Identifying Types of Sound Waves Complete the passage. Sound waves and some earthquake waves are waves are waves. waves. Ocean, light, and other earthquake​

Answer:

The reaction between zinc and hydrochloric acid produces hydrogen gas according to the following equation:

Zn + 2HCl → ZnCl2 + H2

This equation tells us that 1 mole of zinc reacts with 2 moles of hydrochloric acid to produce 1 mole of hydrogen gas. The molar mass of zinc is 65.38 g/mol, and the molar mass of hydrogen is 1.008 g/mol.

Using this information, we can set up the following proportion to find the number of grams of zinc needed to produce 8.08 grams of hydrogen:

1 mole Zn / 2 moles H2 = 65.38 g Zn / 1 mole Zn

x grams Zn / 8.08 g H2 = 65.38 g Zn / 1 mole Zn

Solving for x, we get:

x = (8.08 g H2) x (1 mole Zn / 2 moles H2) x (65.38 g Zn / 1 mole Zn)

x = 261.7 g

Therefore, you would need 261.7 grams of zinc to produce 8.08 grams of hydrogen.

Explanation:

Answer:

Most energy Si> CCl4 > Ar least energy

Explanation:

The strength of a bond is proportional to its bond/attraction energy. This means the molecule with the strongest bonds will have the strongest energy.

We know that Si has the strongest bonds because each atom in the compound is bonded tightly enough that it is solid. Recall that a solid has molecules closer and and more tightly bonded than in a liquid or gas, when the molecules move freer.

With this in mind, we know that Ar has the weakest attraction strength, and thus weakest energy of attraction, because it is a gas and that atoms move freely and interact minimally. There is not enough attraction for the molecules to form bonds nor to effect one another beyond accidental collisions.

The first image illustrates the variation in the pressure, volume, and temperature of given masses of gases.

The second picture illustrates the cooling/heating curve of a substance.

The third picture illustrates the increase in the volume of a gas in a balloon with the increase in temperature.

The fourth picture shows the increase and decrease in the volume of a gas with temperature.

The volume of a gas is inversely related to its pressure and directly related to its temperature and mass.

The kinetic energy of the gas molecules increases together with the temperature, as does their velocity. Additionally, the intermolecular forces between the molecules loosen, causing the spaces between the molecules to widen and the volume to rise.

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The hydrolysis of 2-methylpropionic acid nitrile in acidic conditions proceeds through an acid-catalyzed mechanism.

The mechanism can be described as follows:

The hydrolysis of 2-methylpropionic acid nitrile in acidic conditions results in the conversion of the nitrile group to a carboxylic acid group through the addition of a water molecule and subsequent proton transfer steps. This reaction is commonly used in the synthesis of carboxylic acids from nitriles, and is an important process in organic chemistry.

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For our purposes, we'll rearrange the specific heat equation to produce the temperature rise (T=Q mc T = Q m c), then use it in combination with a revised equation for the temperature change to determine the ultimate temperature (T=Ti+T T f = T i + T).

The first container's mass and temperature are multiplied together, and the result is added to the second container's mass and temperature to determine the mixture's water temperature. Finally, divide that outcome by the combined water masses in each container.

Accordingly, 1 g of  has 540 calories of heat energy in excess of 1 g of water.

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0.375 moles of SnF_2 are produced from the reaction of 30g of HF.

When a substance undergoes a chemical transformation, its chemical identity changes. Rust is one illustration of this. An iron nail rusts, turning brown-red, when it comes into touch with water and is then exposed to air. The chemical makeup of the original material is altered throughout this process.

To determine the moles of SnF2:

[tex]SnO_2(s) + 4HF(aq) = > SnF_2(s) + 2H_2O(l)[/tex]

From the balanced equation,

Now, we have to calculate the number of moles of HF from the given mass of 30g:

30g HF x (1 mol HF/20.01 g HF) = 1.50 mol HF

So, we have 1.50 mol of HF.

