The isotope calcium-41 decays into potassium-41, with half-life of 1.03 x 105 years. There is a sample of calcium-41 containing 5 x 10° atoms. How
many atoms of calcium-41 and potassium-41 will there be after 4.12 › 105 years?
A.
3.125 x 108 atoms of calcium-41 and 4.375 x 10° atoms of potassium-41
6.25 x 108 atoms of calcium-41 and 4.6875 x 10° atoms of potassium-41
•
6.25 x 108 atoms of calcium-41 and 4.375 10° atoms of potassium-41
O D. 3.125 x 108 atoms of calcium-41 and 4.6875 › 10° atoms of potassium-41

Answer:

C

Explanation:

This is a chemical reaction because the materials that were mixed have different solubilities than the materials that were made.

Answer:

C

Explanation:

When a chemical reaction occurs, new materials form. Different materials each have unique physical properties, such as solubility.

When olive oil and sodium hydroxide were mixed together, soap and glycerol were made. The table shows that olive oil and sodium hydroxide have solubilities that are different than soap and glycerol. This means that olive oil and sodium hydroxide are different materials than soap and glycerol. Therefore, this is a chemical reaction because the materials that were mixed have different solubilities than the materials that were made.

The rate of the given reaction is 0.00197 M/s.

The balanced chemical equation of the reaction is:

CO (g) + NO₂ (g) → CO₂ (g) + NO (g)

From the equation, 1 mole of CO produces 1 mole of CO₂, and hence the number of moles of CO2 produced is equal to the number of moles of CO consumed.

The concentration of CO₂ produced = 0.123 M.

Therefore, the concentration of CO consumed is also 0.123 M.

The rate of reaction is given by the formula:

where Δ[C] is the change in concentration and Δt is the change in time.

Over 62.3 seconds, the concentration of CO decreases from 0 M to 0.123 M.

Δ[C] = 0.123 M - 0 M

Δ[C]  = 0.123 M

Δt = 62.3 s

Substituting the values in the formula, we get:

rate of the reaction = Δ[C]/Δt

rate of the reaction = 0.123 M/62.3 s

rate of the reaction = 0.00197 M/s

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Explanation:

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The acidic level is given by the amount of hydronium in a specific solution.

Therefore, the tert-amyl chloride would turn acidic because the quantity of hydronium will increase, which decreases the pH level.

Answer:

0.9moles of Zn are produced

Explanation:

Based on the reaction:

ZnO + 2Na → Na2O + Zn

1 mole of ZnO reacts with 2 moles of Na to produce 1 mole of Na2O and 1 mole of Zn

For 2 moles of sodium present, 1 mole of Zn is produced (The conversion factor is 2mol Na = 1mol Zn

If 1.8 moles of sodium are present:

1.8mol Na * (1mol Zn / 2mol Na) =

Answer:

C

Explanation:

The deeper you go into water, the greater pressure there is on everything. This compresses the air inside and causes the volume to shrink.

Sometimes air is measured in bars. Let's assume the Earth's surface pressure is 1. Let's also say that your lungs have 5.5L and the tank has 11L. That's only 2 breathes, but under 200 bars of pressure deep in the ocean? That's 200 x 11, which equals 2200L. That's about 400 breathes.

In addition, if making liters out of thin air doesn't make any sense, there's an alternative where you divide your liters per breath by the bar pressure. So instead of 200 x 11, you can take your 5.5 from your lungs and divide it by 200. That small number, in this case, 0.0275, can serve as how much air you breath deep in the ocean.

The Px, Py, and Pz orbitals are called degenerate orbitals because they have the same energy. In other words, they are three orbitals that are equivalent in terms of their energy levels.

Degeneracy in this context means that these orbitals have the same energy and are indistinguishable from each other in terms of their properties. The Px, Py, and Pz orbitals belong to the p sublevel, which is characterized by three orbitals aligned along the x, y, and z axes, respectively. These orbitals are oriented perpendicular to each other.

