A gaseous mixture contains 401.0 Torr H2(g), 367.7 Torr N2(g), and 89.9 Torr Ar(g). Calculate the mole fraction, ?, of

A certain gas is present in a 13.0 LL cylinder at 3.0 atmatm pressure. If the pressure is increased to 6.0 atmatm the volume of the gas decreases to 6.5 LL . Find the two constants kiki, the initial value of kk, and kfkf, the final value of kk, to verify whether the gas obeys Boyle’s law by entering the numerical values for kiki and kfkf in the space provided.

Please don't provide handwrittin solution...

A gas mixture containing only O2 and N2. If the mole fraction of O2 is 0.37, and the total pressure is 2.4 atm, what is the partial pressure of N2?

A gaseous mixture contains 404.0 Torr H2(g),404.0 Torr H2(g), 356.7 Torr N2(g),356.7 Torr N2(g), and 75.9 Torr Ar(g).75.9 Torr Ar(g). Calculate the mole fraction, ?, of each of these gases.   ?H2=     ?N2=   ?Ar=

How many moles of a gas mixture would be needed to provide 0.555 mole O2, if the mole fraction of O2 in the mixture is 0.430 ?

What is the mole fraction of O2 in a mixture of 6.00 g He, 19.0 g O2, and 21.0 g N2?     0.608     0.253     0.410     0.209     0.267

a mixture of gases contains 86.6 g of C2H4 and 52.1 g of N2. what is the mole fraction for N2 in such a mixture?

A gaseous mixture consists of 1.26 mol of helium, 0.36 mol of neon, and 1.58 mol of argon. What is the mole fraction of helium in the mixture?

The mole fraction of hydrogen gas in a mixture of gases is 0.17. The total pressure of the gas mixture is 2.8 atm. What is the partial pressure of the hydrogen gas?