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Nikolay [14]
3 years ago
14

Calculate the wavelength of the light emitted when an electron in a one-dimensional box of length 5.4 nmnm makes a transition fr

om the n=9n=9 state to the n=8n=8 state.
Chemistry
1 answer:
bazaltina [42]3 years ago
3 0

Answer : The wavelength of the light emitted is, 5.66\times 10^{-24}m

Explanation :

The energy level of quantum particle in a one-dimensional box is given as:

E_n=\frac{n^2h^2}{8mL^2}

or,

\Delta E=E_9-E_8=\frac{n_9^2h^2}{8mL^2}-\frac{n_8^2h^2}{8mL^2}

\Delta E=E_9-E_8=\frac{h^2}{8mL^2}\times (n_9^2-n_8^2)

where,

E_n = change in energy

n = energy level

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

m = mass of electron = 9.109\times 10^{-31}kg

L = length of a one-dimensional box = 5.4nm=5.4\times 10^{-9}m

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

\Delta E=E_9-E_8=\frac{(6.626\times 10^{-34}Js)^2}{8\times (9.109\times 10^{-31}kg)\times (5.4\times 10^{-9}m)^2}\times [(9)^2-(8)^2]

\Delta E=E_9-E_8=3.5124\times 10^{-2}J

Now we have to calculate the wavelength of the light emitted.

\Delta E=\frac{hc}{\lambda}

where,

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

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

\lambda = wavelength of the light

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

3.5124\times 10^{-2}J=\frac{(6.626\times 10^{-34}Js)\times (3\times 10^{8}m/s)}{\lambda}

\lambda=5.66\times 10^{-24}m

Thus, the wavelength of the light emitted is, 5.66\times 10^{-24}m

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wlad13 [49]
<h3>Answer:</h3>

18.58 liters of hydrogen gas

<h3>Explanation:</h3>

We are given;

  • The equation;

3Mg + 2H₃(PO₄) → Mg₃(PO₄)₂ + 3H₂

  • Atoms of Magnesium = 7.179 x 10^23 atoms
  • Mass of phosphoric acid as 54.21 g

We are required to determine the volume of hydrogen gas produced;

Step 1; moles of Magnesium

1 mole of an element contains 6.02 × 10^23 atoms

therefore;

Moles of Mg = (7.179 x 10^23 ) ÷ (6.02 × 10^23)

                   = 1.193 moles

Step 2: Moles of phosphoric acid

moles = Mass ÷ Molar mass

Molar mass of phosphoric acid = 97.994 g/mol

Therefore;

Moles of Phosphoric acid = 54.21 g ÷ 97.994 g/mol

                                           = 0.553 moles

Step 3: Determine the rate limiting reagent

From the mole ratio of Mg to Phosphoric acid (3 : 2);

1.193 moles of magnesium requires 0.795 moles of phosphoric acid while,

0.0553 moles of phosphoric acid requires 0.8295 moles of Mg

Therefore, phosphoric acid is the rate limiting reagent

step 4: Determine the moles of hydrogen produced

From the equation, w moles of phosphoric acid reacts to produce 3 moles of hydrogen;

Therefore; moles of Hydrogen = moles of phosphoric acid × 3/2

                                                   = 0.553 moles × 3/2

                                                   = 0.8295 moles

Step 5: Volume of hydrogen gas

1 mole of a gas occupies a volume of 22.4 liters at STP

Therefore;

Volume of Hydrogen = 0.8295 moles × 22.4 L/mol

                                  = 18.58 Liters

Therefore; 18.58 liters of hydrogen gas  will be produced

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makvit [3.9K]

<u>Answer:</u> The standard electrode potential of the cell is 4.53 V.

<u>Explanation:</u>

We are given:

E^o_{(F_2/F^-)}=2.87V\\E^o_{(Al^{3+}/Al)}=-1.66V

The substance having highest positive E^o potential will always get reduced and will undergo reduction reaction. Here, fluorine will undergo reduction reaction will get reduced.

Aluminium will undergo oxidation reaction and will get oxidized.

Substance getting oxidized always act as anode and the one getting reduced always act as cathode.

To calculate the E^o_{cell} of the reaction, we use the equation:

E^o_{cell}=E^o_{cathode}-E^o_{anode}

E^o_{cell}=2.87-(-1.66)=4.53V

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