Applying the stoichiometry from the balanced chemical equation,

1.50 mol HF x (1 mol SnF2/4 mol HF) = 0.375 mol SnF2

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van 't Hoff factor for ionic compound [tex]K_{2}[/tex]S is 3.

Define van 't Hoff factor  

The van 't Hoff factor is the difference between the concentration of a material determined by its mass and the concentration of particles actually formed when the substance is dissolved. The van 't Hoff factor is virtually 1 for the majority of non-electrolytes dissolved in water.

The van 't Hoff factor for the majority of ionic compounds dissolved in water is equal to the number of discrete ions in the substance's formula unit. Only perfect solutions can claim this as ion pairing occasionally happens in solutions. Only a small portion of the ions are ever coupled and count as a single particle at any given time. In all electrolyte solutions, ion pairing takes place to some extent.

[tex]K_{2}[/tex]S ⇒ 2K+ + S2-

[tex]K_{2}[/tex]S dissolves into 3 particles .

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The Vant Hoff factor as [tex]K_{2}S[/tex] break into in water is 3

What does vant Hoff factor mean?

The ratio of a substance's mass concentration to the concentration of the particles that are produced when it dissolves is known as the Van't Hoff factor. The Van't Hoff factor describes how much a substance associates or dissociates in a solution.

The ratio of the final moles following dissociation or association to the beginning moles before to dissociation or association of an electrolyte in a solution is known as the Van't Hoff factor. The solute's property governs the number of particles, which is independent of the solution's concentration.

[tex]K_{2}S[/tex] ⇒ 2K+ + -[tex]S_{2}[/tex]

[tex]K_{2}S[/tex] dissolves into 3 particles .

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The new pressure of the balloon, given that  the temperature increases to 32 °C causing the balloon to expand to 2.2 L is 268.97 atm

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

The combined gas equation states shown as below:

P₁V₁ / T₁ = P₂V₂ / T₂

Inputting the various parameters, we can obtain the new pressure as follow:

(385 × 1.5) / 298 = (P₂ × 2.2) / 305

Cross multiply

298 × 2.2 × P₂ = 385 × 1.5 × 305

Divide both sides by (298 × 2.2)

P₂ = (385 × 1.5 × 305) / (298 × 2.2)

P₂ = 268.97 atm

Thus, from the above calculation, it is evident tha the new pressure of the balloon is 268.97 atm

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According to specific heat capacity, the ΔH of reaction  in kJ/mol water formation is- 1.575 kJ/mol.

Specific heat capacity is defined as the amount of energy required to raise the temperature of one gram of substance by one degree Celsius. It has units of calories or joules per gram per degree Celsius.

It varies with temperature and is different for each state of matter. Water in the liquid form has the highest specific heat capacity among all common substances .Specific heat capacity of a substance is infinite as it undergoes phase transition ,it is highest for gases and can rise if the gas is allowed to expand.

It is given by the formula ,

Q=mcΔT it can also be replaced as ΔH= -mcΔt= -0.150×4.2×2.5= - 1.575 where m= 0.250-0.100=0.150.

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Answer: 2310

Explanation:

PV=nRT therefore V=nRT/

n= 7.70 moles

P= 0.0900atm

T= 56.O°C or 329.15K

R= 0.08206

V= ((7.70)(0.08206)(329.15))/0.0900

V= 2310

First, we need to calculate the heat absorbed by the water:

q = m × c × ΔT

where q is the heat absorbed, m is the mass of water, c is the specific heat of water, and ΔT is the change in temperature.

q = 145 g × 4.184 J/g°C × (63.0°C - 24.5°C)

q = 16394.12 J

Next, we need to calculate the amount of substance of MgBr₂ that was added to the water:

n = m/MW

where n is the amount of substance, m is the mass of MgBr₂, and MW is the molecular weight of MgBr₂.

