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3 years ago

if I have 22.1 grams of CO2 gas at -188 degrees Celsius and 165 ml what is the pressure of the gas in kPa

Chemistry

1 answer:

Harman [31]3 years ago

6 0

Answer:

P = 2.145kPa

Explanation:

Mass = 22.1g

Molar mass of CO2 = 44g/mol

Vol = 165mL = 0.165L

T = -188°C = (-188 + 273.15)K = 85.15K

R = 8.314J/mol.K

From ideal gas equation,

PV = nRT

P = pressure of the ideal gas

V = volume the gas occupies

n = number of moles if the gas

R = ideal gas constant

T = temperature of the gas

n = number of moles

n = mass / molar mass

n = 22.1 / 44 = 0.50moles

PV = nRT

P = nRT/ V

P = (0.5 × 8.314 × 85.15) / 0.165

P = 2145.26Pa = 2.145kPa

Pressure of the gas is 2.145kPa

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Answer:

The temperature must be changed to 4 times of the initial temperature so as to keep the pressure and the volume the same.

Explanation:

Pressure in the container is P and volume is V.

Temperature of the helium gas molecules = $T_1$

Molecules helium gas = x

Moles of helium has = $n_1= \frac{x}{N_A}$

PV = nRT (Ideal gas equation)

$PV=n_1RT_1$ ...[1]

After removal of helium gas only a fourth of the gas molecules remains and pressure in the container and volume should remain same.

Molecules of helium left after removal = $\frac{x}{4}$

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3 years ago

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Answer:

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3 years ago

if I have 22.1 grams of CO2 gas at -188 degrees Celsius and 165 ml what is the pressure of the gas in kPa​

if I have 22.1 grams of CO2 gas at -188 degrees Celsius and 165 ml what is the pressure of the gas in kPa