(a) Interpretation: The mass percentage of N 2 O gas should be calculated. Concept introduction: According to the Dalton’s law of partial pressure the partial pressure of any gas in the gaseous mixture is the product of mole fraction of that gas and total pressure. The mathematical expression can be written as: Partial Pressure = Mole fraction of gas × Total Pressure For a gaseous mixture, the average molar mass or apparent molar mass can be calculated as the sum of the mole fractions of each component gas multiplied by their molar mass. The mathematical expression can be written as: M mixture = ( x 1 × M 1 + ...... + x n × M n ) Here: x i = Mole fractions of component gas M i = the molar mass of component gas
(a) Interpretation: The mass percentage of N 2 O gas should be calculated. Concept introduction: According to the Dalton’s law of partial pressure the partial pressure of any gas in the gaseous mixture is the product of mole fraction of that gas and total pressure. The mathematical expression can be written as: Partial Pressure = Mole fraction of gas × Total Pressure For a gaseous mixture, the average molar mass or apparent molar mass can be calculated as the sum of the mole fractions of each component gas multiplied by their molar mass. The mathematical expression can be written as: M mixture = ( x 1 × M 1 + ...... + x n × M n ) Here: x i = Mole fractions of component gas M i = the molar mass of component gas
Solution Summary: The author explains the Dalton's law of partial pressure. The mass percentage of N 2 O in the given mixture is 84.5 %.
The mass percentage of N2O gas should be calculated.
Concept introduction:
According to the Dalton’s law of partial pressure the partial pressure of any gas in the gaseous mixture is the product of mole fraction of that gas and total pressure. The mathematical expression can be written as:
Partial Pressure = Mole fraction of gas × Total Pressure
For a gaseous mixture, the average molar mass or apparent molar mass can be calculated as the sum of the mole fractions of each component gas multiplied by their molar mass. The mathematical expression can be written as:
Mmixture= (x1×M1+ ......+ xn×Mn)
Here:
xi= Mole fractions of component gas
Mi = the molar mass of component gas
Interpretation Introduction
(b)
Interpretation:
The apparent molar mass of anesthetic should be calculated.
Concept introduction:
According to the Dalton’s law of partial pressure the partial pressure of any gas in the gaseous mixture is the product of mole fraction of that gas and total pressure. The mathematical expression can be written as:
Partial Pressure = Mole fraction of gas × Total Pressure
For a gaseous mixture, the average molar mass or apparent molar mass can be calculated as the sum of the mole fractions of each component gas multiplied by their molar mass. The mathematical expression can be written as:
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