Question

(d) calculate the molar absorptivity (ε) of cu2+ at 620 nm given that the cuvettes used in lab had a pathlength of 1.00 cm.

Answer 1

The working equation to be used for our calculations is taken from Beer's Law which is about the absorption of light by the particles in a solution. The equation is written below.

A = ∈LC
where
A is the absorbance
∈ is the molar absorptivity
L is the path length
C is the molar concentration of the solution

Solving for ∈,

∈ = A/LC = A/(1)(C) = A/C

Therefore, the molar absorptivity is equal to the absorbance divided by the molar concentration. (I can't give an exact answer because A and C are not specified)

Answer 2

We do not have the absorbance and concentration hence the question can not be solved.

We define the absorbance of a solution from Beer Lambert's law. From the law we know that;

A = εcl

ε = molar absorptivity

c = concentration

l = path length

In the values given, we have the values of molar absorptivity and path length but we do not have the absorbance and concentration hence the question can not be solved.

Learn more about Beer law: https://brainly.com/question/7184331