Question

What total energy (in kJ) is contained in 1.0 mol of photons, all with a frequency of 2.75*10^14 Hz

Answer 1

Answer:

$1.1 \times 10^{5} J$

Explanation:

The computation is shown below:

Data provided in the question

The frequency of the radio wave is f =  $2.75 \times 10^{14}\ Hz$

Let us assume the number of photons is N $= nNA = 1 \times 6.022 \times 10^{23}$

= $6.022 \times 10^{23}$

And, h = $6.626 \times 10{-34} J$

Based on the above information, the total energy is

As we know that

E = N h f

$= 6.022 \times 10^{23} \times 6.626 \times 10^{-34} \times 2.75 \times 10^{14}$

$= 1.1 \times 10^{5} J$

We just applied the above formula so that the total energy contained could come i.e by multiplying the three items so that the correct value could come