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Andru [333]
3 years ago
8

What does thermodynamics deal with? A. The transfer of heat and energy B. The properties of sound waves C. The movement of elect

rons D. The conservation of matter
Chemistry
2 answers:
Aneli [31]3 years ago
5 0
The correct answer is <span>A. The transfer of heat and energy

Sound waves, electron movement, and conservation of matter are studied by different parts of physics. Thermo is an ancient root word/prefix that is used to refer to heat. An example of that is a Thermos, which is supposed to save heat of a liquid.</span>
grin007 [14]3 years ago
5 0
A. The transfer of heat and energy

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What is Avogadro's number and mole?​
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What causes water to become denser when it is carried to the poles by surface currents? increased temperature and increased sali
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4 years ago
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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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