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CHXI02:STRUCTURE OF ATOM

307430 Which of the following relates to photons both as wave motion and stream of particles?

1

I n t e r f e r e n c e

2

E = m c^{2}

3

D i f f r a c t i o n

4

E = h v

Explanation:

According to Planck’s quantum theory, $E = h v = \frac{h c}{λ}$

CHXI02:STRUCTURE OF ATOM

307431 Calculate the wavelength of light required to break the bond between two chlorine atoms in a chlorine molecule. $T h e C l - C l b o n d e n e r g y i s 243 k J m o l^{- 1} \cdot$
$(h = 6.6 \times 10^{- 34} J s, c = 3 \times 10^{8} m / s$ , Avogadro's number $h = 6.02 \times 10^{23} {mol}^{- 1}$ )

1

4.91 \times 10^{- 7} m

2

4.11 \times 10^{- 6} m

3

8.81 \times 10^{- 31} m

4

6.26 \times 10^{- 21} m

Explanation:

Energy required to break one $Cl - Cl$ bond
$= \frac{B o n d e n e r g y p e r m o l e}{A v a g a d r o^{'} s n u m b e r}$
$E = \frac{243 \times 10^{3}}{6.023 \times 10^{23}} J$
Let the wavelength of the photon to cause rupture of one $Cl - Cl$ bond be $λ$ .
$λ = \frac{h c}{E}$
$= \frac{6.6 \times 10^{- 34} \times 3 \times 10^{8} \times 6.023 \times 10^{23}}{243 \times 10^{3}}$
$= \frac{119.255}{243} \times 10^{- 34} \times 10^{31} \times 10^{- 3}$
$= 4.91 \times 10^{- 7}$ m

CHXI02:STRUCTURE OF ATOM

307432 Calculate the energy in joule corresponding to light of wavelength 45 nm: (Planck’s constant $h = 6 .63 \times 1 0^{- 34} J s;$ speed of light $c = 3 \times 1 0^{8} m s^{- 1})$

1

6 .67 \times 1 0^{15}

2

6 .67 \times 1 0^{11}

3

4 .42 \times 1 0^{- 15}

4

4 .42 \times 1 0^{- 18}

Explanation:

$\frac{h c}{λ} = \frac{6 .63 \times 1 0^{- 34} \times 3 \times 1 0^{8}}{45 \times 1 0^{- 9}}$
$= 4 .42 \times 1 0^{- 18} J$

CHXI02:STRUCTURE OF ATOM

307433 Nitrogen laser produces a radiation at a wavelength of $337.1 nm$ . If the number of photons emitted is $5.6 \times 10^{24}$ . Calculate the power of this laser.

1

3.33 \times 10^{6} J

2

3.33 \times 10^{5} J

3

1.56 \times 10^{6} J

4

15.6 \times 10^{8} J

Explanation:

$E = \frac{nhc}{λ}$
$= \frac{5.6 \times 10^{24} \times 6.602 \times 10^{- 34} J . S \times 3 \times 10^{8} m \cdot S^{-}}{337.1 \times 10^{- 9} m}$ $= 3.33 \times 10^{6} J$

CHXI02:STRUCTURE OF ATOM

307430 Which of the following relates to photons both as wave motion and stream of particles?

1

I n t e r f e r e n c e

2

E = m c^{2}

3

D i f f r a c t i o n

4

E = h v

Explanation:

According to Planck’s quantum theory, $E = h v = \frac{h c}{λ}$

CHXI02:STRUCTURE OF ATOM

307431 Calculate the wavelength of light required to break the bond between two chlorine atoms in a chlorine molecule. $T h e C l - C l b o n d e n e r g y i s 243 k J m o l^{- 1} \cdot$
$(h = 6.6 \times 10^{- 34} J s, c = 3 \times 10^{8} m / s$ , Avogadro's number $h = 6.02 \times 10^{23} {mol}^{- 1}$ )

1

4.91 \times 10^{- 7} m

2

4.11 \times 10^{- 6} m

3

8.81 \times 10^{- 31} m

4

6.26 \times 10^{- 21} m

Explanation:

