Which set contains only examples of analogous structures?

Answer:

ima guess producer

Explanation:

Taking into account the definition of molarity, the molar concentration of 5.8501 g NaCl dissolved in 500.00 cm³ volumetric flask is 0.2 mol/L.

Molarity is a measure of concentration that indicates the number of moles of solute that are dissolved in one liter of solution. This is, the molarity indicates the number of moles of solute that are dissolved in a given volume.

The molarity of a solution is calculated according to the following expression:

molarity= number of moles of solute÷ volume

Molarity is expressed in units moles/L.

In this case, you have:

Replacing in the definition of molarity:

molarity= 0.1 moles÷ 0.5 L

Solving:

molarity= 0.2 mol/L

Finally, the molar concentration is 0.2 mol/L.

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The partial pressure of \(N_2\)is 165.6 kPa and the partial pressure of \(H_2\)is 434.4 kPa.

To calculate the partial pressures of \(H_2\)and \(N_2\)in the 10dmcube container, we need to use the ideal gas law equation, which states that the pressure of a gas is directly proportional to its number of moles and temperature, and inversely proportional to its volume.

First, we need to calculate the number of moles for each gas. Since we are given the volume of each gas and the volume of the container, we can use the formula:

Number of moles = Volume / Molar volume

The molar volume is the volume occupied by one mole of a gas at a given temperature and pressure. At standard temperature and pressure (STP), the molar volume is 22.4 L/mol.

For \(N_2\), the number of moles is 2 dmcube / 22.4 L/mol = 0.089 mol
For \(H_2\), the number of moles is 5 dmcube / 22.4 L/mol = 0.223 mol

Next, we can calculate the partial pressures of each gas using the formula:

Partial pressure = (Number of moles / Total number of moles) * Total pressure

The total pressure is the sum of the pressures of each gas:

Total pressure = Pressure of N2 + Pressure of \(H_2\)

Given that the pressure of N2 is 100 kPa and the pressure of \(H_2\)is 500 kPa, we have:

Total pressure = 100 kPa + 500 kPa = 600 kPa

Now we can calculate the partial pressure of \(N_2\):

Partial pressure of \(N_2\)= (0.089 mol / (0.089 mol + 0.223 mol)) * 600 kPa = 165.6 kPa

Similarly, we can calculate the partial pressure of \(H_2\):

Partial pressure of H2 = (0.223 mol / (0.089 mol + 0.223 mol)) * 600 kPa = 434.4 kPa

Therefore, the partial pressure of \(N_2\)is 165.6 kPa and the partial pressure of \(H_2\)is 434.4 kPa.

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22.704 grams of CO2 are produced by burning 7.49 g of C4H10

This can be calculated as :

The basic reaction is: C4H10 + O2 = CO2 + H2O

We have 4 carbons for each reactant molecule, and this reacts with oxygen to form carbon dioxide and water.  We, therefore, need to show 4 CO2 molecules to consume these 4 carbons.

Next, let's balance the H atoms.  The 10 H atoms from the C4H10 must find a home in the water molecules.  5 water molecules can be made from 10 hydrogen atoms.

The only atom left is oxygen.  So far, the product side contains 13 O atoms (8 from the CO2 and 5 from the H2O).  Awkward, since oxygen only comes in pairs, an even number.  Let's use a fraction, 6.5, for the O2 for now, just to get it balanced:

This equation is balanced, but not legal since we can't have 1/2 of an O2 molecule.  So simply multiply all coefficients by 2:

The equation is now properly balanced.  It is telling us that we'll get 8 moles of CO2 for every 2 moles of C4H10.  That's a molar ratio of 4CO2/1 C4H8.

Let's find the moles of C4H8.  Divide the grams of C4H8 by its molar mass (58.04g/mole).

Now multiply moles C4H8 by the molar ratio we calculated above:

Convert to grams CO2 by multiplying by CO2's molar mass:

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The average atomic mass of naturally occurring strontium which consists of four isotopes, Sr-84, Sr-86, Sr-87, and Sr-88 is 87.1 amu.

