10) For the balanced equation (with hypothetical 'chemicals'):
3F+ 2H-> P + 2S
Exp#
1
2
3
[F](mol/L)
0.000345
initial rate (M/sec)
3.24 x 100
0.000690
3.24 x 108
0.000690
3.24 x 10-7
a. What is the rate law equation for this reaction using the given data?
[H](mol/L)
0.000765
0.000765
0.00765
b. Calculate the rate constant.

A. The mass (in grams) of SnF₂ that can be produced theoretically from the reaction is 13.20 g

B. The percentage yield of the reaction is 83.3%

The mass of SnF₂ produced theorethically, can be obtained as shown below:

Sn + 2HF ->  SnF₂ +  H₂

From the balanced equation above,

118.71 g of Sn reacted to produce 156.71 g of SnF₂

Therefore,

10 g of Sn will react to produce = (10 × 156.71) / 118.71 = 13.20 g of SnF₂

Thus, the mass of SnF₂ produced is 13.20 g

The percentage yield for the reaction can be obtained as follow:

Percentage yield = (Actual /Theoretical) × 100

Percentage yield of SnF₂ = (11 / 13.20) × 100

Percentage yield of SnF₂ = 83.3%

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Complete question:

See attached photo

The new volume [tex]V_{2}[/tex]) of the gas is approximately 1710 L when the temperature changes from 42 ∘C to 94 ∘C, assuming no change in pressure or amount of gas.

What is Temperature?

Temperature is a measure of the average kinetic energy of the particles in a substance, such as a gas, liquid, or solid. It is commonly measured in Celsius (°C), Fahrenheit (°F), or Kelvin (K) scales. Temperature determines the direction of heat transfer, which is the movement of energy between substances due to a temperature difference.

To use the ideal gas law, we need to convert the temperatures to Kelvin by adding 273.15 to each:

[tex]T_{1}[/tex] = 42 + 273.15 = 315.15 K

[tex]T_{2}[/tex]= 94 + 273.15 = 367.15 K

Since the pressure, amount of gas, and ideal gas constant remain constant in this problem, we can set up the following ratio:

([tex]V_{1}[/tex] / [tex]T_{1}[/tex]) = ([tex]V_{2}[/tex]/ [tex]T_{2}[/tex])

Plugging in the values:

(1.47 ×[tex]10^{3}[/tex]L / 315.15 K) = ([tex]V_{2}[/tex] / 367.15 K)

Now we can solve for [tex]V_{2}[/tex]:

[tex]V_{2}[/tex] = 1.47×[tex]10^{3}[/tex] L * 367.15 K / 315.15 K

[tex]V_{2}[/tex]≈ 1710 L (rounded to three significant figures)

Therefore, the new volume (V2) of the gas is approximately 1710 L when the temperature changes from 42 ∘C to 94 ∘C, assuming no change in pressure or amount of gas.

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The reactions with a positive Δrxn are:

A(g) + B(g) ⟶ 3C(g)

A(s) + B(s) ⟶ C(g)

The entropy change (Δrxn) of a reaction indicates the change in the degree of randomness or disorder of the system during the reaction. If the number of product molecules is greater than the number of reactant molecules, the disorder of the system usually increases, resulting in a positive Δrxn. Therefore, we can determine the answer by analyzing the stoichiometry of each reaction:

A(g) + B(g) ⟶ C(g)

In this reaction, the number of product molecules is less than the number of reactant molecules, so the disorder of the system decreases. Therefore, this reaction has a negative Δrxn.

A(g) + B(g) ⟶ 3C(g)

In this reaction, the number of product molecules is greater than the number of reactant molecules, so the disorder of the system increases. Therefore, this reaction has a positive Δrxn.

A(s) + B(s) ⟶ C(g)

In this reaction, the solid reactants are combining to form a gaseous product. The disorder of the system is expected to increase, resulting in a positive Δrxn.

