If the amount of dissolved solute in a solution at a given temperature is greater than the amount that can permanently remain in
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Answer:
The final volume of air after compression: V₂ = 4477.63 L = 158.12 cf
Explanation:
Given: Initial gauge pressure of the gas = 0 psi
Initial absolute pressure of the gas: P₁ = gauge pressure + atmospheric pressure = 0 psi + 12.20 psi = 12.20 psi
Initial Temperature = 70°F
⇒ T₁ = (70°F − 32) × 5/9 + 273.15 = 294.26 K
Initial volume of the gas: V₁ = 1200 cf = 1200 × 28.317 = 33980.4 L (∵ 1 cf ≈ 28.317 L)
Final gauge pressure of the gas = 90 psi
Final absolute pressure of the gas: P₂ = gauge pressure + atmospheric pressure = 90 psi + 12.20 psi = 102.2 psi
Final Temperature: T₂ = 125°F
⇒ T₂ = (125°F − 32) × 5/9 + 273.15 = 324.82 K
Final volume of the gas: V₂ = ? L
<u>According to the </u><u>Combined gas law</u><u>:</u>
→
→
→
<u>Therefore, the final volume of air after compression: </u><u>V₂ = 4477.63 L = 158.12 cf</u>
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,
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