To determine average atomic mass,

we take average of weight of all of the isotopes of that element.

Molecular weight of -

Sr-84 = 83.9 amu

Sr-86 = 85.9 amu

Sr-87 = 86.9 amu

Sr-88 = 87.9 amu

Average = 83.9 + 85.9 + 86.9 + 87.9 = 86.15

                                     4

We'll see the abundance of each isotope of strontium. Since the most abundant isotope of strontium is Sr-88 with 82.6% abundance. Therefore, the average atomic mass of strontium is closest to the mass of Sr-88, and the other isotopes are less than this mass.

Hence, the atomic mass of strontium is, 87.1 amu.

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Answer:

shape and texture.... .......

With regular / diffuse reflection, the angle and color of the object will determine the sharpness of reflection.

When two distinct media come together at an interface, a wave front might reverse direction so that it returns to the first medium, which is known as reflection. The reflection of light, sound, and water waves are typical examples.

Reflection offers the brain a chance to stop in the middle of the chaos, organize observations and experiences, take into account many interpretations, and come up with meaning. Learning from this meaning can then guide future behaviors and mindsets.

An image is a representation of an item created by light that has been reflected or refracted. A surface must be exceptionally smooth in order for reflection to provide an image that is both clear and crisp. An picture may not develop if the surface is even slightly uneven or lumpy.

Thus, with regular / diffuse reflection, the angle and color of the object will determine the sharpness of reflection.

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The energy of a photon of radiation with a frequency of 9.50 × 10¹³ Hz is 6.3 × 10⁻²⁰ J.

The Energy that comes from electromagnetic radiation is quantized, It exists in the form of small energy packets known as photons.

The energy of a photon is depends on the frequency at which it propagates from radiation source.

We can calculate the energy of a photon by the equation given below:

E = hν

where, E is the energy of photon

h is Plancks's constant whose value is 6.626 × 10⁻³⁴ Js

ν is the frequency of the radiation.

According to the question,

given,

frequency ν = 9.50 × 10¹³ Hz

therefore,

E = 6.626 × 10⁻³⁴ Js ×  9.50 × 10¹³ Hz      (∵1 Hz = 1s⁻¹)

E = 6.2947 × 10⁻²⁰ J

E≈ 6.3 × 10⁻²⁰ J

Thus, energy of the photon is 6.3 × 10⁻²⁰ J

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Answer:

One could be What kind of insulator do you use in the winter?

Explanation:

Explanation:

impurities affect both melting point and boiling point

in the case of melting point it lowers the melting point

so I guess one of the samples Ie contained impurities

Answer:

D. Liquid

Explanation:

It's mercury given the density and mercury's a metal that is liquid at room temperature

Answer:

A

Explanation:

it can occur between two hydrogen bonds

The climatic change in Earth's history that has resulted in glaciers is the cold climate.

During the last 2.6 million years, the Earth has experienced a series of ice ages, or periods of colder global climate, which have led to the growth of glaciers in regions with sufficient snowfall.

These colder periods are associated with changes in the Earth's orbit, tilt, and precession, which affect the amount and distribution of solar radiation received by the Earth. These climatic changes have had significant impacts on the Earth's surface and have influenced the evolution of life on our planet.

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to generate steam which act on copper

Answer:

Explanation:"Carbon can form single, double, or triple bonds with another carbon atom."

Carbon atoms has 6 electrons, therefore #1 is incorrect And carbon bonds usually increase the melting point of molecules. #2 is incorrect.

The frequency of the light released when an electron moves from the 2nd energy level to the 1st energy level in hydrogen is 2.47 x 10¹⁵ Hz.

