A volatile organic liquid with known molecular weight is added to a vapor density flask which has a known volume. The flask is h
1 answer:
Answer: Mass of the condensed vapor is 21.35 grams.
Explanation: As a gas, the Ideal Gas Law can be used to determine how many mols there are in the flask on the conditions described in question.
Temperature in K: 273 + 99.3 = 372.4K
Pressure in mmHg: P = 760.5 mmHg
Volume in L: V = 496.3. = 0.5 L
Universal Constant of Gases in mmHg: R = 62.36 L.mmHg.K⁻¹.mol⁻¹
PV = nRT
n =
n =
n = 0.1625
To determine the mass in grams:
n =
m = nM
m = 0.1625.131.4
m = 21.35
On the conditions cited above, there are <u>21.35 grams</u> of the unknown condensed vapor
You might be interested in
Explanation:
;ewFim,jhbuikew d
The energy for the transition:
The energy for the transfer of an electron from the n=2 level to the n=5 level of a hydrogen atom is 4.57 x J
Calculation:
We are aware of the energy levels as n=2 and n=5. So, we may determine the wavelength of the photon released by the electron during this transition using Rydberg's equation:
1/λ = R x (1/ - 1/
)
where,
1/λ = the wavelength of the emitted photon,
R = Rydberg's constant, 1.0974 x
= the final energy level = 5
= the initial energy level = 2
Now, put the value in the above equation, we get,
1/λ = 1.0974 x x ( 1/
- 1/
)
1/λ = 1.0974 x x (-0.21)
1/λ = -0.23 x
λ = 4.347 x m
Since, E = hc/λ
where,
h = Plank's constant = 6.626 x Js
c = speed of light = 3 x m/s
So, the transition energy for your particular transition is,
E = 6.626 x x 3 x
/ (4.347 x
)
E = 4.57 x J
Learn more about Rydberg's formula here,
#SPJ4