Help With Dalton's Law of Partial Pressure!!?

Question

For a mixture of two gases, consisting of 1.50 mol of CF4 and 3.00 mol of H2, at a total pressure of 3.66 atm, what is the partial pressure of CF4?

Answer 1

One form of Dalton's Law is:

Partial Pressure = Total pressure x mole fraction

mole fraction = moles of gas/total moles of all gases

Add together the moles to get the total moles (1.50 + 3.00 = 4.50)

Make the mole fraction for CF4 by dividing its number of moles by the total moles.

1.50 divided by 4.50 = 1/3

Multiply this mole fraction times the total pressure to get the partial pressure:

3.66 x 1/3 = 1.20 atm.

Answer 2

1/3 of the mixture is CF4, so at 1 atmosphere, the partial pressure of CF4 is 1/3 atmosphere. At 3.66 atmospheres, the partial pressure of CF4 is 3.66/3 or 1.22 atmospheres.

Answer 3

cf4 would calculate to 16.47

we learned about it in my science class an thats what our teacher told us the answer was .