The degeneracy of the Px, Py, and Pz orbitals arises from the symmetry of the system. Since these orbitals have the same energy, they are all equally likely to be occupied by electrons. This degeneracy allows for electron movement and distribution within the p sublevel without any preference for a specific orbital.

The degenerate nature of these orbitals has important implications in molecular bonding and chemical reactions. For example, during hybridization, the degenerate p orbitals can combine to form hybrid orbitals with different shapes and orientations, such as sp, sp2, or sp3 hybrid orbitals.

These hybrid orbitals then participate in bonding with other atoms, enabling the formation of various molecular geometries and structures.

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The IUPAC name for the compound given in the question is 2,3-dibromo-5-methylheptane

The IUPAC name for compound can be obtained by using the following steps:

Thus, the IUPAC name for the compound is: 2,3-dibromo-5-methylheptane

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Answer:

when placed in water, a sodium pellet catches on fire as hydrogen gas is liberated and sodium hydroxide forms. chemical change = fire is a sign of chemical reaction.

Explanation:

When placed in water the sodium pellets catch the fire and liberate the hydrogen gas. On mixing with water solid sodium forms a colorless basic solution.

Sodium is a soft metal. It is a very reactive element with a low melting point. Sodium reacts very quickly with water, snow, and ice to produce sodium hydroxide and hydrogen. It is an alkali metal and the sixth most abundant metal on earth. It has a silvery white color.

It has a strong metallic luster. On reacting with oxygen it produces sodium oxide which on reacting with the water produces sodium hydroxide.

It is used to improve the structure of certain alloys and soaps. It is also used in the purification of metals. Sodium is also present in sodium chloride, an important compound found in the environment.

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Based on the percentage mass of oxygen in trifluoroacetic acid, the mass of the trifluoroacetic acid sample is 168.5 grams.

The percentage mass of oxygen in trifluoroacetic acid is determined as follows:

The molar mass of trifluoroacetic acid = 12 * 2 + 1 + 19 * 3 + 16 * 2

The molar mass of trifluoroacetic acid = 114 g

The percentage mass of oxygen in trifluoroacetic acid = (16 * 2)/114 * 100%

The percentage mass of oxygen in trifluoroacetic acid = 28.07%

The mass of the trifluoroacetic acid sample will be 47.3/ 28.07% = 168.5 grams

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When a sample (oxygen) is enclosed within a container and is heated, the partial pressure of the oxygen would also increase.

Partial pressure is defined as the total amount of pressure that is being exerted by a single gas within a container.

From the given question, the partial pressure of a given gas such as the oxygen is being affected by an increase in temperature of the gas.

According to gas law, an increase in the temperature of a gas within an enclosed medium would lead to an increase in the pressure of the has as there in increased intermolecular collisions.

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Answer:

Mass percentage of NH₄Cl = 3.54%

Mass percentage of K₂CO₃ = 1.01%

Explanation:

If a 200.0 mL aliquot produced  0.105 g of KB(C₆H₅)₄, then a 100.0 mL aliquot would produce 1/2 * 0.105 g = 0.0525 g of KB(C₆H₅)₄.

Therefore, mass of NH₄B(C₆H₅)₄ in the 100.0 ml aliquot = (0.277 - 0.0525)g = 0.2245 g

Number of moles of NH₄B(C₆H₅)₄ in 0.2245 g = 0.2245 g/ 337.27 g/mol = 0.0006656 moles

In 500 ml solution, number of moles present = 0.0006656 * 500/100 = 0.003328 moles.