The given parameters;

The energy of photon released when electron moves from the second energy level to the first energy level in hydrogen is calculated as following;

\(\Delta E = R_H\times h\times C (\frac{1}{n_1^2 } - \frac{1}{n_2^2} )\\\\\)

where;

Rh is the Rydberg constant

h is Plank's constant

C is the speed of light

\(\Delta E = (1.0974 \times 10^7 \times 6.626 \times 10^{-34} \times 3\times 10^8)(\frac{1}{2^2} - \frac{1}{1^2} )\\\\\Delta E= 2.18 \times 10^{-18}(-0.75)\\\\\Delta E= - 1.635 \times 10^{-18} \ J\)

The frequency of the light released is calculated as;

\(E = hf\)

where;

f is the frequency of the light;

\(f = \frac{E}{h} \\\\f = \frac{1.635\times 10^{-18}}{6.626 \times 10^{-34}} \\\\f = 2.47 \times 10^{15} \ Hz\)

Thus, the frequency of the light released is 2.47 x 10¹⁵ Hz.

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Answer:

235 °C

Explanation:

Since the pressure is being held constant, you can use Charles' Law to find the final temperature:

V₁ / T₁ = V₂ / T₂

In this equation, "V₁" and "T₁" represent the initial volume and temperature. "V₂" and "T₂" represent the final volume and temperature. You can plug the given values into the equation and simplify to find "T₂". The final answer should have 3 sig figs like the given values.

V₁ = 792 mL                             V₂ = 1.05 x 10³ mL

T₁ = 177 °C                                T₂ = ? °C

V₁ / T₁ = V₂ / T₂                                             <----- Charles' Law

792 mL / 177 °C = 1.05 x 10³ mL / T₂           <----- Insert values

4.4746 = 1.05 x 10³ mL / T₂                         <----- Simplify left side

(4.4746) x T₂ = 1.05 x 10³ mL                      <----- Multiply both sides by T₂

T₂ = 235                                                      <----- Divide both sides by 4.4746

Answer: 18.8 g

Explanation:

To find the mass of a 23.8 mL sample, all we have to do is set up a proportion.

\(\frac{0.791g}{mL} =\frac{x}{23.8mL}\)

\(18.8358=x\)

x=18.8 g

We round to 18.8 because of significant figures.

Taking into account the definition of density, the mass of a 23.8 mL sample of methanol is 18.83 g.

But first you must know that density is defined as the property that matter, whether solid, liquid or gas, has to compress into a given space.

Then, density is a quantity that allows us to measure the amount of mass in a certain volume of a substance. That is, it is the relationship between the weight (mass) of a substance and the volume it occupies.

Then, the expression for the calculation of density is the quotient between the mass of a body and the volume it occupies:

\(density= \frac{mass}{volume}\)

In this case:

Replacing in the definition of density:

\(0.791 \frac{g}{mL} = \frac{mass}{23.8 mL}\)

Solving:

mass= 0.791 \(\frac{g}{mL}\)× 23.8 mL

mass= 18.83 g

In conclusion, the mass of a 23.8 mL sample of methanol is 18.83 g.

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If you're attempting to synthesize 2 benzyl pentanoic acid from acetoacetic ester, keep in mind that you can do so fairly quickly by following these simplified instructions:

From its pungent free scent to its solid state at temperatures ranging from 118 120°C, acetoacetic ester (better known as ethyl acetoacetate) offers significant value for those working within organic synthesis.

As one of many potent ketones utilized by researchers around the globe its unique properties make it ideal for building complex molecules essential for modern medicine and more.

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Answer:

it's a day I think so ........

Answer:

Lunar cycle

Explanation:

Year is the amount of time for the Earth to rotate a complete circle around the sun.

Lunar cycle (moon phases) is the rotation of the Moon around the Earth.

Day is the time for the Earth to rotate on its own axis completely.

Solar cycle is the changes that the sun's electric field goes through about every 11 years.

The value of Kc for the reaction at 25°C is 11.25.

