Question

In theory, $1.00mol$ of water vapor in a $10.0L$ container at $400K$ should have a pressure of $3.28$ atm, according to the ideal gas law, However, the observed pressure is actually $3.24atm$.
Which of the following is the best justification for why the observed pressure is slightly less than the predicted value?

• A. Water molecules tend to travel at faster speeds than other gas molecules.
• B. Water molecules experiences intermolecular attractive forces with each other.
• C. Water molecules ten to bounce off each other with a large repulsive force.
• D. Water molecules experience adhesion with the walls of the container.

Answer 1

The correct option is B Water molecules experiences intermolecular attractive forces with each other.

Water molecules experiences intermolecular attractive forces with each but in ideal gas there is no attractive forces between two molecules of a gas.