In the flask diagrammed below, the left bulb contains 3.0l of neon at a pressure of 2.0 atm. the right bulb contains 2.0l of argon at a pressure of 1.0 atm. what is the mole fraction of neon and argon in the final mixture after the valve is opened and a uniform pressure is reached at constant temperature (25 ? c)?

i've determined the final pressure to be 1.6atm using p1v1+p2v2 = pfvf, but i have no idea how to get the mole fractions.

Mole fraction of Neon  = 0.75 = 3/4

Mole fraction of Argon =  0.25 = 1/4

Explanation:

Step 1: Given data

Volume of the left bulb = 3.0 L of Neon

Pressure of the left bulb = 2.0 atm

Volume of the right bulb = 2.0 L of argon

Pressure of the right bulb = 1.0 atm

Temperature = 25°C

Step 2: Calculate nimber of moles

Via the ideal gas law P*V = n*R*T

n = P*V / R*T

nNeon = (2*3)/ (0/08206* 298)

nNeon : 6/ 24.45 = 0.245

nArgon = (1*2)/(0/08206*298)

nArgon = 2/24.45 = 0.0818

nTotal = nNeon + nArgon = 0.245 + 0.0818 = 0.3268

Step 3: Calculate mole fraction

Mole fraction of Neon = 0.245 / 0.3268 = 0.75 = 3/4

Mole fraction of Argon = 0.0818 / 0.3268 = 0.25 = 1/4

b

explanation:

mitosis

the earth would become to overheated and everything alive on it will eventually die from overheating. plants will eventually die as well, water will evaporate, and it will be nothing but a hot planet without anything living on it.