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lord [1]
2 years ago
4

If a concentration of 10 fluorescent molecules per μm2of cell membrane is needed to visualize a cell under the microscope, how m

any molecules of dye would be needed to visualize a single egg? Enter your answer in scientific notation rounded to two significant figures.
Chemistry
1 answer:
Feliz [49]2 years ago
8 0

Answer : 78500 molecules of dye would be needed to visualize a single egg.

Explanation : An single egg cell has an diameter of 100 μm which is an approximate value.

To calculate the area of the cell membrane we can use this formula.

A = π (100)^{2} / 4;

Therefore, A = 3.14 X (100)^{2} / 4

So, A =  7850 μm^{2}

Now. to calculate the amount of dye molecules needed for 10 fluorescent molecules / μm^{2}

will be;

as 1 μm^{2} = 7850 μm^{2} dye molecules.

Then 10 fluorescent molecules will need;

7850 X 10 = 78500 molecules of dye.

Therefore, the answer is 78500 molecules of dye.

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Consider the balanced equation below. 4NH3 + 3O2 --> 2N2 + 6H2O What is the mole ratio of NH3 to N2?
AURORKA [14]
The balanced equation given is:
4NH3 + 3O2 .....> 2N2 + 6H2O

From this equation, we can note that 4 moles of NH3 are required to produce 2 moles of N2.

Therefore, the mole ratio of NH3 to N2 is 4:2 which can be simplified into 2:1
4 0
2 years ago
Read 2 more answers
2KOH+H2SO4=k2SO4+2H2O Is a balanced equation, displaying the combination of potassium hydroxide with sulfuric acid increase pota
Lerok [7]

Answer:

The number of moles of potassium hydroxide, KOH required to make 4 moles of K₂SO₄ is 8 moles of KOH

Explanation:

2KOH + H₂SO₄ → K₂SO₄ + 2H₂O

From the above reaction, we have 2 moles of KOH combining with 1 mole of H₂SO₄ to produce 1 mole of K₂SO₄  and 2 moles of H₂O.

Therefore the number of moles of potassium hydroxide that will be needed to make 4 moles of K₂SO₄ is;

8KOH + 4H₂SO₄ → 4K₂SO₄ + 8H₂O

8 moles of KOH is required to make 4 moles of K₂SO₄.

6 0
2 years ago
A sample of fluorine gas is confined in a 5.0-L container at 0.432 atm and 37 °C. How many moles of gas are in this sample?
Ahat [919]

Answer:

About 0.08486 moles

Explanation:

PV=nRT, when P is the pressure in atmospheres, V is the volume in liters, n is the number of moles, R is the universal gas constant, and T is the temperature in Kelvin.

0.432 \cdot 5= n \cdot 0.0821 \cdot 310

n\approx 0.08486 moles

Hope this helps!

7 0
2 years ago
A 0.286-g sample of gas occupies 125 ml at 60. cm of hg and 25°
irga5000 [103]
Using the Equation: PV=nRT
Where P is the pressure 60 cmHg or 600 mmHg or 600/760= 0.789 atm
V is the volume 125 ml or 0.125 L, n is the number of moles, R is a constant 0.082057, and T is temperature 25 °C or 298 K; 
Therefore:
0.789 × 0.125 = n × 0.082057 × 298
 n = 0.0987/24.45 
    = 0.004036 mol
0.004036 mole has a mass of  0.286 g
Hence; 1 mole has a mass of 0.286/0.004036 
  = 70.8 g /mol
Therefore the molar mass of the gas is 71 g/mol (2 sfg)

     

4 0
2 years ago
A sample of 0.6760 g of an unknown compound containing barium ions (ba2+) is dissolved in water and treated with an excess of na
notka56 [123]

Answer: 35.72 % of Barium ions will be present in the original unknown compound.

Explanation: The reaction of Barium ions and sodium sulfate is:

Na_2SO_4(aq.)+Ba^{2+}(aq.)\rightarrow BaSO_4(s)+2Na^+(aq.)

Here, Sodium sulfate is present in excess, Barium ions are the limiting reagent because it limits the formation of product.

Now, 1 mole of barium sulfate is produced by 1 mole of Barium ions.

Molar mass of Barium sulfate = 233.38 g/mol

Molar mass of Barium ions = 137.327 g/mol

233.38 g/mol of barium sulfate will be produced by 137.323 g/mol of Barium ions, so

0.4105 grams of barium sulfate will be produced by = \frac{137.327g/mol}{233.38g/mol}\times 0.4105g of Barium ions

Mass of barium ions = 0.2415 grams

To calculate percentage by mass, we use the formula:

\% mass=\frac{\text{Mass of solute (in grams)}}{\text{Total mass of the solution(in grams)}}\times 100

Mass of the solution = 0.6760 grams

Putting the value in above equation, we get

\% \text{ mass of }Ba^{2+}\text{ ions}=\frac{0.2415g}{0.6760g}\times 100

% mass of Barium ions = 35.72%.

8 0
2 years ago
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