Energy required to break one $Cl - Cl$ bond
$= \frac{B o n d e n e r g y p e r m o l e}{A v a g a d r o^{'} s n u m b e r}$
$E = \frac{243 \times 10^{3}}{6.023 \times 10^{23}} J$
Let the wavelength of the photon to cause rupture of one $Cl - Cl$ bond be $λ$ .
$λ = \frac{h c}{E}$
$= \frac{6.6 \times 10^{- 34} \times 3 \times 10^{8} \times 6.023 \times 10^{23}}{243 \times 10^{3}}$
$= \frac{119.255}{243} \times 10^{- 34} \times 10^{31} \times 10^{- 3}$
$= 4.91 \times 10^{- 7}$ m

CHXI02:STRUCTURE OF ATOM

307432 Calculate the energy in joule corresponding to light of wavelength 45 nm: (Planck’s constant $h = 6 .63 \times 1 0^{- 34} J s;$ speed of light $c = 3 \times 1 0^{8} m s^{- 1})$

1

6 .67 \times 1 0^{15}

2

6 .67 \times 1 0^{11}

3

4 .42 \times 1 0^{- 15}

4

4 .42 \times 1 0^{- 18}

Explanation:

$\frac{h c}{λ} = \frac{6 .63 \times 1 0^{- 34} \times 3 \times 1 0^{8}}{45 \times 1 0^{- 9}}$
$= 4 .42 \times 1 0^{- 18} J$

CHXI02:STRUCTURE OF ATOM

307433 Nitrogen laser produces a radiation at a wavelength of $337.1 nm$ . If the number of photons emitted is $5.6 \times 10^{24}$ . Calculate the power of this laser.

1

3.33 \times 10^{6} J

2

3.33 \times 10^{5} J

3

1.56 \times 10^{6} J

4

15.6 \times 10^{8} J

Explanation:

$E = \frac{nhc}{λ}$
$= \frac{5.6 \times 10^{24} \times 6.602 \times 10^{- 34} J . S \times 3 \times 10^{8} m \cdot S^{-}}{337.1 \times 10^{- 9} m}$ $= 3.33 \times 10^{6} J$

CHXI02:STRUCTURE OF ATOM

307430 Which of the following relates to photons both as wave motion and stream of particles?

1

I n t e r f e r e n c e

2

E = m c^{2}

3

D i f f r a c t i o n

4

E = h v

Explanation:

According to Planck’s quantum theory, $E = h v = \frac{h c}{λ}$

CHXI02:STRUCTURE OF ATOM

307431 Calculate the wavelength of light required to break the bond between two chlorine atoms in a chlorine molecule. $T h e C l - C l b o n d e n e r g y i s 243 k J m o l^{- 1} \cdot$
$(h = 6.6 \times 10^{- 34} J s, c = 3 \times 10^{8} m / s$ , Avogadro's number $h = 6.02 \times 10^{23} {mol}^{- 1}$ )

1

4.91 \times 10^{- 7} m

2

4.11 \times 10^{- 6} m

3

8.81 \times 10^{- 31} m

4

6.26 \times 10^{- 21} m

Explanation:

Energy required to break one $Cl - Cl$ bond
$= \frac{B o n d e n e r g y p e r m o l e}{A v a g a d r o^{'} s n u m b e r}$
$E = \frac{243 \times 10^{3}}{6.023 \times 10^{23}} J$
Let the wavelength of the photon to cause rupture of one $Cl - Cl$ bond be $λ$ .
$λ = \frac{h c}{E}$
$= \frac{6.6 \times 10^{- 34} \times 3 \times 10^{8} \times 6.023 \times 10^{23}}{243 \times 10^{3}}$
$= \frac{119.255}{243} \times 10^{- 34} \times 10^{31} \times 10^{- 3}$
$= 4.91 \times 10^{- 7}$ m

CHXI02:STRUCTURE OF ATOM

307432 Calculate the energy in joule corresponding to light of wavelength 45 nm: (Planck’s constant $h = 6 .63 \times 1 0^{- 34} J s;$ speed of light $c = 3 \times 1 0^{8} m s^{- 1})$

1

6 .67 \times 1 0^{15}

2

6 .67 \times 1 0^{11}

3

4 .42 \times 1 0^{- 15}

4

4 .42 \times 1 0^{- 18}

Explanation:

$\frac{h c}{λ} = \frac{6 .63 \times 1 0^{- 34} \times 3 \times 1 0^{8}}{45 \times 1 0^{- 9}}$
$= 4 .42 \times 1 0^{- 18} J$

CHXI02:STRUCTURE OF ATOM

307433 Nitrogen laser produces a radiation at a wavelength of $337.1 nm$ . If the number of photons emitted is $5.6 \times 10^{24}$ . Calculate the power of this laser.

