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2 years ago

What does the wavelength of a wave measure?

Chemistry

2 answers:

julia-pushkina [17]2 years ago

8 0

Answer:

Explanation:

The wavelength of a wave measure is the width of the wave. It is the amount of distance that is in between two successive crests or troughs of a single wave.

Iteru [2.4K]2 years ago

6 0

Wave length measures the width of the wave

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Consider water at 500 kPa and a specific volume of 0.2 m3/kg, what is the temperature (in oC)?

Artyom0805 [142]

Answer:

$T=-272.9^{o}C$

Explanation:

We have the ideal gasses equation $PV=nRT$ and the expression for the specific volume $v=\frac{V}{m}$ , that is the inverse of the density, and for definition the number of moles is equal to the mass over the molar mass, that is $n=\frac{m}{M}$

And we can relate the three equations as follows:

$PV=nRT$

Replacing the expression for n, we have:

$PV=\frac{m}{M}RT$

$P\frac{V}{m}=\frac{RT}{M}$

Replacing the expression for v, we have:

$Pv=\frac{RT}{M}$

Now resolving for T, we have:

$T=\frac{PvM}{R}$

Now, we should convert all the quantities to the same units:

-Convert 500kPa to atm

$500kPa*\frac{0.00986923}{1kPa}=4.93atm$

-Convert 0.2 $\frac{m^{3}}{kg}$ to $\frac{L}{kg}$

$0.2\frac{m^{3} }{kg}*\frac{1L}{1m^{3}}=0.2\frac{L}{kg}$

- Convert the molar mass M of the water from $\frac{g}{mol}$ to $\frac{kg}{mol}$

$18\frac{g}{mol}=\frac{1kg}{1000g}=0.018\frac{kg}{mol}$

Finally we can replace the values:

$T=\frac{(4.93atm)(0.2\frac{L}{kg})(0.018\frac{kg}{mol})}{0.082\frac{atm.L}{mol.K}}$

$T=0.216K$

$T=0.216K-273.15\\T=-272.9^{o}C$

5 0

3 years ago

Briefly describe bohr's model postulates and its limitations.

ch4aika [34]

Answer:

Bohr's Model postulates-

I postulate - The electrons in an atom orbit around the nucleus in definite circular paths called orbits or shells.

II Postulate - Each shell or orbit represents a specific amount of energy.

III Postulate - By emitting or absorbing energy, an electron may shift from one stationary energy orbit to another.

Three main Limitations -

1- It adjusts to the hydrogen atom's spectrum but not to the spectra of other atoms.

2 - In the definition of the electron as a tiny particle that spins around the atomic nucleus, the wave properties of the electron are not described.

3- Bohr is unable to understand why classical electromagnetism is inapplicable to his model. That is why, when electrons are in a stationary orbit, they do not emit electromagnetic radiation.

Explanation:

About Bohr's postulates-

1 - The electron spins in circling circles around the nucleus, emitting no energy. The orbital angular momentum is constant in these orbits.

Only certain radii of orbits, corresponding to certain given energy levels, are required for electrons in an atom.

2- Not every orbit is possible. However, whenever an electron is in a legal orbit, it is in a state of unique and constant energy and does not emit energy (stationary energy orbit).

For example - The energies allowed for electrons in the hydrogen atom are given by the following equation: The Rydberg constant for the hydrogen atom is $-2.8\times10^-^1^8$ in this equation, and n = quantum number will range from 1 to ∞. For each of the values of n, the electron energies of a hydrogen atom produced by the above equation are negative. As n rises, the energy becomes less negative and thus rises.

3- By emitting or absorbing energy, an electron may shift from one stationary energy orbit to another.

The energy difference between the two states would be equal to the energy released or consumed. This energy E is in the form of a photon, and it can be measured using the following formula:

$E=h$ $v$

E is the energy (absorbed or emitted) in this equation, and h is the Planck constant (its value is $6.63\times10^-^3^4 Js$ ) and v denotes the frequency of light, which is calculated in 1/ s.