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3 years ago

The density of a certain type of steel is 8.1 g/cm3. What is the mass of a 124 cm3 chunk of this steel? Show

Chemistry

1 answer:

posledela3 years ago

8 0

Mass of the steel is $1004.4 g$

density of a substance can be regarded as the ratio of the mass of that substance to that of it's volume.

Mass of substance can be regarded as the quantitative measure of inertia, it can be simply explained as a fundamental property of all matter

We can express this mathematically as ;

$Density= \frac{ mass }{volume }$

Given :

Density of this steel= 8.1g/cm3

$Mass= 124 cm^{3}$

If we make Mass subject of formula,

$Mass= ( density *volume)$

Then let us substitute the values into the expression

$Mass= (124*8.1)$

$= 1004.4 g$

Therefore, mass of the steel is $1004.4 g$

Learn more at: brainly.com/question/9196460?referrer=searchResults

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Microwave radiation has a wavelength on the order of 1.0 cm. Calculate the frequency and the energy of a single photon of this r

denis23 [38]

Answer :

(1) The frequency of photon is, $3\times 10^{10}Hz$

(2) The energy of a single photon of this radiation is $1.988\times 10^{-23}J/photon$

(3) The energy of an Avogadro's number of photons of this radiation is, 11.97 J/mol

Explanation : Given,

Wavelength of photon = $1.0cm=0.01m$ (1 m = 100 cm)

(1) Now we have to calculate the frequency of photon.

Formula used :

$\nu=\frac{c}{\lambda}$

where,

$\nu$ = frequency of photon

$\lambda$ = wavelength of photon

c = speed of light = $3\times 10^8m/s$

Now put all the given values in the above formula, we get:

$\nu=\frac{3\times 10^8m/s}{0.01m}$

$\nu=3\times 10^{10}s^{-1}=3\times 10^{10}Hz$ $(1Hz=1s^{-1})$

The frequency of photon is, $3\times 10^{10}Hz$

(2) Now we have to calculate the energy of photon.

Formula used :

$E=h\times \nu$

where,

$\nu$ = frequency of photon

h = Planck's constant = $6.626\times 10^{-34}Js$

Now put all the given values in the above formula, we get:

$E=(6.626\times 10^{-34}Js)\times (3\times 10^{10}s^{-1})$

$E=1.988\times 10^{-23}J/photon$

The energy of a single photon of this radiation is $1.988\times 10^{-23}J/photon$

(3) Now we have to calculate the energy in J/mol.

$E=1.988\times 10^{-23}J/photon$

$E=(1.988\times 10^{-23}J/photon)\times (6.022\times 10^{23}photon/mol)$

$E=11.97J/mol$

The energy of an Avogadro's number of photons of this radiation is, 11.97 J/mol

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Answer:

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N2+3H2+6e- = 2NH3

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kondaur [170]

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Answer:

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