A 2.0-L container containing neon at a pressure of 150 kPa is connected to a 4.0-L vessel containing argon at a pressure of 350 kPa. That valve between the two vessels is opened and the gases are allowed to mix until equilibrium is attained. Assuming that the temperature remains constant, calculate the total pressure of the mixture.

To calculate the total pressure of the mixture, we can use Dalton's Law of Partial Pressures, which states that the total pressure of a mixture of gases is equal to the sum of the partial pressures of each gas.First, we need to calculate the partial pressure of each gas in the final mixture.Initial number of moles of neon (Ne) = PV/RT = (150 kPa x 2.0 L) / RTInitial number of moles of argon (Ar) = PV/RT = (350 kPa x 4.0 L) / RTSince the temperature (T) and gas constant (R) are constant, we can combine the two equations:Total number of moles = (150 kPa x 2.0 L + 350 kPa x 4.0 L) / RTTotal volume = 2.0 L + 4.0 L = 6.0 LNow, we can calculate the total pressure (P_total) of the mixture:P_total = (Total number of moles x RT) / Total volume= ((150 kPa x 2.0 L + 350 kPa x 4.0 L) / RT) x RT / 6.0 L= (300 kPa + 1400 kPa) / 6.0 L x (6.0 L)= 233.33 kPaTherefore, the total pressure of the mixture is approximately 233.33 kPa.Please note that this calculation assumes ideal gas behavior and neglects any potential interactions between the gases.

Answered by eiyerice | 2024-10-26