<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:

Or,

where,
= 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 = 
T = temperature of the solution = ![25^oC=[273+25]=298K](https://tex.z-dn.net/?f=25%5EoC%3D%5B273%2B25%5D%3D298K)
Putting values in above equation, we get:

Hence, the molar mass of the insulin is 6087.2 g/mol
1. Complete ionization in water.
2. Ionization constant.
3. A good hydrogen-ion acceptor.
4. Weak acid.
5. This base ionizes slightly in aqueous.
I really hope this answer helps you out! It makes my day helping people like you and giving back to the community that has helped me through school! If you could do me a favor, if this helped you and this is the very best answer and you understand that all of my answers are legit and top notch. Please mark as brainliest! Thanks and have a awesome day!
All problems are caused by a factor in which human beings play an important role in its cause.
Answer:
Please one time click here
Mark brainliest
Work out the number of moles in
100.00 grams of the oxide.
For nitrogen: The atomic mass of N is 14.0067, and we have 36.84 g N:
36.84 g N14.0067 g N/mol N=2.630 mol N
For oxygen: The atomic mass of O is
15.9994, and we have
100.00−36.84=63.16 g O:
63.16 g N 15.9994 g N/mol N=3.948 mol N
Now the ratio 3.958 2.630 is very close to
1.5=32
. So we conclude that the gas has three moles
O to two moles N making the empirical formula
N2O3.
<h2>
<u>Mark as Brainliest</u></h2>