Two identical cylinders contain helium at $2.5 a t m$ and argon at $1 a t m$ respectively. If both the gases are filled in one of the cylinders, the pressure would be

3.5 a t m

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1.75 a t m

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1.50 a t m

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1 a t m

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Solution

The correct option is A $3.5 a t m$
Dalton's law (also
called Dalton's law of partial pressures) states that the total
pressure exerted by the mixture of non-reactive gases is equal to the sum of the partial pressures of individual gases.
$P_{total} = P_{1} + P_{2}$

$= 1 + 2.5$

$= 3.5 atm$

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Two identical cylinders contain helium at 2.5 atm and argon at 1 atm respectively. If both the gases are filled in one of the cylinders, the pressure would be

The correct option is A 3.5 atmDalton's law (also called Dalton's law of partial pressures) states that the total pressure exerted by the mixture of non-reactive gases is equal to the sum of the partial pressures of individual gases. Ptotal=P1+P2 =1+2.5 =3.5 atm

Two identical cylinders contain helium at $2.5 a t m$ and argon at $1 a t m$ respectively. If both the gases are filled in one of the cylinders, the pressure would be

The correct option is A $3.5 a t m$
Dalton's law (also
called Dalton's law of partial pressures) states that the total
pressure exerted by the mixture of non-reactive gases is equal to the sum of the partial pressures of individual gases.
$P_{total} = P_{1} + P_{2}$

$= 1 + 2.5$

$= 3.5 atm$