MW(MgBr₂) = 184.11 g/mol

n = 23.2 g ÷ 184.11 g/mol

n = 0.1259 mol

Finally, we can calculate the enthalpy of solution, ΔH, using the following formula:

ΔH = q ÷ n

where ΔH is the enthalpy of solution.

ΔH = 16394.12 J ÷ 0.1259 mol

ΔH = 130233.72 J/mol

Converting to kilojoules per mole (kJ/mol):

ΔH = 130.23 kJ/mol

Therefore, the enthalpy of solution for dissolving magnesium bromide in water is 130.23 kJ/mol.

The enthalpy of solution of magnesium bromide in water is calculated using the formula for heat transfer and taking into account the mass of the solvent, the specific heat of the solvent, and the change in temperature. The result is 186 kJ/mol.

To calculate the enthalpy of solution of magnesium bromide (MgBr₂), we need to use the formula for heat transfer: Q = m * c * ΔT, where m is the mass of the solvent (water), c is the specific heat of the solvent, and ΔT is the change in temperature.

In our case, the mass of water is 145g, the specific heat of water (c) is 4.18 J/g°C, and the change in temperature (ΔT) is 63.0 °C - 24.5 °C = 38.5 °C.

Using the formula Q = m * c * ΔT, we can calculate the heat transferred to the water: Q = 145g * 4.18 J/g°C * 38.5 °C = 23432 J or 23.432 kJ. This is the heat absorbed by the water.

The enthalpy of the solution is defined as the amount of heat absorbed (or released) when one mole of a substance is dissolved in water. So, to find the enthalpy of solution, we first need to convert the grams of MgBr₂ to moles. The molar mass of MgBr₂ is 184.11 g/mol, so 23.2 g of MgBr₂ is 23.2 g / 184.11 g/mol = 0.126 mol.

Now we can calculate the enthalpy change by dividing the heat absorbed by the moles of the solute: ΔH = Q / n = 23.432 kJ / 0.126 mol = 186 kJ/mol. Therefore, the enthalpy of solution for magnesium bromide in water is 186 kJ/mol.

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The mass (in grams) of Cu(OH)₂ that can be made when you mix 374.48 mL of 1.451 M NaOH with excess CuCl₂ is 52.98 grams

First, we shall determine the mole present in 374.48 mL of 1.451 M NaOH Details below:

Molarity = Mole / Volume

Cross multiply

Mole of NaOH = molarity × volume

Mole of NaOH = 1.451 × 0.37448

Mole of NaOH = 0.543 mole

Next, we shall determine the mole of Cu(OH)₂ obtained from the reaction. Details below:

CuCl₂ + 2NaOH -> Cu(OH)₂ + 2NaCl

From the balanced equation above,

1 moles of NaOh reacted to produce 1 mole of Cu(OH)₂

Therefore,

0.543 mole of NaOH will also react to produce 0.543 mole of Cu(OH)₂

Finally, we shall determine the mass of Cu(OH)₂ obtained from the reaction. Details below:

Molar mass of Cu(OH)₂ = 97.56 g/mol

Mole of Cu(OH)₂ = 0.543

Mass of Cu(OH)₂ = ?

Mole = mass / molar mass

0.543 = Mass of Cu(OH)₂ / 142

Cross multiply

Mass of Cu(OH)₂ = 0.543 × 97.56

Mass of Cu(OH)₂ = 52.98 grams

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As photons of light leave the core, they collide with electrons and atomic nuclei, scattering off each one.

Rays are straight lines that light waves that move in from their source. Rays do not curve around corners, therefore when they come into contact with an opaque object (one that does not allow light to flow through it), they are prevented from reaching the other side.

Light travels in a straight line until it encounters a new medium, whether it be in air, water, glass, diamond, a smokey Broadway stage, or any other transparent substance (or in nothing — the vacuum of space). The path of light is the Ultimate Straight Line, so straight that analogies fail.

