14. A 21.0-L tank of carbon dioxide gas (CO 2 ) is at a pressure of 9.20 10 5 Pa

Question

14. A 21.0-L tank of carbon dioxide gas (CO2) is at a pressure of 9.20 105 Pa and temperature of 20.0°C.

(a) Calculate the temperature of the gas in Kelvin._______________ K

(b) Use the ideal gas law to calculate the number of moles of gas in the tank.___________ mol

© Use the periodic table to compute the molecular weight of carbon dioxide, expressing it in grams per mole. _________________g/mol

(d) Obtain the number of grams of carbon dioxide in the tank. _______________ g

(e) A fire breaks out, raising the ambient temperature by 224.0 K while 82.0 g of gas leak out of the tank. Calculate the new temperature and the number of moles of gas remaining in the tank.

Temperature: ________________ K

Number of moles ________________ mol

(f) Using the ideal gas law, find a symbolic expression for the final pressure, neglecting the change in volume of the tank. (Use the following as necessary: ni, the initial number of moles; nf, the final number of moles; Ti, the initial temperature; Tf, the final temperature; and Pi, the initial pressure.)

Pf

=

(g) Calculate the final pressure in the tank as a result of the fire and leakage.
8 Pa

PLEASE SHOW ALL FORMULAS AND CALCULATIONS USED. THANKS

Pf

=

Explanation / Answer

(a)

T = 20.0+ 273.15 = 293.15K

(b)

pV = nRT
9.20 x 105 Pa * 21L = n * 8.314J/K·mol * 293.15K * 1000L / 1m³
n = 7.927 mol

(c)

c = 12g

o = 16 g

molwt = 12g + 2*16g = 44 g/mol

(d)

mass m = moles * molwt = 7.927mol * 44g/mol

m = 348.78 g

(e)

new T = 293.15K + 224.0K = 517.15K
new mass m' = 348.78 g - 82g = 266.78 g
new n = 266.78g / 44g/mol

new n = 6.063 mol

(f)

Pi / (ni*Ti) = Pf / (nf*Tf)

so
Pf = (Pi*nf*Tf) / (ni*Ti)

(g)

Pf = 9.20 x 105Pa * 6.063mol * 517.15 / (7.927mol * 293.15K)
Pf = 1.332 x 106 Pa

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