Calculating Boltzmann's Constant (k) with h=6.6E23

  • Thread starter Thread starter PStudent111
  • Start date Start date
  • Tags Tags
    Constant
AI Thread Summary
To calculate Boltzmann's constant (k) using Planck's constant (h=6.6E23), the equations E = kT and E = hv are utilized. The approach involves substituting E with hv and rearranging to express k in terms of h, wavelength (lambda), and temperature (T). The discussion indicates confusion at the step of isolating k, particularly when relating frequency and wavelength. The final goal is to demonstrate that k equals 0.71 cm-1 deg-1. Clarification on the calculations and units is needed to reach the correct conclusion.
PStudent111
Messages
7
Reaction score
0

Homework Statement


Using h=6.6E23, show that k (Boltzmann constant) = 0.71 cm-1 deg-1? (




Homework Equations



E = kT
E = hv

...?

The Attempt at a Solution


The only approach I can think of is:

1. E = hv
2. kT = hv
3. k = hv/T
4. Since v = c/lambda, k = hc/(lambda)T

But, I am stuck at the step above...
 
Physics news on Phys.org
h=6.6E23
sure
??
 
I believe it's

E = kT = hf = (hc)/\lambda
then
1/(T\lambda)=k/(hc)
 
janhaa said:
h=6.6E23
sure
??

E-34, my bad
 
Thread 'Confusion regarding a chemical kinetics problem'
TL;DR Summary: cannot find out error in solution proposed. [![question with rate laws][1]][1] Now the rate law for the reaction (i.e reaction rate) can be written as: $$ R= k[N_2O_5] $$ my main question is, WHAT is this reaction equal to? what I mean here is, whether $$k[N_2O_5]= -d[N_2O_5]/dt$$ or is it $$k[N_2O_5]= -1/2 \frac{d}{dt} [N_2O_5] $$ ? The latter seems to be more apt, as the reaction rate must be -1/2 (disappearance rate of N2O5), which adheres to the stoichiometry of the...
Back
Top