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Byju's Answer

Standard XII

Chemistry

Reasons of Stability

The energy re...

Question

The energy required to break one mole of $C l - C l$ bond in ${C l}_{2}$ in $242 k J {m o l}^{- 1}$ . 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 $N_{A} = 6.02 \times 10^{23} {m o l}^{- 1}$ ]

594 nm

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640 nm

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700 nm

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494 nm

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Solution

The correct option is A 494 nm
Energy if $C l - C l$ bond $= - 242 k J / ㏖ = 4.02 \times 10^{- 19} J / ㏖$

Now, $\frac{h c}{λ} = E \Rightarrow λ = \frac{h c}{E} = \frac{h c}{4.02 \times 10^{- 19}}$

$= 494 ㎚$

Hence, the correct option is $D$

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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 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})

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 Cl–Cl bonds in

C l_{2}

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})

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 bond in Cl2 in 242 kJ mol−1 . The longest wavelength of light capable of breaking a single Cl−Cl bond is: [c=3×104ms−1 and NA=6.02×1023mol−1]

The correct option is A 494 nmEnergy if Cl−Cl bond=−242kJ/㏖=4.02×10−19J/㏖Now,hcλ=E⇒λ=hcE=hc4.02×10−19=494㎚ Hence, the correct option is D

The energy required to break one mole of $C l - C l$ bond in ${C l}_{2}$ in $242 k J {m o l}^{- 1}$ . 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 $N_{A} = 6.02 \times 10^{23} {m o l}^{- 1}$ ]

The correct option is A 494 nm
Energy if $C l - C l$ bond $= - 242 k J / ㏖ = 4.02 \times 10^{- 19} J / ㏖$

Now, $\frac{h c}{λ} = E \Rightarrow λ = \frac{h c}{E} = \frac{h c}{4.02 \times 10^{- 19}}$

$= 494 ㎚$

Hence, the correct option is $D$