2A(g) + B(g) ⟶ C(g)

In this reaction, the number of product molecules is less than the number of reactant molecules, so the disorder of the system decreases. Therefore, this reaction has a negative Δ rxn.

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To determine the size of the entire population: In the equation N = M, replace the variables of M solutions, R (number all marked recaptured), with T (total recaptured during second visit). T R = frac M T R N = RMT.

In order for the mark-recapture method to function, it must be assumed that the proportion the marked organisms that are recaptured inside the second sample corresponds to that of the original marked in the entire population. This equation R(recaptured)/C(captured in second sample)=M(marked initially)/N) illustrates this (total number in population).

It has been suggested that capture-recapture techniques be used to gauge a register's degree of completeness. These techniques were initially created to determine how big a confined animal colony was. The process aims to capture, tag, and release as many animals is possible in a given region all at once. This is known as the "capture" stage.

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The molar mass of hydrogen is approximately 1 g/mol. This means that 1 mole of hydrogen atoms has a mass of 1 gram. So, to find the number of atoms in 20 grams of hydrogen, we need to first find how many moles of hydrogen there are, using the following equation:

moles of hydrogen = mass of hydrogen / molar mass of hydrogen

Plugging in the values, we get:

moles of hydrogen = 20 g / 1 g/mol = 20 mol

So there are 20 moles of hydrogen present in 20 g of hydrogen.

Finally, we can find the number of atoms of hydrogen using Avogadro's number, which gives the number of particles (such as atoms, molecules, or ions) in one mole of a substance. Avogadro's number is approximately 6.02 x 10^23 particles per mole. So we can find the number of atoms of hydrogen as follows:

number of atoms of hydrogen = moles of hydrogen x Avogadro's number

Plugging in the values, we get:

number of atoms of hydrogen = 20 mol x 6.02 x 10^23 atoms/mol

number of atoms of hydrogen = 1.204 x 10^25 atoms

Therefore, there are approximately 1.204 x 10^25 atoms of hydrogen in 20 g of H2.

The standard change in Gibbs free energy for the given reaction at 25°C is -757.9 kJ/mol.

Gibbs energy, also known as Gibbs free energy, is a thermodynamic quantity used to determine the maximum amount of work that can be obtained from a system at a constant temperature and pressure. It is denoted by the symbol G and is named after the American physicist Josiah Willard Gibbs who introduced the concept in the late 19th century.

Gibbs energy is defined as the difference between the enthalpy of a system and the product of the temperature and the entropy of the system:

G = H - TS

where H is the enthalpy, T is the temperature in Kelvin, and S is the entropy of the system.

The Gibbs energy is related to the equilibrium constant of a reaction through the following equation:

ΔG = -RTlnK

To calculate the standard change in Gibbs free energy for the given reaction at 25°C, we need to use the ΔG°f values (standard Gibbs free energy of formation) for the reactants and products involved in the reaction.

The ΔG°f values for Fe₂O₃(s), Al(s), Al₂O₃(s), and Fe(s) can be found in a table of thermodynamic data and are:

ΔG°f [Fe₂O₃(s)] = -824.2 kJ/mol

ΔG°f [Al(s)] = 0 kJ/mol

ΔG°f [Al₂O₃(s)] = -1582.3 kJ/mol

ΔG°f [Fe(s)] = 0 kJ/mol

The standard change in Gibbs free energy for the reaction can be calculated using the following equation:

Δ°rxn = ΣΔG°f(products) - ΣΔG°f(reactants)

Substituting the values, we get:

Δ°rxn = [ΔG°f(Al₂O₃(s)) + 2ΔG°f(Fe(s))] - [ΔG°f(Fe₂O₃(s)) + 2ΔG°f(Al(s))]

Δ°rxn = [(-1582.3 kJ/mol) + 2(0 kJ/mol)] - [(-824.2 kJ/mol) + 2(0 kJ/mol)]

Δ°rxn = -757.9 kJ/mol

Therefore, the standard change in Gibbs free energy for the given reaction at 25°C is -757.9 kJ/mol.

