Bond energy of Br 2 is 194 kJ mol -1 . If the minimum wave number of photons required to break this bond is given as X × 106 m -1, then the value of X will be (h=6.62 × 10-34 Js , c=3 × 108 m / s )

Question

Bond energy of Br 2 is 194 kJ mol -1 . If the minimum wave number of photons required to break this bond is given as X × 106 m -1, then the value of X will be (h=6.62 × 10-34 Js , c=3 × 108 m / s ) (A)  (B)  (C)  (D)

Tardigrade Admin · Accepted Answer

(h c/λ) × NA=194 × 103 (1/λ)=(194 × 103/6.63 × 10-34 × 108 × 6 × 1023) ≃ 1.62 × 106 m -1

Q. Bond energy of $B r_{2}$ is $194 k J m o l^{- 1} .$ If the minimum wave number of photons required to break this bond is given as $X \times 1 0^{6} m^{- 1}$ , then the value of $X$ will be
$(h = 6.62 \times 1 0^{- 34} J s, c = 3 \times 1 0^{8} m / s)$

$\frac{h c}{λ} \times N_{A} = 194 \times 1 0^{3}$
$\frac{1}{λ} = \frac{194 \times 1 0 ^{3}}{6.63 \times 1 0 ^{- 34} \times 1 0 ^{8} \times 6 \times 1 0 ^{23}}$
$≃ 1.62 \times 1 0^{6} m^{- 1}$

Q. Bond energy of Br2​ is 194kJmol−1. If the minimum wave number of photons required to break this bond is given as X×106m−1, then the value of X will be (h=6.62×10−34Js,c=3×108m/s)

λhc​×NA​=194×103 λ1​=6.63×10−34×108×6×1023194×103​ ≃1.62×106m−1

Q. Bond energy of $B r_{2}$ is $194 k J m o l^{- 1} .$ If the minimum wave number of photons required to break this bond is given as $X \times 1 0^{6} m^{- 1}$ , then the value of $X$ will be
$(h = 6.62 \times 1 0^{- 34} J s, c = 3 \times 1 0^{8} m / s)$

$\frac{h c}{λ} \times N_{A} = 194 \times 1 0^{3}$
$\frac{1}{λ} = \frac{194 \times 1 0 ^{3}}{6.63 \times 1 0 ^{- 34} \times 1 0 ^{8} \times 6 \times 1 0 ^{23}}$
$≃ 1.62 \times 1 0^{6} m^{- 1}$