From equation of the reaction; mole ratio of  NH₄⁺ and NH₄B(C₆H₅)₄ = 1:1

Similarly, mole ratio of  NH₄⁺ and NH₄Cl = 1:1

Therefore, moles of NH₄Cl in 500 ml sample = 0.003328 moles

Mass of NH₄Cl  = 0.003328 mol * 53.492 g/mol = 0.178 g

Mass percentage of NH₄Cl = (0.178/5.025) * 100% = 3.54%

Number of moles of KB(C₆H₅)₄ in 0.105 g (precipitated from 200.0 ml aliquot) = 0.105 g/ 358.33 g/mol = 0.000293 moles

In 500 ml solution, number of moles present = 0.000293 * 500/200 = 0.0007326 moles.

From equation of the reaction; mole ratio of  K⁺ and KB(C₆H₅)₄ = 1:1

Similarly, mole ratio of  K⁺ and K₂CO₃ = 2:1

Therefore, moles of K₂CO₃ in 500 ml sample = 0.0007326/2 moles =  0.0003663 moles

Mass of  K₂CO₃ = 0.0003663 mol * 138.21 g/mol = 0.05063 g

Mass percentage of K₂CO₃ = (0.05063/5.025) * 100% = 1.01%

The thickness of the aluminum is approximately 0.00172 cm or 0.0172 mm

To calculate the thickness of the aluminum, we need to use the formula:

Density = Mass / (Length x Width x Thickness)

Given:

Mass of aluminum = 0.475 g

Length of aluminum = 10.08 cm

Width of aluminum = 10.08 cm

We need to rearrange the formula to solve for thickness:

Thickness = Mass / (Length x Width x Density)

The density of aluminum is approximately 2.7 g/cm³.

Now we can substitute the given values into the formula:

Thickness = 0.475 g / (10.08 cm x 10.08 cm x 2.7 g/cm³)

Thickness ≈ 0.475 g / (102.4064 cm² x 2.7 g/cm³)

Thickness ≈ 0.475 g / 275.879104 cm³

Thickness ≈ 0.00172 cm or 0.0172 mm

Therefore, the thickness of the aluminum is approximately 0.00172 cm or 0.0172 mm.

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To balance the equation we start by counting the number of atoms we have of each element on each side of the reaction.

Reagents side:

C=1 atom

H= 4 atoms

O= 2 atoms

Products side:

C=1 atom

O= 3 atoms

H= 2 atoms

The carbon is balanced, let's start by balancing the hydrogen. We have 4 hydrogens on the reactant side and 2 on the product side.

To have the same number we must place the coefficient 2 in the H2O molecule as follows.

Now we must balance the oxygen. On the reactants side, we have 2 and on the products side, we have 4. Then we put the coefficient two in the O2 molecule and we have our balanced equation.

Reagents side:

C=1 atom

H= 4 atoms

O= 4 atoms

Products side:

C=1 atom

O= 4 atoms

H= 4 atoms

We have the same number of atoms of each element on both sides of the reaction. So the equation is balanced.

Now, we see in the reaction a fuel, methane (CH4) reacting with oxygen. This type of reaction is combustion and generates a large amount of energy producing CO2 and water

The empirical formula of the compound is C₂H₁₆S₂N₃O.

The moles of each element is as follows::

For CO₂:

Carbon (C) has a molar mass of 12.01 g/mol.

Oxygen (O) has a molar mass of 16.00 g/mol.

Moles of C in CO₂ = 2.08 g / 12.01 g/mol = 0.173 moles

Moles of O in CO₂ = 2.08 g / 16.00 g/mol = 0.130 moles

For H₂O:

Hydrogen (H) has a molar mass of 1.01 g/mol.

Oxygen (O) has a molar mass of 16.00 g/mol.

Moles of H in H₂O = 1.28 g / 1.01 g/mol = 1.27 moles

Moles of O in H₂O = 1.28 g / 16.00 g/mol = 0.080 moles

For SO₃:

Sulfur (S) has a molar mass of 32.06 g/mol.

Oxygen (O) has a molar mass of 16.00 g/mol.

Moles of S in SO₃ = 4.77 g / 32.06 g/mol = 0.149 moles

Moles of O in SO₃ = 4.77 g / 16.00 g/mol = 0.298 moles

For HNO₃:

Hydrogen (H) has a molar mass of 1.01 g/mol.

