If 1.30 grams of a protein (non -electrolyte) are added to a 100.0 mL of water, the osmotic pressure of the resulting solution is 0.0074 atm at 298 K. What is the molar mass of the protein ?

M = 0.43× 10⁵ g/mol

Explanation:

Given data:

Mass of protein = 1.30 g

Volume of water = 100.0 mL ( 100/1000 =0.1 L)

Pressure of solution = 0.0074 atm

Temperature = 298 K

Molar mass of protein = ?

Solution:

Formula:

PV = nRT

n = PV / RT

n = 0.0074 atm ×0.1 L / 0.0821 atm. L / mol.K × 298 K

n = 0.00074 / 24.5 /mol

n = 3.0 × 10⁻⁵ mol

Molar mass of protein:

Number of moles = mass /  molar mass

3.0 × 10⁻⁵ mol = 1.30 g/ M

M = 1.30 g/  3.0 × 10⁻⁵ mol

M = 0.43× 10⁵ g/mol

1.consider the following balanced equation and answer parts a through. show calculations for each part.  

3 ag(s) + 4 hno3(aq) → 3 agno3(aq) + no(g) + 2 h2o(l)  

a. calculate the number of moles of agno3 produced by the reaction of 3 moles of ag with excess hno3. if the number to the left of the compound represents the number of moles of the compound which are present, then 3 moles of ag react with 4 moles hno3 to produce 3 moles agno3 (aq).

so the answer to a would be 3 moles.

b. calculate the number of moles of agno3 produced by the reaction of 108 grams of ag with excess hno3.  

i'm not sure how to plug in the grams of silver into an equation using moles to find how many moles are produced.

c. calculate the number of grams of agno3 produced by the reaction of 108 grams of ag with excess hno3  

d. calculate the number of moles of no produced as a byproduct of the reaction of 108 grams of ag with excess hno3.  

e. calculate the number of grams of no produced as a byproduct starting with 108 grams of ag and excess hno3.  

explanation:

answer: c.

explanation: