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max2010maxim [7]
3 years ago
13

What elements are found in ammonia

Chemistry
2 answers:
nalin [4]3 years ago
4 0
Answer: Nitrogen<span> and H</span><span>ydrogen</span>
Kobotan [32]3 years ago
3 0
Ammonia is <span>colorless gas composed of </span>nitrogen<span> and </span><span>hydrogen</span>
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Only valence electrons can be shared stolen or given away<br><br> True <br><br> False
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false

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A student is participating in the school science fair. She wants to investigate household cleaners.
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A science club made pine wood cars. Each car was set on the same track and then released. The distance traveled was measured. Li
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Isn't this a math problem?
If it is the the answer should be 102.

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7 0
3 years ago
5. Inside the mouth, these cells are joined together in a sheet. Why are they scattered here?
anyanavicka [17]

Answer:

Inside the mouth, these cells are joined together in a sheet. Why are they scattered here? They are scattered here because we disrupted there original form by scrapping them off our mouths and smearing them on the slide.

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5 0
3 years ago
A solution made by dissolving 33 mg of insulin in 6.5 mL of water has an osmotic pressure of 15.5 mmHg at 25°C. Calculate the mo
Liula [17]

<u>Answer:</u> The molar mass of the insulin is 6087.2 g/mol

<u>Explanation:</u>

To calculate the concentration of solute, we use the equation for osmotic pressure, which is:

\pi=iMRT

Or,

\pi=i\times \frac{\text{Mass of solute}\times 1000}{\text{Molar mass of solute}\times \text{Volume of solution (in mL)}}\times RT

where,

\pi = osmotic pressure of the solution = 15.5 mmHg

i = Van't hoff factor = 1 (for non-electrolytes)

Mass of solute (insulin) = 33 mg = 0.033 g   (Conversion factor: 1 g = 1000 mg)

Volume of solution = 6.5 mL

R = Gas constant = 62.364\text{ L.mmHg }mol^{-1}K^{-1}

T = temperature of the solution = 25^oC=[273+25]=298K

Putting values in above equation, we get:

15.5mmHg=1\times \frac{0.033\times 1000}{\text{Molar mass of insulin}\times 6.5}\times 62.364\text{ L.mmHg }mol^{-1}K^{-1}\times 298K\\\\\text{molar mass of insulin}=\frac{1\times 0.033\times 1000\times 62.364\times 298}{15.5\times 6.5}=6087.2g/mol

Hence, the molar mass of the insulin is 6087.2 g/mol

8 0
3 years ago
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