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A compound formed between two or more non-metal elements that share electrons is called a covalent compound or a molecular compound.

In covalent compounds, the atoms share electrons in order to achieve a full outer shell of electrons and become more stable. Covalent compounds typically have low melting and boiling points, are often gases or liquids at room temperature, and are poor conductors of electricity. Examples of covalent compounds include water (H2O), carbon dioxide (CO2), and methane [CH4].

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four score and seven years ago (our father) brought this continent, a new nation,

When 3 g of a petroleum are burned with more oxygen than is required, 8.8 g of Atmospheric carbon dioxide plus 5.4 g liquid [tex]H_{2}O[/tex] are produced.

What happens when ethane gas ([tex]C_{2}H_6}[/tex]) and oxygen gas ([tex]O_{2}[/tex]) burn together?

Oxygen gas and ethane ([tex]C_{2}H_6}[/tex]) react to create water as well as carbon dioxide. Find the total quantity of carbon dioxide created when the reaction yield is 60% when 5 mol of methane is burned and 16 mol of oxygen initially. 2[tex]C_{2}H_4}[/tex]+7[tex]O_{2}[/tex] →4[tex]CO_{2}[/tex]+6[tex]H_{2}O.[/tex]

How many tumours of CO2 are created when 2.2 blackheads of [tex]C_{2}H_4}[/tex]are burned?

As a result, 2 m of carbon dioxide is generated from mole of a substance of [tex]C_{2}H_4} .[/tex] Thus, multiply 2.2 over 2 by 1 pot to get 2.2 moles for c into h or just a cross. It consists of 4.4 moles of carbon.

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463.5 grams of HCl are required to react with 6.35 moles of CaCO₃.

Mass of one mole of substance is referred to as the molar mass. The molar mass of a substance can be calculated by adding up the atomic masses of all the atoms in a molecule.

Balanced chemical equation for the reaction between calcium carbonate (CaCO₃) and hydrochloric acid (HCl) is: CaCO₃ + 2HCl → CaCl₂ + H₂O + CO₂

6.35 mol CaCO₃ * 2 mol HCl / 1 mol CaCO₃ = 12.7 mol HCl

Now, we use the molar mass of HCl (36.46 g/mol) to convert from moles to grams: 12.7 mol HCl * 36.46 g/mol = 463.5 g HCl

Therefore, 463.5 grams of HCl are required to react with 6.35 moles of CaCO₃.

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The reaction [tex]2NH_3=N_2H_4+H_2[/tex] has a standard reaction free energy of -62.4 kJ/mol.

Energy is the capacity to carry out tasks or affect change. It comes in a variety of shapes and sizes, including kinetic energy (energy of motion), potential energy (stored energy of position), thermal energy (heat), electrical, chemical, and nuclear energy. Energy is required for the survival and growth of all living things. Additionally, it is necessary for the operation of industries and equipment.

Equation can be used to get a reaction's standard reaction free energy.

ΔG°rxn = ΣΔG°f (products) - ΣΔG°f (reactants).

For the reaction [tex]2NH_3=N_2H_4+H_2[/tex], the ΔG°f values are as follows:

ΔG°f ([tex]2NH_3[/tex]) = -46.2 kJ/mol

ΔG°f ([tex]N_2H_4[/tex]) = -20.8 kJ/mol

ΔG°f ([tex]H_2[/tex]) = 0 kJ/mo

The equation yields the average reaction free energy (ΔG°rxn) of the reaction is:

ΔG°rxn = (2 x -20.8) - (-46.2)

            = -62.4 kJ/mol

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A concentrated saltwater solution weighing 29.97 g and fitting into a flask to the mark of 25.0 ml has a density of about 1199.2 g/L.

