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Assuming ideal behavior, how much pressure will 2.75 mol hydrogen gas exert on the walls of a 4.00 L container at 35.0ºC?
A. 17.4 atm B. 19.8 atm C. 278 atm D. 296 atm

Respuesta :

Willchemistry
R = 0.082 atm

T = 35.0 + 273 = 308 K

P x V = n x R x T

P x 4.00 = 2.75 x 0.082 x 308

P x 4.00 = 69.454

P = 69.454 / 4.00

P = 17.4 atm

Answer A

Answer:

The correct answer is option A.

Explanation:

Pressure of the gas = P =?

Volume of the container in which gas is placed, V= 4.00 L

Temperature of the gas = T = 35°C = 308.15 k

Moles of gas = N = 2.75 mol

Using ideal gas equation:

PV=nRT

[tex]P=\frac{nRT}{V}=\frac{2.75 mol\times 0.0821 atm L/mol K\times 308.15 K}{4 L}[/tex]

P = 17.3931 atm ≈ 17.4 atm

The pressure of the gas in the container is 17.4 atm.

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