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Calculate the pressure, in atmospheres, exerted by each of the following:

a) 2.50 L HF containing 1.35 mol at 320.0 G
b) 4.75 L NO2 containing 0.86 mol at 300.0 K
c) 5.50 × 104 mL CO2 containing 2.15 mol at 57°C

Respuesta :

Answer:

a) 14.2 atm

b) 4.46 atm

c) 1.06 atm

Explanation:

For an ideal gas,

PV = nRT

P = pressure of the gas

V = volume occupied by the gas

n = number of moles of the gas

R = molar gas constant = 0.08206 L.atm/mol.K

T = temperature of the gas in Kelvin

a) For HF,

P =?, V = 2.5L, n = 1.35 moles, T = 320K

P = 1.35 × 0.08206 × 320/2.5

P = 14.2 atm

b) For NO₂

P =?, V = 4.75L, n = 0.86 moles, T = 300K

P = 0.86 × 0.08206 × 300/4.75

P = 4.46 atm

c) For CO₂

P =?, V = 5.5 × 10⁴ mL = 55L, n = 2.15 moles, T = 57°C = 330K

P = 2.15 × 0.08206 × 330/55

P = 1.06 atm

a) The pressure should be 14.2 atm.

b)  The pressure should be 4.46 atm.

c)   The pressure should be 1.06 atm.

Calculation of the pressure in terms of the atmosphere:

For an ideal gas,

The following formula should be used.

PV = nRT

Here

P = pressure of the gas

V = volume occupied by the gas

n = number of moles of the gas

R = molar gas constant = 0.08206

T = temperature of the gas in Kelvin

Now

a) For HF,

P = 1.35 × 0.08206 × 320/2.5

P = 14.2 atm

b) For NO₂

P = 0.86 × 0.08206 × 300/4.75

P = 4.46 atm

c) For CO₂

P = 2.15 × 0.08206 × 330/55

P = 1.06 atm

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