Asolution of 62.4 g of insulin in enough water to make 1.000 l of solution has an osmotic pressure of 0.305 atm at 25°c. based on these data, what is the molar mass of insulin?

Molecular Mass of insulin = 5004

Explanation:

Mass of insulin = 62.4 g

Volume of the solution = 1.00 L

Osmotic pressure = 0.305 L

Temperature = 25 °C = 25 + 273 = 298 K

PV = nRT

Where,

P = osmotic pressure

V = Volume of the solution

n = No. of moles

R gas constant = 0.08206  L atm K^{-1} Mol^{-1}

T = Temperature

PV = nRT

n = 0.01247

No. of mol = Mass in g/molecular mass

Molecular mass = Mass in g/No. of mol

Molecular mass = 62.4/0.01247

                          = 5004

it can be observed without changing the identity of the object.

it depends on what substance you're talking about as well as many other factors. in quantum mechanics, the observation of particles affects the observers ability to measure certain properties. for example: you can know the velocity of a particle, but you can't know it's position; or you can know it's position, but not it's velocity. it's like trying to find out where a grain of sand is by throwing other grains of sand at it. once you find out where it is, it's been moved. it's also like trying to find an answer to the question of whether or not a tree falling in a forest makes a sound if nobody is there to hear it. paradoxically, the only way to find out is to be there and hear it.