By dividing the solution's mass by its volume, we may get its density: density = mass/volume

We need to know the density of water at the solution's temperature as well as the capacity of the flask up to the 25.0 ml level in order to calculate the volume of the solution.

Since 1 mL = 0.001 L, volume is equal to 25.0 mL, or 0.0250 L.

Now, we may determine the solution's density as follows:

1199.2 g/L or 29.97 g/0.0250 L is what is referred to as density.

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C and O since their electronegativity differs by quite a lot

I think it is Ba since the radius increases along the group.but decreases along the period

Answer:

Ba

Explanation:

Ba

Under the given circumstances, the pressure difference between methane and an ideal gas is 58.5 atm.

An ideal gas is a theoretical gas composed of a large number of small particles that have zero volume, do not interact with each other, and are in constant random motion. The behavior of an ideal gas is described by the ideal gas law, which relates the pressure, volume, temperature, and number of moles of the gas.

The van der Waals equation can be used to figure out the pressure difference between methane and an ideal gas under these circumstances:

(P + a n² / V²)(V - n b) = n R T

where P is the pressure, n is the number of moles, V is the volume, T is the temperature in Kelvin, R is the ideal gas constant (0.08206 L·atm/K·mol), a and b are the van der Waals constants for methane.

First, we can calculate the pressure of an ideal gas under these conditions using the ideal gas law:

P = n R T / V

P = (15.0 mol) (0.08206 L·atm/K·mol) (293.45 K) / (6.00 L)

P = 299.8 atm

Next, we can use the van der Waals equation to calculate the pressure of methane under these conditions:

(P + a n² / V²)(V - n b) = n R T

(P + (2.300 L²·atm/mol²) (15.0 mol)² / (6.00 L)²) ((6.00 L) - (15.0 mol) (0.0430 L/mol)) = (15.0 mol) (0.08206 L·atm/K·mol) (293.45 K)

Simplifying the equation gives:

P + 1.319 atm = 359.6 atm

P = 358.3 atm

As a result, under these circumstances, the pressure difference between methane and an ideal gas is:

ΔP = P (methane) - P (ideal gas) = 358.3 atm - 299.8 atm = 58.5 atm.

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0.20 g of methane gas at 312 K and 2.00 atm occupies a volume of 0.13 L (rounded to two significant figures).

What is volume?

To solve this problem, we can use the ideal gas law, which relates the pressure, volume, temperature, and number of moles of a gas:

PV = nRT

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

First, we need to calculate the number of moles of methane gas:

n = m/MW

where m is the mass of the gas (0.20 g) and MW is the molecular weight of methane (16.04 g/mol).

n = 0.20 g / 16.04 g/mol = 0.0125 mol

Next, we can rearrange the ideal gas law to solve for the volume:

V = nRT/P

Plugging in the values we have:

V = (0.0125 mol)(0.0821 L·atm/mol·K)(312 K)/(2.00 atm)

V = 0.128 L

Therefore, 0.20 g of methane gas at 312 K and 2.00 atm occupies a volume of 0.13 L (rounded to two significant figures).

What is molecular weight ?

Molecular weight, also known as molecular mass, is the mass of a molecule, which is the sum of the masses of all the atoms in the molecule. It is typically expressed in atomic mass units (amu) or in grams per mole (g/mol). The molecular weight is an important property of a substance in chemistry, as it is used to calculate various properties such as the molar mass, molar volume, and stoichiometric relationships in chemical reactions.

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Complete question is:  0.13 L volume does 0.20 g methane gas (CH4) occupy at 312 K and 2.00 atm.

Answer: The units for molarity are moles/liter.

Similarly, the equation to find molarity is moles divided by liters.

Explanation:  

mol / L is a unit of molar concentration. These are the number of moles of dissolved material per liter of solution. 1 mol / L is also called 1M or 1molar. Mol / m3 is also a unit of molar concentration.

