A container holds 500 mL of oxygen gas at a pressure of 1.3 atm and a temperature of 25 ˚C. If the temperature increases to 29 ˚C and the pressure increases to 2.0 atm, will the volume of the gas increase or decrease? What is the final volume of the gas in liters (L)?

The new volume of the gas is decreased, to 0.329 L

Explanation:

Step 1: Data given

Volume of oxygen = 500 mL = 0.500 L

Pressure = 1.3 atm

Temperature = 25.0 °C

Temperature increases to 29.0 °C

New pressure = 2.0 atm

Step 2: Calculate new volume

p1*V1/T1 = p2*V2/T2

⇒with p1 = the initial pressure = 1.3 atm

⇒with V1 = the initial volume = 0.500L

⇒with T1 = the initial temperature = 25 °C = 298 K

⇒with p2 = the new pressure = 2.0 atm

⇒with V2 = the new volume = TO BE DETERMINED

⇒with T2 = the new temperature = 29 °C = 302 K

(1.3 * 0.500)/298 = (2.0 * V2) /302

0.0021812 = 2.0V2 / 302

V2 = 0.329 L = 329 mL

The new volume of the gas is decreased, to 0.329 L

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.