Question

John places a certain number n₁ of moles of Helium (He) in a vessel, and the gas has
pressure 30 torr at 0° C. If he had placed a number n₂ of moles of neon (Ne) in the
same vessel at 0° C, the gas would have pressure 70 torr. If he had placed a number
n₃ of moles of argon (Ar) in the same vessel at 0° C, the gas would have pressure 20
torr. According to the ideal gas laws, what would be the total pressure if n₁ moles of
helium, n₂ moles of neon, and n₃ moles of argon were placed into the same vessel at
0 °C?

Answer 1

From the knowledge of ideal gas laws ,here the Dalton's law states that total pressure exerted by non-reacting gases is equal to partial pressures of the individual gases.

So,total pressure in above question = (30+70+20) torr = 120 torr.