Molarity is expressed in units of moles per liter (mol / L). This is a very common unit, so it has its own symbol, which is the uppercase M. A solution with a concentration of 5 mmol / l is called a 5 M solution or has a concentration value of 5 mol.

The molar concentration of the solution is equal to the number of moles of the solute divided by the mass of the solvent (kilogram), and the molar concentration of the solution is equal to the number of moles of the solute divided by the volume of the solution (liter). increase.

A)  the activation energy is  = 66.5 kJ/mol

B) the slope of the line in this case would be -8000 K^-1

C)  the temperature at which the rate constant is 1.00x10^-3 M^-1 x s^-1 is 408 K (135°C).

a) To calculate the activation energy, we can use the Arrhenius equation:

k = Ae^(-Ea/RT)

where k is the rate constant, A is the pre-exponential factor, Ea is the activation energy, R is the gas constant (8.314 J/mol x K), and T is the temperature in Kelvin.

Taking the natural logarithm of both sides of the equation, we get:

ln(k) = ln(A) - (Ea/RT)

We can use the two sets of data to set up two equations:

ln(k1) = ln(A) - (Ea/RT1)

ln(k2) = ln(A) - (Ea/RT2)

Solving for Ea by taking the difference between the two equations:

ln(k2/k1) = (Ea/R) [(1/T1) - (1/T2)]

Ea = -R ln(k2/k1) / [(1/T1) - (1/T2)]

Plugging in the values:

Ea = -8.314 J/mol x K x ln(2.07x10^-2 / 3.97x10^-3) / [(1/398 K) - (1/398 K)]

Ea = 66.5 kJ/mol

b) In an Arrhenius plot, ln(k) is plotted against 1/T, and the slope of the line is equal to -Ea/R. Therefore, the slope of the line in this case would be:

slope = -Ea/R = -(66.5 x 10^3 J/mol) / (8.314 J/mol x K) = -8000 K^-1

c) To solve for the temperature at which the rate constant is 1.00x10^-3 M^-1 x s^-1, we can rearrange the Arrhenius equation:

k = Ae^(-Ea/RT)

ln(k) = ln(A) - (Ea/RT)

1/T = (ln(k) - ln(A)) / (-Ea/R)

T = -R / (Ea ln(k) - ln(A))

Plugging in the values:

T = -8.314 J/mol x K / [(66.5 x 10^3 J/mol) ln(1.00x10^-3) - ln(3.97x10^-3)]

T = 408 K

Therefore, the temperature at which the rate constant is 1.00x10^-3 M^-1 x s^-1 is 408 K (135°C).

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The volume of [tex]SO_{3}[/tex] would be produced by complete reaction of 100cm3 of [tex]H_{2}O[/tex]with [tex]O_{2}[/tex] is at STP is 60.03L.

22.4 L divided by 2.68 moles per mole yields 60.03 L [tex]SO_{3}[/tex].

describing the elements contributing to the response,

[tex]2SO_{2(g)}+ O_{2} = 2SO_{3}[/tex]

In this instance, [tex]SO_{3}[/tex] and [tex]O_{2}[/tex] have a mole ratio of 2:1. Assume the reaction takes place at STP, where 1 mole of any gas has a volume of 22.4 L. Consequently, 30 [tex]dm^{3}[/tex]of [tex]O_{2}[/tex] (1 dm3 = 1 L) equals 30 L of [tex]O_{2}[/tex] and 30 L/22.4 L times 1 mole equals 1.34 moles of [tex]O_{2}[/tex].

According to stoichiometry, when 1.34 moles of [tex]O_{2}[/tex]are reacted with [tex]SO_{2}[/tex], 2.68 moles of [tex]SO_{3}[/tex] are created, or 2/1 x 1.34 moles of [tex]SO_{3}[/tex].

This means that the amount of [tex]SO_{3}[/tex]produced will be (2.68 moles/1 mole) x 22.4 L = 60.03 L [tex]SO_{3}[/tex].

