvent (water) in kilograms.

The molar mass of NaCl is 58.44 g/mol, so 4.0 grams of NaCl is equal to 0.0684 moles of NaCl.

The mass of water is 3000 grams or 3.0 kg.

Therefore, the molality of the solution is:

molality = moles of solute / mass of solvent in kg

molality = 0.0684 moles / 3.0 kg

molality = 0.0228 mol/kg

So the molality of the solution is 0.0228 mol/kg.

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The concentration of the reactant after precisely two days is 4.62 M.

For a zero-order reaction, the rate is independent of the concentration and is given by the expression:

rate = k

where k is the rate constant.

The integrated rate law for a zero-order reaction is:

[A] = -kt + [A]₀

where [A] is the concentration of the reactant at time t, [A]₀ is the initial concentration of the reactant, k is the rate constant, and t is time.

Substituting the given values into the equation, we get:

[A] = -kt + [A]₀

[A] = -0.0119 M/hr * (224 hr) + 5.19 M

[A] = -0.5712 M + 5.19 M

[A] = 4.6188 M

Rounding off to three significant figures and two decimal places, we get the final concentration as 4.62 M.

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