Knowee
Questions
Features
Study Tools

For a 5% solution of urea (Molar mass = 60 g/mol), calculate the osmotic pressure at 300 K.[R = 0·0821 L atm K–1 mol–1

Question

For a 5% solution of urea (Molar mass = 60 g/mol), calculate the osmotic pressure at 300 K.[R = 0·0821 L atm K–1 mol–1
🧐 Not the exact question you are looking for?Go ask a question

Solution 1

Sure, here's how you can calculate the osmotic pressure for a 5% solution of urea at 300 K:

Step 1: Calculate the molarity of the solution. The 5% solution means that there are 5 g of urea in 100 g of solution. Since the density of water is approximately 1 g/mL, we can assume that 100 g of solution Knowee AI is a powerful AI-powered study tool designed to help you to solve study problem.

Knowee AI  is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI  is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI  is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI  is a powerful AI-powered study tool designed to help you to solve study problem.
Knowee AI

This problem has been solved

Similar Questions

Osmotic pressure of a solution is 0.0821 atm at a temperature of 300 K. The concentration in moles/lit will be   ____________________*0.330.6660.00333

At what temperature (in K) would 2.10 mol of N2 gas have a pressure of 1.25 atm in a 24.9 L tank? (R = 0.0821 L·atm/mol·K.

If equilibrium constant is 2 at 300 K then the standard free energy change at 300 K and 1 atm pressure is

At what temperature (in K) would 2.10 mol of N2 gas have a pressure of 1.25 atm in a 22.1 L tank? (R = 0.0821 L·atm/mol·K.

The osmotic pressure of 0.0400 mol L-1 NaNO3 at 25.0oC is:Question 8Select one:100 kPa350 kPa198 kPa99 kPa18.5 kPa

1/3

Upgrade your grade with Knowee

Get personalized homework help. Review tough concepts in more detail, or go deeper into your topic by exploring other relevant questions.