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Explanation: the answer is 3840 because 2950+890=3840

The molality of the solution is 1.080 mol/kg of a 48 grams of MgCl2 is dissolved in 500g of water, density of water = 1 kg/1L.

Taking the moles of solute and dividing it by the kilograms of solvent yields the molality of a solution.

Molality is calculated as follows: kg of solvent/kg of solute

500 g, or 0.500 kg, is the mass of the solvent.

MgCl2 molecular weight divided by its mass gives the amount of moles.

48 g / 95.2 g m o l 1 equals the quantity of moles of magnesium chloride.

0.504 moles of MgCl2 are present in one mole.

Molality is calculated as 0.504moles per kilogram.

Molality is equal to 1.080 mol k g 1.

As stated in the definition, molality is the "total moles of a solute contained in a kilogram of a solvent." The terms "molality" and "molal concentration" are synonymous. It is a measurement of a solvent.

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Answer: Oxygen (??)

Explanation: Im not sure but smth like H2O (my brain is not braining T-T)

The number of mole of H₃PO₄ that can be formed from the reaction of 2 moles of P₄O₁₀ and 8 moles of H₂O is 5.33 moles

First, we shall determine the limiting reactant. Details below

P₄O₁₀ + 6H₂O -> 4H₃PO₄

From the balanced equation above,

1 mole of P₄O₁₀ reacted with 6 moles of H₂O

Therefore,

2 moles of P₄O₁₀ will react with = 2 × 6 = 12 moles of H₂O

From the above calculation, we can see that a higher amount of H₂O is needed to react completely with 2 moles of P₄O₁₀

Thus, H₂O is the limiting reactant.

Now, we shall determine the mole of H₃PO₄ formed from the reaction. Details below:

P₄O₁₀ + 6H₂O -> 4H₃PO₄

From the balanced equation above,

6 moles of H₂O reacted with 4 moles of H₃PO₄

Therefore,

8 moles of H₂O will react with = (8 × 4) / 6 = 5.33 moles of H₃PO₄

Thus, the mole of H₃PO₄ formed is 5.33 moles

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The amount that would remain, given that 3 half-lives has pass when you started with 20.0 g is 2.50 grams (1st option)

The following data were obtained from the question:

The amount remaining can be obtained as shown below:

N = N₀ / 2ⁿ

N = 20 / 2³

N = 20 / 8

N = 2.50 grams

Thus, we can conclude from the above calculation that the amount that would remain after 3 half-lives to pass is 2.50 grams (1st option)

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Answer:

2.50g

Explanation:

Answer:  the temperature of the gas is approximately 16.1°C.

Explanation: PV=nRT Rearranging the equation gives us T = PV/(nR), with all variables defined as before. Convert mL to L: V = 4191 mL = 4.191 L. Use equation: T = (89.9 atm) x (4.191 L) / (2.6 mol x 0.08206 L atm/(mol K)). Simplify to get T = 289.2 K. Convert Kelvin to Celsius: T = 289.2 K - 273.15 = 16.1°C.

Answer:

strength in ionic compounds.

Explanation:

:)

Lattice energy is an estimate of the bond of strength. It denotes the amount of energy required to break down one mole of a solid ionic compound into its constituent gaseous ions.

The strength of an ionic compound's ionic bonds is measured by lattice energy. It explains several properties of ionic solids, including their volatility, solubility, and hardness. An ionic solid's lattice energy cannot be measured directly.

The higher an ionic compound's lattice energy, the more difficult it is to disassemble the crystal lattice structure and dissolve it in water. As a result, compounds with high lattice energies are less soluble in water than those with low lattice energies.

The value of lattice energy is determined by the charges on the two ions as well as the distance between them. The distance between the ions is directly proportional to their size.

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Complete question:

Lattice energy is an estimated bond of the bond:

A. conductivity

B. group

C. length

D. strength

Choose the correct option.

You can only get 1 mole of ammonia (NH3) since NH2 is the limiting reactant