A gas has a pressure of 2.82 atm and occupies a volume of 7 L. If the gas is compressed to a volume of 2.74 L, what will its pressure be, assuming constant temperature?

7.20 atm

Explanation:

Since the gas remains at constant temperature, we can solve this problem by using Boyle's Law, which states that:

"For a constant mass of an ideal gas kept at constant temperature, the pressure of the gas is inversely proportional to its volume"

Mathematically:

where

p is the pressure of the gas

V is the volume

The equation can be also rewritten as:

where in this problem, we have:

is the initial pressure of the gas

is the initial volume of the gas

is the final volume of the gas

Solving for p2, we find the final pressure:

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.