1

3.33 \times 10^{6} J

2

3.33 \times 10^{5} J

3

1.56 \times 10^{6} J

4

15.6 \times 10^{8} J

Explanation:

$E = \frac{nhc}{λ}$
$= \frac{5.6 \times 10^{24} \times 6.602 \times 10^{- 34} J . S \times 3 \times 10^{8} m \cdot S^{-}}{337.1 \times 10^{- 9} m}$ $= 3.33 \times 10^{6} J$

CHXI02:STRUCTURE OF ATOM

307430 Which of the following relates to photons both as wave motion and stream of particles?

1

I n t e r f e r e n c e

2

E = m c^{2}

3

D i f f r a c t i o n

4

E = h v

Explanation:

According to Planck’s quantum theory, $E = h v = \frac{h c}{λ}$

CHXI02:STRUCTURE OF ATOM

307431 Calculate the wavelength of light required to break the bond between two chlorine atoms in a chlorine molecule. $T h e C l - C l b o n d e n e r g y i s 243 k J m o l^{- 1} \cdot$
$(h = 6.6 \times 10^{- 34} J s, c = 3 \times 10^{8} m / s$ , Avogadro's number $h = 6.02 \times 10^{23} {mol}^{- 1}$ )

1

4.91 \times 10^{- 7} m

2

4.11 \times 10^{- 6} m

3

8.81 \times 10^{- 31} m

4

6.26 \times 10^{- 21} m

Explanation:

Energy required to break one $Cl - Cl$ bond
$= \frac{B o n d e n e r g y p e r m o l e}{A v a g a d r o^{'} s n u m b e r}$
$E = \frac{243 \times 10^{3}}{6.023 \times 10^{23}} J$
Let the wavelength of the photon to cause rupture of one $Cl - Cl$ bond be $λ$ .
$λ = \frac{h c}{E}$
$= \frac{6.6 \times 10^{- 34} \times 3 \times 10^{8} \times 6.023 \times 10^{23}}{243 \times 10^{3}}$
$= \frac{119.255}{243} \times 10^{- 34} \times 10^{31} \times 10^{- 3}$
$= 4.91 \times 10^{- 7}$ m

CHXI02:STRUCTURE OF ATOM

307432 Calculate the energy in joule corresponding to light of wavelength 45 nm: (Planck’s constant $h = 6 .63 \times 1 0^{- 34} J s;$ speed of light $c = 3 \times 1 0^{8} m s^{- 1})$

1

6 .67 \times 1 0^{15}

2

6 .67 \times 1 0^{11}

3

4 .42 \times 1 0^{- 15}

4

4 .42 \times 1 0^{- 18}

Explanation:

$\frac{h c}{λ} = \frac{6 .63 \times 1 0^{- 34} \times 3 \times 1 0^{8}}{45 \times 1 0^{- 9}}$
$= 4 .42 \times 1 0^{- 18} J$

CHXI02:STRUCTURE OF ATOM

307433 Nitrogen laser produces a radiation at a wavelength of $337.1 nm$ . If the number of photons emitted is $5.6 \times 10^{24}$ . Calculate the power of this laser.

1

3.33 \times 10^{6} J

2

3.33 \times 10^{5} J

3

1.56 \times 10^{6} J

4

15.6 \times 10^{8} J

Explanation:

$E = \frac{nhc}{λ}$
$= \frac{5.6 \times 10^{24} \times 6.602 \times 10^{- 34} J . S \times 3 \times 10^{8} m \cdot S^{-}}{337.1 \times 10^{- 9} m}$ $= 3.33 \times 10^{6} J$

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