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Romashka [77]
3 years ago
6

The cell cycle can be divided into two phases interphase and mitosis (cell division), Mitosis is further subdivided into prophas

e, metaphase, anaphase, and telophase.
A lab technician observed 200 cells from a cell line and recorded the number of cells in each phase of the cell cycle. The results are shown in the table.
Number of Cells Observed
(out of 200)
Phase Number of Cells Observed
Interphase
170
prophase
metaphase
anaphase
telophase
Based on the data, what is the probability a randomly chosen cell will be observed undergoing cell division?
You may use the calculator,
A 15%
B. 18%
C 30%
D. 85%
Chemistry
2 answers:
stealth61 [152]3 years ago
7 0
Well the answer is C
docker41 [41]3 years ago
3 0

the answer to this is c i hope this helped

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Air is made up of different gases, such as oxygen, nitrogen, and carbon dioxide.
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Determine the electron configuration of nitrogen numerically.
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What volume (in mL) of a 0.113 M NaCl solution contains 0.087 mol NaCl?
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If 0.500 mol neon at 1.00 atm and 273 K expands against a constant external pressure of 0.100 atm until the gas pressure reaches
trapecia [35]

Answer:

The work done on neon = -323 J

The internal energy change= -392.84 J

The heat absorbed by neon = -69.84 J

Explanation:

Step 1: Data given

Number of moles  = 0.500 moles

Pressure  = 1 atm

Temperature  = 273 Kelvin

The pressure will change from 1.00 atm to 0.200 atm. The temperature changes from 273 to 210 Kelvin.

a) calculate the work done on neon

W = -P(V2-V1)    

⇒ with P = the pressure = 0.1 atm

⇒ with V1 = the initial volume = nRTi /Pi

⇒ with V2 = the final volume = nRTf /Pf

W = -PnR((T2/P2) -(T1/P1))

⇒ with T2 = the final temperature = 210 K

 ⇒ with T1 = the initial temperature = 273 K

 ⇒ with P2 = the final pressure = 0.200 atm

 ⇒ with P1 = the initial pressure = 1.00 atm

W = -nR (210*(0.1/0.2) - 273*(0.1/1.00))

W = -nR*(105 - 27.3)

W= -(0.500)*(8.314)*(77.7)

W = -323 J

b) calculate the internal energy change

E = (3/2)*nRT

ΔE = Ef - Ei

ΔE =(3/2)*nR(T2-T1)

⇒ with n= number of moles = 0.500 moles

⇒ with T2 =the final temperature = 210 K

⇒ with T1 = the initial temperature = 273 K

ΔE = (3/2)*(0.5)*(8.314)(210-273)

ΔE = -392.84 J

c) Calculate the heat absorbed by neon

ΔE = q + W

q = ΔE -W

⇒ with ΔE = -392.84 J

⇒ with W = -323 J

q = -392.84 J -( -323 J)

q =-392.84 J + 323 J

q = -69.84 J

4 0
3 years ago
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