The equilibrium constant expression for the reaction:

2NO(g) + \(Cl_2\)(g) ⇌ 2NOCl(g)

is Kc = \(([NOCl]^2)/([NO]^2[Cl_2])\), where [NO], [\(Cl_2\)], and [NOCl] are the molar concentrations of NO, \(Cl_2\), and NOCl, respectively, at equilibrium.

At 25°C, if the concentration of NO and \(Cl_2\) are 0.2 M and the concentration of NOCl is 0.3 M, then we can substitute these values into the equilibrium constant expression to find the value of Kc:

Kc =\(([NOCl]^2)/([NO]^2[Cl_2])\)

Kc = \((0.3^2)/(0.2^2*0.2)\)

Kc = 11.25

Therefore, the value of Kc for the reaction at 25°C is 11.25.

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--The complete Question is, Assuming trials with equilibrium constants, what is the equilibrium constant expression for the reaction:

2NO(g) + Cl2(g) ⇌ 2NOCl(g)

and what is the value of Kc at 25°C if the concentration of NO and Cl2 are 0.2 M and the concentration of NOCl is 0.3 M? --

The concentration of the KOH=  0.15M.

What is concentration?

The concentration of a substance, such as salt, in a particular volume of tissue or liquid, such as blood. The substance concentrates when there is less water present.

What is stock solution?

A solution that has been diluted to a lower concentration and will be used. The default strategy could be used independently or as a component of a more complex solution. A working solution is the option we ultimately settle on.

M stock V stock = M dilute V dilute

25ml* 6M = M* 1L * 1000ML/1L

25Ml*6M/1000Ml = M

M dilute = 0.15M

Concentration of KOH = 0.15M

Therefore, the concentration of the KOH=  0.15M.

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6.02 x \(10^{20\) formula units of MgCl₂ is equal to 0.1 moles of MgCl₂.

To convert formula units of MgCl₂ to moles of MgCl₂, we need to use Avogadro's number, which relates the number of formula units to the number of moles.

Avogadro's number (NA) is approximately 6.022 x 10^23 formula units per mole.

Given that we have 6.02 x 10^20 formula units of MgCl₂, we can set up a conversion factor to convert to moles:

(6.02 x 10^20 formula units MgCl₂) * (1 mol MgCl₂ / (6.022 x 10^23 formula units MgCl₂))

The formula units of MgCl₂ cancel out, and we are left with moles of MgCl₂:

(6.02 x 10^20) * (1 mol / 6.022 x 10^23) = 0.1 mol

Therefore, 6.02 x 10^20 formula units of MgCl₂ is equal to 0.1 moles of MgCl₂.

It's important to note that this conversion assumes that each formula unit of MgCl₂ represents one mole of MgCl₂. This is based on the stoichiometry of the compound, where there is one mole of MgCl₂ for every one formula unit.

Additionally, this conversion is valid for any substance, not just MgCl₂, as long as you know the value of Avogadro's number and the number of formula units or particles you have.

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The molecular formula is (CH2O)5 when the scale factor is 5 and the empirical formula is CH2O.

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

Empirical formula is CH₂O

Molar mass of compound = 150 g/mol

Scaling factor (n) =?

Empirical formula × n = molar mass

[CH₂O]n = 150

[12 + (2×1) + 16]n = 150

[12 + 2 + 16]n = 150

30n = 150

Divide both sides by 30

n = 5

Therefore, the scaling factor is 5

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Answer:

The scale factor is 5. The formula is CH2O.

Multiply each by 5.

So:

C (there is only one)= 1×5

H (there are 2)= 2×5

O(there is only one)= 1×5

Equalling= C5H10O5

The density of the solid block is 3.79 * 10⁻³ g/cm³.

The density of a substance is defined as the ratio of mass and volume of a substance.

Density measure how close together the particles of a given mass of a substance is. Substances with high density have greater masses compared to the volume of those substances whereas substances with low densities have greater volume compared to their masses.