Nitrogen (N) has a molar mass of 14.01 g/mol.

Oxygen (O) has a molar mass of 16.00 g/mol.

Moles of H in HNO₃ = 3.48 g / 1.01 g/mol = 3.45 moles

Moles of N in HNO₃ = 3.48 g / 14.01 g/mol = 0.248 moles

Moles of O in HNO₃ = 3.48 g / 16.00 g/mol = 0.217 moles

The simplest whole-number ratio of the elements will be:

Carbon: 0.173 moles / 0.080 moles ≈ 2.16

Hydrogen: 1.27 moles / 0.080 moles ≈ 15.88

Sulfur: 0.149 moles / 0.080 moles ≈ 1.86

Nitrogen: 0.248 moles / 0.080 moles ≈ 3.10

Oxygen: 0.080 moles / 0.080 moles = 1

Therefore, the empirical formula is C₂H₁₆S₂N₃O.

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The internal pressure of the container will increase, given that the temperature of the confined gas increases from 10 °C to 30 °C (Option B)

To determine if the pressure will decrease, increase or remain the same, we shall obtain the new pressure of the container. Details below

The following data were obtained from the question:

P₁V₁ / T₁ = P₂V₂ / T₂

Volume = contant

P₁ / T₁ = P₂ / T₂

P / 283 = P₂ / 303

Cross multiply

P₂ × 283 = P × 303

Divide both sides by 283

P₂ = (P × 303) / 283

P₂ = 1.07 × P

From the above calculation, we can see that the new pressure is 1.07 times the initial pressure.

Thus, we can conclude that the internal pressure will increase (Option B)

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Complete question:

A 100.-milliliter sample of helium gas is placed in a sealed container of fixed volume. As the temp of the confined gas increases from 10°c to 30°c, the internal pressure

A. Decreases

B. Increases

C. Remain the same

Answer:

Part A: Protonation, Protonation

Part B: An elimination, A substitution

Explanation:

The dehydration ethanol and the condensation of ethanol all begin from the protonation of ethanol. This is because, water is a good leaving group. Thus, the protonation of the -OH moiety of the molecule is the first step in each mechanism.

The dehydration of ethanol is an elimination reaction because it involves the loss of H-O-H from the ethanol molecule while the condensation of ethanol is an substitution reaction because the -OH moiety is replaced by -OCH2CH3.

Answer:

Copper will start to react with the oxygen in the air to form copper oxide. The copper oxide will continue reacting to oxygen over time. As the copper oxide continues to react with carbon dioxide and water in the air it coats the surface with that iconic blue-green patina colour

Answer: Less

Explanation:

Ethane is a non-polar molecule while water is a polar molecule

The two chemical compounds are not the same, because their ratio is not equal. In both samples the composition of lead and oxygen is different.

A chemical compound is a substance made of numerous similar molecules (or molecular entities) joined by chemical bonds and comprising atoms from various chemical elements. Therefore, a molecule made up of only one type of atom is not a compound. Chemical reactions, which may entail interactions with other molecules, can change a compound into a distinct substance. Atomic bonds may be broken or new ones created during this process.

sample 1 = mass of lead / mass of oxygen = 12.92g/2g = 6.46 .

sample 2 = mass of lead/ mass of oxygen = 34.27 - 14.39/14.39 = 1.38 .

so, the ratios are not the same.

Hence, the two chemical compounds are not the same, because their ratio is not equal. In both samples the composition of lead and oxygen is different.

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an ionic compound is made of two or more elements held by a strong electrostatic force. metal atoms lose electrons to become positive ions, and non metals gain electrons to become negative ions. ionic bonding occurs between metals and non metals

Answer: Quantitative data

Explanation:

Double bond in ethene is made up of sigma and Pi bonds.

