Question

(1) Consider the following sample of gases: = He Z (iii) If the three samples are all at the same temperature, rank them with respect to (a) total pressure; (b) partial pressure of helium; (c) density; (d) average kinetic energy of particles. (II) The temperature of a gas is raised from 10 °C to 20 °C. Will the volume double if mass and pressure do not change? Why or why not? (Show your calculations) (III) If 3.25 L of gas at 16.0°C and 1.00 atm is compressed at a pressure of 125 atm at 20.0 °C, calculate the new volume of the gas. (IV) Calculate its volume (in liters) of 88.4 g of CO2 at STP. (V) H20 and CHA are gases at 150 °C. Which exhibits more ideal behavior? Why? (VI) Assume that you have a cylinder with a movable piston. What would happen to the gas pressure inside the cylinder if you were to do the following? (a) Triple the Kelvin temperature while holding the volume constant (b) Reduce the amount of gas by 1/3 while holding the temperature and volume constant (c) Decrease the volume by 45% at constant T (d) Halve the Kelvin temperature, and triple the volume

Answer 1

Hello, i am sorry to say that as per HOMEWORKLIB RULES experts can answer either only one full question that too first question or first 4 sub-parts like a), b), c) & d) only. I request you to please post remaining question as separate one since my allotted time could not permit me to answer more than one question also. Thank you in advance for your continued support to us.

I am gonna answer 1st question in full.

PV = nRT

(a) total pressure: iii > i > ii

Although i & iii have same number of moles, but N₂ is diatomic and bigger molecule, so higher pressure

Remember if volume and temperature of a gas are constant, then P ∝ mN (∝ means "proportional to") m = mass of gas

(b) partial pressure of helium: i > ii > iii

partial pressure increases with increase in number of molecules of gas

(c) density: iii > i > ii

density = mass / volume, mass means more number of molecules

(d) average kinetic energy of particles: i = ii = iii

The average K.E ∝ absolute temperature of the gas. This means all gases at the same temperature have the same average kinetic energy.

Hope this helped you!

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