1. Use the five flasks above to answer the questions that follow (description)

Question

a. which flask do the molecules have the greatest average speed of the particles. Explain your answer.

b. which nitrogen flask has the most number of particles? explain your reasoning

c. which oxygen flask has the most number of particles? explain your reasoning

d. if flask C were placed into flask E and there was no change in temperature, what would be the total pressure? explain your reasoning

e. which flasks have the same amount of kinetic energy? explain your reasoning

Flask A= N2 T=30 C P=1 atm

Flask B= N2 T= 50 C P= 0.5 atm

Flask C= O2 T=40 C P= 2 atm

Flask D= O2 T= 50 C P= 1 atm

Flask E= O2 T= 40 C P=0.5 atm

link to photo

https://dochub.com/23oswaldelliana/jo3xELpR3Q8p6JNVJBa7nr/img-9379-jpg

Answer 1

a. The greatest average speed will be based upon the equation, v_avg = √((8RT) / (πM)). Since the speed (velocity) only depends on the molar mass (M) and temperature (T), the flask containing the lowest molar mass gas with the highest temperature will have the greatest speed. The lowest mass is N₂, the highest temperature is 50°C, so flask B will have the greatest speed.

b. For the number of particles, we want to think about the ideal gas law, PV = nRT. according to this relation, moles and temperature are inversely proportional while moles and pressure and directly proportional. So we want a lower temperature and higher pressure (or more specifically we want a greater pressure caused by more gas particles, not a higher temperature). This would mean flask A, which is at a lower temperature and higher pressure, has the greatest number of N₂ particles.

c. Same reasoning for part b can be applied to part c. Flask C has the greatest number of O₂ particles because it has a higher pressure, and that pressure is not caused by a higher temperature (evidenced by having a lower temperature).

d. According to Dalton's Law, P_tot = P₁ + P₂ + P₃ + ..., the total pressure is equal to the sum of the partial pressures. Additionally, nothing is different between the two flasks, therefore, we can sum the pressures of each gas to give the total pressure within the flask: P_{flask E} = 0.5 atm + 2 atm = 2.5 atm

e. According to the kinetic molecular theory of an ideal gas, the kinetic energy of an ideal gas depends only on the temperature of that gas. Therefore, all gases that have the same temperature have the same kinetic energy. ∴ Flasks B and D have the same kinetic energy. Flasks C and E have the same kinetic energy.