Question

According to law of photochemical equivalence the energy absorbed (in ergs/mole) is given as (h = 6.62 × 10⁻²⁷ ergs, c = 3 × 10¹⁰ cm s⁻¹, $N_A$ = 6.02 × 10²³ mol⁻¹)
(a) $\frac{1.196 x 10^{16}}{\lambda}$
(b) $\frac{1.196 x 10^{8}}{\lambda}$
(c) $\frac{2.859 x 10^5}{\lambda}$
(d) $\frac{2.859 x 10^16}{\lambda}$

Answer 1

Answer:

b) 1.196 × 10~8/ λ

Explanation:

The photochemical equivalence law, relates to the chemical reactions that are induced by light, which states that for every quantum of a radiation which is absorbed, there is one molecule of the substance that reacts.

Energy absorbed in the mole = h = 6.62 × 10⁻²⁷ ergs (Given)

c = 3 × 10¹⁰ cm s⁻¹ (Given)

N_A = 6.02 × 10²³ mol⁻¹ (Given)

Thus,

E = HcNa/λ

= 6.62 × 10⁻²⁷ × 3×10¹⁰ × 6.02 × 10²³/λ

= 1.1955 × 10~8/ λ

=  1.196 × 10~8/ λ mol

Therefore, according to the law of photochemical equivalence the energy absorbed (in ergs/mole) is given as 1.196 × 10~8/ λ.

Answer 2

Explanation:

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answer:-option b