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Byju's Answer

Standard XII

Chemistry

1900's Physics and Wave

The energy re...

Question

The energy required to break one mole of Cl–Cl bonds in $C l_{2}$ is $242 k J m o l^{- 1}$ . The longest wavelength of light capable of breaking single Cl-Cl bond is $(c = 3 \times 10^{8} m s e c^{- 1}$ , $N_{A} = 6.023 \times 10^{23} m o l^{- 1})$

700 nm

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494 nm

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594 nm

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640 nm

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Solution

The correct option is B 494 nm
Bond energy of single bond = $\frac{242}{6.023 \times 10^{23}} = 4.017 \times 10^{- 22} K J = 4.017 \times 10^{- 19} J$
Now $E = \frac{h c}{λ}$ or $λ = \frac{h c}{E}$
$= \frac{6.626 \times 10^{- 34} \times 3 \times 10^{8}}{4.017 \times 10^{- 19}} = 494 n m$

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Similar questions

Q. The energy required to brake one mole of

C l - C l

bonds in

C l_{2}

242 k j m o l^{- 1}

. The longest wavelength of light capable of breaking single

C l - C l

bond is:

(c = 3 \times 10^{8} m s^{-} 1

and

N_{A} = 6.02 \times 10^{23} m o l^{- 1})

Q. The energy required to break one mole

C l - C l

bonds in

C l_{2}

242 K J m o l^{- 1}

. The longest wavelength of light capable of breaking a single

C l - C l

bond is:

Q. The energy required to break one mole of

C l - C l

bond in

{C l}_{2}

242 k J {m o l}^{- 1}

. The longest wavelength of light capable of breaking a single

C l - C l

bond is:

[

c = 3 \times 10^{4} {m s}^{- 1}

and

N_{A} = 6.02 \times 10^{23} {m o l}^{- 1}

]

Q. The energy required to break one mole of

C l - C l

bonds in

C l_{2}

242 {kJ mol}^{- 1}

. The longest wavelength of light capable of breaking a single

C l - C l

bond is:

(c = 3 \times 10^{8} m/s and N_{A} = 6.02 \times 10^{23} {mol}^{- 1})

Th e energy required to break one mol of Cl-Cl bonds in Cl₂ is 242 kJmol^-1. The longest wavelength of light capable of breaking a single Cl-Cl bond is

A. 594nm

B.640nm

C. 700nm

D.494nm

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The energy required to break one mole of Cl–Cl bonds in Cl2 is 242 kJ mol−1. The longest wavelength of light capable of breaking single Cl-Cl bond is (c=3×108 m sec−1, NA=6.023×1023 mol−1)

The correct option is B 494 nmBond energy of single bond = 2426.023×1023=4.017×10−22KJ=4.017×10−19J Now E=hcλ or λ=hcE =6.626×10−34×3×1084.017×10−19=494 nm

The energy required to break one mole of Cl–Cl bonds in $C l_{2}$ is $242 k J m o l^{- 1}$ . The longest wavelength of light capable of breaking single Cl-Cl bond is $(c = 3 \times 10^{8} m s e c^{- 1}$ , $N_{A} = 6.023 \times 10^{23} m o l^{- 1})$

The correct option is B 494 nm
Bond energy of single bond = $\frac{242}{6.023 \times 10^{23}} = 4.017 \times 10^{- 22} K J = 4.017 \times 10^{- 19} J$
Now $E = \frac{h c}{λ}$ or $λ = \frac{h c}{E}$
$= \frac{6.626 \times 10^{- 34} \times 3 \times 10^{8}}{4.017 \times 10^{- 19}} = 494 n m$