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Saponification number = (V × M × F × 56.1) / W

Where:

V = volume of HCl used in the back titration

M = molarity of HCl

F = factor of KOH (which is 1 for pure KOH)

W = weight of the butter sample used in grams

First, we need to calculate the amount of KOH used in the saponification reaction:

0.5131 M KOH = 0.5131 moles KOH / liter

25.00 mL KOH = 0.02500 L KOH

moles KOH used = 0.5131 moles/L × 0.02500 L = 0.0128 moles KOH

Since the saponification reaction is a 1:1 reaction between KOH and the triacylglycerol in the butter sample, the amount of butter used is also 0.0128 moles.

Next, we need to calculate the amount of HCl that reacted with the excess KOH:

0.5000 M HCl = 0.5000 moles HCl / liter

10.26 mL HCl = 0.01026 L HCl

moles HCl used = 0.5000 moles/L × 0.01026 L = 0.00513 moles HCl

Since the reaction between HCl and KOH is also a 1:1 reaction, the moles of KOH that were not used in the saponification reaction is equal to the moles of HCl used in the back titration:

moles KOH not used = moles HCl used = 0.00513 moles HCl

To find the saponification number,

Saponification number = (V × M × F × 56.1) / W

Saponification number = (0.01026 L × 0.5000 moles/L × 1 × 56.1) / 2.085 g

Saponification number = 6.50

Therefore, the saponification number for this sample of butter is 6.50.

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The balanced equation for the reaction is written as:

C + 2ZnO -> CO₂ + 2Zn

Chemical equation equation basically has two sides. These are the reactants and products

Reactants -> Products

The balancing of chemical equation is done by ensuring that the number of atoms of the reactants is equal to the number of atoms of the products.

Now, we shall write the balance the equation as follow:

C + ZnO -> CO₂ + Zn

There are 2 atoms of O on the right side and 1 atom on the left side. It can be balanced by writing 2 before ZnO as shown below:

C + 2ZnO -> CO₂ + Zn

There are 2 atoms of Zn on the left side and 1 atom on the right side. It can be balanced by writing 2 before Zn as shown below:

C + 2ZnO -> CO₂ + 2Zn

Thus,  the equation is balanced!

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Answer:

mark me brilliant

Explanation:

According to the balanced chemical equation, for every 3 moles of H2 consumed, 2 moles of NH3 are produced.

Therefore, to find the number of moles of NH3 produced, we need to determine the ratio of H2 to NH3 based on the balanced equation:

3 moles H2 : 2 moles NH3

If 3 moles of H2 produces 2 moles of NH3, then 2.35 moles of H2 would produce:

(2 moles NH3 / 3 moles H2) x 2.35 moles H2 = 1.57 moles NH3

So, 1.57 moles of NH3 would be produced if 2.35 moles of H2 were consumed in this reaction.

The amount of moles are present in the oxygen gas is 0.04 mol.

To calculate the number of moles of oxygen present, we can use the ideal gas law equation:

PV = nRT

Given that:

P = pressure = 300 kPa = 303/101.3 = 2.9911 atm

V = volume = 0.64 L

R = gas constant = 0.08206 Latm/molK

T = temperature = 600 K

n = number of moles (what we are trying to find)

Rearranging the equation to solve for n, we get:

PV = nRT

n = PV / RT

Substituting the given values, we get:

n = ( 2.9911 atm × 0.64 L ) / ( 0.08206 Latm/molK ×  600 K )

n = 1.914304 / 49.236

n = 0.04 mol

Therefore, the amount present is 0.04 mol.

