at 127 centigrade and 1 atm pressure of a gas contains 0.3mole of nitrogen molecule, 0.2 mole of oxygen molecule.the volume of the mixture is
What is the total pressure of the gas produced in the burette if it contains
nitrogen gas whose pressure is 1.5 atm, oxygen gas whose pressure is 1.6 atm
and water vapour with a pressure of 1.3 atm.
To find the volume of the gas mixture, we can use the ideal gas law equation: PV = nRT. In this equation, P represents the pressure, V represents the volume, n represents the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
First, we need to convert the temperature from degrees Celsius to Kelvin. The conversion formula is: Kelvin = Celsius + 273.15.
Given:
Temperature (T) = 127 °C = 127 + 273.15 = 400.15 K
Pressure (P) = 1 atm
Number of moles of nitrogen (n1) = 0.3 mol
Number of moles of oxygen (n2) = 0.2 mol
To find the total number of moles (n) of the gas mixture, we add the number of moles of nitrogen and oxygen:
n = n1 + n2 = 0.3 mol + 0.2 mol = 0.5 mol
Now, we can plug in the values into the ideal gas law equation:
PV = nRT
V = (nRT) / P
Substituting the values:
V = (0.5 mol * 0.0821 L·atm/mol·K * 400.15 K) / 1 atm
V ≈ 16.51 L
Therefore, the volume of the gas mixture at 127 °C and 1 atm pressure is approximately 16.51 liters.