# A protein subunit from an enzyme is part of a research study and needs to be characterized. a total of 0.185 g of this subunit was dissolved in enough water to produce 2.00 ml of solution. at 28 ?c the osmotic pressure produced by the solution was 0.138 atm. what is the molar mass of the protein?

Answer:The molar mass of the protein is 16,544 g/mol.

Explanation:

Volume of the solution ,V = 2.00 ml= 0.002 L

Osmotic pressure = 0.138 atm

temperature at which solution is prepared = 28° C = 301 K()

Number of moles of protein,n=

Osmotic pressure is determined by :

The molar mass of the protein is 16,544 g/mol.

The molar mass of the protein : 16517.86 g/mol

Further explanation

Osmosis pressure is the minimum pressure given to the solution so that there is no osmotic displacement from a more dilute solution to a more concentrated solution.

General formula:

π = osmosis pressure (atm)

M = solution concentration (mol / l)

R = constant = 0.08205 L atm mol-1 K-1

T = Temperature (Kelvin)

Mass of a protein: 0.185 g

Volume: 2.00 ml of solution. at 28 C

the osmotic pressure: 0.138 atm

We enter into the equation to find moles from protein concentrations

π = M. R. T

t = 28 C + 273 = 301 K

0.138 = M. 0.08205. 301 K

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## Related Questions

Determine the moles of solute particles in 1.0 kg of a 3.0 m Ca(NO3)2 solution.

3.0 mol.

Explanation:

Molaity (m) is defined as the no. of moles of solute per kg of solvent.

m = (no. of moles of solute Ca(NO₃)₂)/(kg of solvent).

∴ no. of moles of solute Ca(NO₃)₂ = (m)(kg of solvent) = (3.0 m)(1.0 kg) = 3.0 mol.

Which type of radioactive decay does not produce any particles? a. beta decay
c. gamma decay
b. alpha decay
d. electron decay

The answer is is gamma as alpha an beta both result in the release of a particle

Calculate the number of moles of each compound, given the number of molecules. If you need to make a number a superscript, put a ^ in front of the number. For example, 2.45 x 1022 would be written as 2.45 x 10^22. 2.46 x 1021 molecules of CO2 10,000 molecules of H2O 8.75 x 1032 molecules of C6H12O6

-  4.08×10⁻³ moles of CO₂

-  1.66×10⁻²⁰ moles of H₂O

-  1453.5 moles of C₆H₁₂O₆

Explanation:

Let's determine the amount of molecules of each compound:

- 2.46×10²¹ molecules of CO₂

- 1×10⁴ molecules of H₂O

- 8.75×10³² molecules of C₆H₁₂O₆

1 mol  has 6.02×10²³ moles, so the rule of three will be:

NA of molecules are contained in 1 mol

- 2.46×10²¹ molecules of CO₂ are contained in (2.46×10²¹/ NA) =

- 1×10⁴ molecules of H₂O are contained in (1×10⁴ / NA) =

- 8.75×10³² molecules of C₆H₁₂O₆ are contained in (8.75×10³² / NA) =

-  4.08×10⁻³ moles of CO₂

-  1.66×10⁻²⁰ moles of H₂O

-  1453.5 moles of C₆H₁₂O₆

The number of moles in each compound is:

• 2.46 x 10²¹ molecules CO₂ = 0.00408 mol CO₂
• 10,000 molecules H₂O = 1.66 × 10⁻²⁰ mol H₂O
• 8.75 x 10³² molecules C₆H₁₂O₆ = 1.45 × 10⁹ mol C₆H₁₂O₆

It is the number of atoms or molecules in one mole of a substance, equal to 6.023 × 10²³.

We want to convert molecules to moles, so Avogadro's number will be the conversion factor.

• 2.46 x 10²¹ molecules CO₂ × 1 mol CO₂/6.023 × 10²³ molecules = 0.00408 mol CO₂

• 10,000 molecules H₂O × 1 mol H₂O/6.023 × 10²³ molecules = 1.66 × 10⁻²⁰ mol H₂O

• 8.75 x 10³² molecules C₆H₁₂O₆ × 1 mol C₆H₁₂O₆/6.023 × 10²³ molecules = 1.45 × 10⁹ mol C₆H₁₂O₆

The number of moles in each compound is:

• 2.46 x 10²¹ molecules CO₂ = 0.00408 mol CO₂
• 10,000 molecules H₂O = 1.66 × 10⁻²⁰ mol H₂O
• 8.75 x 10³² molecules C₆H₁₂O₆ = 1.45 × 10⁹ mol C₆H₁₂O₆