Answer:
D.
Explanation:
CH₃C≡ CCH₂CH₂Cl
Since there are 5 carbons so the suffix used is "pent"
There is a triple bond so its alkyne
So the compound becomes 2-pentyne (2 because the triple bond is with the 2nd carbon)
Then,
The functional group of chlorine is attached with 5th carbon So the compound becomes
5-chloro,2-pentyne
1. <em>Describe</em>
Frequency (f) and wavelength (λ) are inversely related.
f ∝ 1/λ
As one goes up, the other goes down and vice versa.
2. <em>Infer
</em>
The frequency of infrared light is less than that of red light, so infra could mean something like less than or below or beneath.
Ultrahigh frequencies are extremely high compared with those of visible light. Ultrasound has frequencies that are far beyond what we can hear. An ultracentrifuge goes at extremely high speed, and an ultramicroscope can “see” tiny structures. Ultra could probably mean something like extremely or far beyond.
3. <em>Analyze
</em>
Energy is directly proportional to frequency (E ∝ f).
Frequency is inversely proportional to wavelength (f ∝ 1/λ).
Energy is inversely proportional to wavelength (E ∝ 1/λ).
Mole of electron required by
mole is 
- Faraday law expressed how the change that is been being produced by a current at an electrode-electrolyte interface is related and proportional to the quantity of electricity that is been used.
- There is one mole of electron required for 1 Faraday of electricity.
- Avogadro constant is

- Mole of electron can be calculated by dividing the number of electron by avogadro's constant.
=
= 
Therefore, it requires
Faraday of electricity for the 
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The partial pressure of oxygen, P(O₂) is 198.83 mmHg.
<h3>What is partial pressure of a gas?</h3>
The partial pressure of a gas is the pressure gas will exert in a mixture of gases which do not react chemically together.
The sum of partial pressure of gases at atmospheric pressure = 760 mmHg
P(N₂) + P(H₂O) + P(CO₂) + P(O₂) + P(other) = 760 mmHg
P(N₂) = 0.72 atm = 547.2 mmHg
P(H₂O) = 7.7 torr = 7.7 mmHg
P(CO₂) = 0.37 mmHg
P(other) = 0.97 kPa = 5.9 mmHg
P(O₂) = 760 - (547.2 + 7.7 + 0.37 + 5.9) = 198.83 mmHg
Therefore, the partial pressure of oxygen, P(O₂) is 198.83 mmHg.
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The pressure of the gas is 1.0 bar.
<em>pV</em> = <em>nRT</em>
<em>T</em> = (0 + 273.15) K = 273.15 K
<em>p</em> = (<em>nRT</em>)/<em>V</em> = (2.0 mol × 0.083 14 bar·L·K⁻¹mol⁻¹ × 273.15 K)/44.8 L = 1.0 bar