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The mass percentage of the sugar (C₁₂H₂₂O₁₁) in the mixture, given that the mixture has a mass of 12.76 g, is 85.42%

We'll begin by obtaining the molar mass of sugar (C₁₂H₂₂O₁₁) and NaCl. Details below:

For C₁₂H₂₂O₁₁

Molar mass of C₁₂H₂₂O₁₁ = (12 × 12) + (1 × 22) + (16 × 11)

Molar mass of C₁₂H₂₂O₁₁ = 342 g/mol

For NaCl

Molar mass of NaCl = 23 + 35.5

Molar mass of NaCl = 58.5 g/mol

Next, we shall obtain the mass of the sugar (C₁₂H₂₂O₁₁) in the mixture. Details below:

Mass of C₁₂H₂₂O₁₁ = [molar mass of C₁₂H₂₂O₁₁ / molar mass of (C₁₂H₂₂O₁₁ + NaCl)] × mass of mixture

Mass of C₁₂H₂₂O₁₁ = [342 / (342 + 58.5)] × 12.76

Mass of C₁₂H₂₂O₁₁ = 10.90 g

Finally, we shall determine the mass percentage of the sugar (C₁₂H₂₂O₁₁). This is illustrated as follow:

Mass percentage of sugar (C₁₂H₂₂O₁₁) = (mass of of KClO₃ / mass of mixture) × 100

Mass percentage of sugar (C₁₂H₂₂O₁₁) = (10.90 / 12.76) × 100

Mass percentage of sugar (C₁₂H₂₂O₁₁) = 85.42%

Thus, the mass percentage of the sugar (C₁₂H₂₂O₁₁) is 85.42%

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2 L

The solution is D. 1.4 L The formula is 2 C2H6(s), 702(g), 6 H2O(l), and 4 CO2(g). According to this equation, four molecules of carbon dioxide and seven molecules of oxygen are created for every two molecules of C2H6.

We can thus determine how many litres of carbon dioxide gas will be produced if we have 4.6 litres of oxygen gas. By dividing 4.6 litres of oxygen gas by 7, we get 0.657 litres of oxygen gas per molecule, which we may use for this purpose.

This is 2.628 litres of carbon dioxide gas when multiplied by four molecules of carbon dioxide. Finally, we arrive at 1.4 litres of carbon dioxide gas after rounding this to the nearest litre. The solution is D as a result.

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Answer:

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Explanation:

The lattice energy (ΔHlatt) can be calculated using the following equation:

ΔHlatt = ΔHf - ΔHsub - 1/2 ΔHbond - ΔHIE - ΔHEA

where ΔHf is the enthalpy of formation of the ionic compound, ΔHsub is the sublimation energy of the metal, ΔHbond is the bond energy of the diatomic gas, ΔHIE is the ionization energy of the metal, and ΔHEA is the electron affinity of the gas.

Substituting the given values:

ΔHlatt = (-639 kJ/mol) - (198 kJ/mol) - 1/2(142 kJ/mol) - (525 kJ/mol) - (-372 kJ/mol)

ΔHlatt = -639 kJ/mol - 198 kJ/mol - 71 kJ/mol - 525 kJ/mol + 372 kJ/mol

ΔHlatt = -1061 kJ/mol

Therefore, the lattice energy of the ionic compound MX is -1061 kJ/mol. Note that the negative sign indicates that the process of forming the solid ionic compound from the separate ions is exothermic (releases heat).

The acidic equilibrium equation for CCl₂HCOOH, which is also known as dichloroacetic acid, can be written as; CCl₂HCOOH ⇌ CCl₂HCOO⁻ + H⁺

In this equation, CCl₂HCOOH represents dichloroacetic acid in its uncharged, acidic form. When dichloroacetic acid dissolves in water or an aqueous solution, it can dissociate into its corresponding ions, CCl₂HCOO⁻ (dichloroacetate ion) and H⁺ (hydrogen ion).

The arrow (⇌) indicates that the reaction can proceed in both directions, with dichloroacetic acid donating a hydrogen ion to form the dichloroacetate ion, and the dichloroacetate ion accepting a hydrogen ion to reform dichloroacetic acid. This is an example of a weak acid dissociating in water to form its conjugate base and hydrogen ions, establishing an acidic equilibrium.

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