Wikipedia
Mole fraction - In chemistry, mole fraction x (also, and more correctly, known as the amount fraction) is a way of expressing the composition of a mixture. The mole fraction of each component i is defined as its amount of substance n i divided by the total amount of substance in the system, ..
TutorVista
how to calculate mole fraction?
how to calculate mole fraction..
how to calculate mole fractions
how to calculate mole fractions..
how to calculate the mole fraction
how to calculate the mole fraction..
how to find mole fractions
how to find mole fractions..
MOLES. Maria Powell's F Period Chemistry. JMMMMARIAPOWELLIUM. WHAT YOU KNOW ABOUT MOLES What you know about moles What you know about moles What you know about moles Aye don't you know I got 6.02 times 10 to the 23rd yee it's Avogadro's numbah-- born 16th century. What you know about moles what you know about moles what you know about moles I know all about moles! I got my wife-beater Moles over liters It's called Molarity Don't you hate on me What you know about moles What you know about moles What you know about moles I know all about moles! A mole of melon seeds How large would the melon be? Times ten to the 23 Larger than the moon you see. If a mole of pennies Was given to everybodys How much could they spend on flowers A million dollars every hours Mole of gas in a vacuum What is the volume? 22.4 Liters Still got my wife beaters What you know about moles What you know about moles What you know about moles I know all about moles!
Jacobs Energy Blows Off Natural Gas Well after Nitrogen Frac Jacobs Energy contractor blows off a natural gas well in Kentucky after a hydraulic nitrogen frac
Question : The total pressure of 1 L of vapor over liquid acetic acid at 71.3oC is 146 mmHg. If the density of the vapor is 0.628 g/L, what is the mole fraction of dimer in the vapor?
Answer : Density for an ideal gas can be derived from the ideal gas law. Density = Pm/RT I don't know which version of R you use, so I will use the most common. R = 0.082 057 Latm/molK and P = pressure, atm m = average molecular weight, g/mol T = absolute temperature, K We can rearrange the equation to solve for m. m = densityxRxT/P 0.628 g/L x 0.082 057 Latm/molK x (71.3+273.17)K --------------------------------------------------------------------------- = m 146mmHg / 760 mmHg/atm m = 92.4 g/mol This is the average molecular weight of the vapor phase. The MW of acetic acid = 60.05. The MW of the dimer = 120.1. The average can be found from: m = 60.05 X1 + 120.1 X2 = 92.4 Where X1 = mole fraction of monomer X2 = mole fraction of dimer It is also true that X1 + X2 = 1. We can multiply this equation by -60.05 and get -60.05 X1 - 60.05 X2 = -60.05 Adding that equation to the first yields: 0 X1 + 60.05 X2 = 32.35 X2 = 32.35/60.05 = 0.53..
Answer : Density for an ideal gas can be derived from the ideal gas law. Density = Pm/RT I don't know which version of R you use, so I will use the most common. R = 0.082 057 Latm/molK and P = pressure, atm m = average molecular weight, g/mol T = absolute temperature, K We can rearrange the equation to solve for m. m = densityxRxT/P 0.628 g/L x 0.082 057 Latm/molK x (71.3+273.17)K --------------------------------------------------------------------------- = m 146mmHg / 760 mmHg/atm m = 92.4 g/mol This is the average molecular weight of the vapor phase. The MW of acetic acid = 60.05. The MW of the dimer = 120.1. The average can be found from: m = 60.05 X1 + 120.1 X2 = 92.4 Where X1 = mole fraction of monomer X2 = mole fraction of dimer It is also true that X1 + X2 = 1. We can multiply this equation by -60.05 and get -60.05 X1 - 60.05 X2 = -60.05 Adding that equation to the first yields: 0 X1 + 60.05 X2 = 32.35 X2 = 32.35/60.05 = 0.53..
Question : There is a mixture of x and b and it is know that the mole% of a is 5. What is the mole fraction of a (Xa) and the mole fraction of b (Xb)?
I know that the sum of mole fractions in a mixture should equal 1, so
Xa + Xb = 1
I know that in terms of a the mole&% is defined as
mol%a = [mol a/(mol a + mol b)]*100
so,
5 = [mol a/(mol a + mol b)]*100
0.05 = [mol a/(mol a + mol b)]
So how can I solve this equation to find the mol a and (mol a + mol b)?
sorry, I meant 'th..
Answer : mole percentages add up to 100. So the mix is... 5% of a and 95% of b. mole fractions add up to 1. So... mole fraction of a is 0.05 and mole fraction of b is 0.95 i.e. mole fractions are one-hundredth of mole percentages. OK?
Answer : mole percentages add up to 100. So the mix is... 5% of a and 95% of b. mole fractions add up to 1. So... mole fraction of a is 0.05 and mole fraction of b is 0.95 i.e. mole fractions are one-hundredth of mole percentages. OK?
