The volume of an ideal gas is inversely proportional to the pressure applied to the gas at a constant temperature. A gas has a volume of

239 liters at a pressure of 2.00 atmospheres (atm). What pressure is

applied to this gas if the volume is .500 liters?

Final pressure is 0.956 atm

Explanation:

Based on Boyle's law, "The volume of an ideal gas is inversely proportional to the pressure when temperature is constant". The equation is:

P₁V₁ = P₂V₂

Where 1 represents initial state and 2 final state of the gas.

If a gas has 239L and 2.00 atm as initial state. If the final volume is 500L:

239Lₓ2.00atm =  P₂500L

239Lₓ2.00atm / 500L =  P₂

0.956atm =  P₂

the best answer is d because the strong cohesion is caused by the ability of water molecules to undergo hydrogen bonding.

a is incorrect because when water solidifies, it becomes   ice, which expands and occupies a bigger volume for the same mass of water in its liquid state.

b is incorrect because water has high surface tension. besides bonding to itself it hydrogen bonds to other molecules at the top decreasing possibility for breaking of attractive forces.

c is incorrect because the water molecule has oxygen which is highly electronegative and so pulls the electron pair towards itself creating a dipole moment, making the molecule polar.

e is incorrect because water has strong adhesion, ability to stick to other molecules such as glass because of this molecules having stronger hydrogen bonding than water.