The covalent bond will be formed by the lateral overlap of the atomic orbitals is known as pi bond. For example, ethylene molecule contain 5 sigma bonding as well as 1 pi bonding in it. Pi bond formation will takes place by the parallel orientation of the two p orbitals in an adjacent atoms by proper sideways overlap. Thus in any molecule in which pi bond formation will takes place at all the atoms must be having in the same plane. Thus in pi bond carbon carbon double bond rotation is restricted due to the maximum overlap of the p orbitals. Example : Ethene molecule

Sigma bond (σ bond): A covalent bond will be formed by the overlap of atomic orbitals and/or hybrid orbitals along with the bond axis (i.e., along a line connected to the two bonded atoms). The sigma bond in the hydrogen molecule is formed by overlap of a pair of 1s orbitals, one from each hydrogen atom.

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B. 45.0 L.The balloon has a 45.0 L volume shortly before it bursts.

When temperature is held constant, a gas's volume and pressure have an inverse relationship. This implies that the volume increases as the pressure falls.

Using the Ideal Gas Law, we can calculate the change in volume with the following equation:

\(\frac{V2}{T2} = \frac{V1}{T1}\)

where T1 denotes the starting temperature, T2 denotes the finished temperature, V1 denotes the starting volume, and V2 is the finished volume.

Given:

V1 = 7.2 L

T1 = 27℃ = 300 K

T2 = -32℃ = 241 K

We can solve for V2:

\(V2 = \frac{(V1 * T2) }{ T1} \\\)

\(V2 =\frac{ (7.2 L * 241 K) }{ 300 K }\\V2 = 45.0 L\)

Therefore, the volume of the balloon just before it bursts is 45.0 L.

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the pH of the aqueous solution is 8.51 with a hydrogen ion concentration of [H+]=3.1×\(10^-9\)M

The pH of the aqueous solution can be calculated using the formula:

pH = -log[H+]

where [H+] is the hydrogen ion concentration of the solution.

Substituting the given value, we get:

pH = -log(3.1×\(10^-9\))

pH = 8.51

An aqueous solution is one in which water serves as the solvent. It is utilised in a variety of applications, including analytical chemistry, biochemistry, and industrial chemistry. It is the most prevalent kind of solution used in chemical reactions. Water serves as both the solvent and the solute in an aqueous solution, where the solute is often a solid, liquid, or gas. Due to its high polarity and capacity to make hydrogen bonds with other molecules, water is an excellent solvent that can dissolve a variety of materials, including polar molecules and ionic compounds. Acid-base reactions, redox reactions, and precipitation reactions are just a few of the numerous chemical processes that take place in aqueous solutions. A variety of variables can have an impact on an aqueous solution's characteristics.

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Answer:

0.028 mole of ammonium phosphate, (NH₄)₃PO₄.

Explanation:

We'll begin by writing the balanced equation for the reaction. This is illustrated below:

H₃PO₄ + 3NH₃ —> (NH₄)₃PO₄

From the balanced equation above,

3 moles of NH₃ reacted to produce 1 mole of (NH₄)₃PO₄.

Finally, we shall determine the number of mole of (NH₄)₃PO₄ produced by the reaction of 0.085 mole of ammonia, NH₃. This can be obtained as follow:

From the balanced equation above,

3 moles of NH₃ reacted to produce 1 mole of (NH₄)₃PO₄.

Therefore, 0.085 mole of NH₃ will react to produce = (0.085 × 1)/3 = 0.028 mole of (NH₄)₃PO₄.

Thus, 0.028 mole of ammonium phosphate, (NH₄)₃PO₄ were obtained from the reaction.

We need collisonal section area

\(\\ \sf\longmapsto \sigma=2d\)

\(\\ \sf\longmapsto \sigma=2(0.20nm)\)

\(\\ \sf\longmapsto \sigma=0.4nm\)

Answer:

\(224 \times 13313\frac{.131?}{?244} \)