The volume of the solid block = 78 * 55 * 35 = 150150 cm³

mass of solid block = 569 g

Density of the solid block = 569 g/150150 cm³

Density of the solid block = 3.79 * 10⁻³ g/cm³

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Answer:

∆H = - 450 kJ/mol

Explanation:

You can calculate the change in enthalpy provided we have the heat of solution (q). That would be the only approach to this problem. But this approach is only possible if we have a specific set-up; we would have to use a calorimeter. So then the reactants are taken as the system, and water as the surroundings. When calculating q, the heat of the solution, we take 4.18. Remember that heat is flowing from the reaction mixture, to the water, from the system to surroundings, so it's exothermic and ∆H = negative:

The mass of the gas that is produced is  112 g.

What is the mass of the nitrogen that is need?

We know that the density of the gas is the ratio of the mass to the volume of the gas. In the case of the question that we have here, we can see that there are about 70 L of the nitrogen gas and then we have also about 1.16 g/L  given as the density of the gas.

Density = Mass/ volume

Mass = Density * volume

Mass of the gas = 70 L * 1.16 g/L

Mass of the gas = 112 g

Thus the inflating gas is  112 g nitrogen.

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1. The standard cell potential for this reaction is 0.14 V.

2. The standard cell potential for this reaction is 0.46 V.

3. The reduction potential for Hg2+(aq) + 2e^- → Hg(l) is 0.79 V.

1. The half-reactions are:

Oxidation: Sn2+(aq) → Sn(s) + 2e^-

Reduction: Pt2+(aq) + 2e^- → Pt(s)

To balance the charges, we multiply the oxidation half-reaction by 2:

2Sn2+(aq) → 2Sn(s) + 4e^-

Now, we can combine the half-reactions to form the overall cell reaction:

2Sn2+(aq) + Pt2+(aq) → 2Sn(s) + Pt(s)

The cell notation for this reaction is:

Sn(s) | Sn2+(aq) || Pt2+(aq) | Pt(s)

To calculate the standard cell potential (E°), we can look up the reduction potentials for each half-reaction. The reduction potential for Pt2+(aq) + 2e^- → Pt(s) is typically listed as 0.00 V. The reduction potential for Sn2+(aq) + 2e^- → Sn(s) is -0.14 V. The standard cell potential is the sum of the reduction potentials:

E° = E°(reduction) - E°(oxidation)

E° = 0.00 V - (-0.14 V) = 0.14 V

2. The half-reactions are:

Oxidation: Co2+(aq) → Co(s) + 2e^-

Reduction: Cr3+(aq) + 3e^- → Cr(s)

To balance the charges, we multiply the reduction half-reaction by 2:

2Cr3+(aq) + 6e^- → 2Cr(s)

Now, we can combine the half-reactions to form the overall cell reaction:

Co2+(aq) + 2Cr3+(aq) + 6e^- → Co(s) + 2Cr(s)

The cell notation for this reaction is:

Co(s) | Co2+(aq) || Cr3+(aq) | Cr(s)

To calculate the standard cell potential (E°), we look up the reduction potentials for each half-reaction. The reduction potential for Co2+(aq) + 2e^- → Co(s) is typically listed as -0.28 V. The reduction potential for Cr3+(aq) + 3e^- → Cr(s) is -0.74 V. The standard cell potential is the sum of the reduction potentials:

E° = E°(reduction) - E°(oxidation)

E° = -0.28 V - (-0.74 V) = 0.46 V

3. The half-reactions are:

Oxidation: Cr2+(aq) → Cr(s) + 2e^-

Reduction: Hg2+(aq) + 2e^- → Hg(l)

The balanced overall cell reaction is:

Cr2+(aq) + 2Hg2+(aq) + 4e^- → Cr(s) + 2Hg(l)

The cell notation for this reaction is:

Hg(l) | Hg2+(aq) || Cr2+(aq) | Cr(s)

To calculate the standard cell potential (E°), we look up the reduction potentials for each half-reaction. The reduction potential for Cr2+(aq) + 2e^- → Cr(s) is typically listed as -0.91 V.

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