A 0.0218-m3 tank of carbon dioxide (CO2) is at a pressure of 8.94x10^5 Pa and te

Question

A 0.0218-m3 tank of carbon dioxide (CO2) is at a pressure of 8.94x10^5 Pa and temperature of 19.4C. (A) Calculate the number of moles of gas in the tank. (B) Obtain the number of grams of carbon dioxide in the tank. Hint: You can obtain the molar mass of CO2 by adding the molar mass of C and twice the molar mass of O. The molar mass of an element is given on the periodic table in units of grams/mole. (C) A fire breaks out, raising the ambient temperature to 69.1C while 82.3 g of gas leak out of the tank. Calculate the final pressure (Pa) in the tank as a result of the fire and leakage. Answers between 7.00, 9.50 mol, 300, 400 g, 6.00 × 105 , 9.50 × 105 Pa

Explanation / Answer

a)

PV = nRT

So, (8.94*10^5)*(0.0218) = n*(8.314)*(273 + 19.4)

So, n = 8.02 moles <------- answer

b)

Molar mass of CO2 = 44.1 g/ml

So, mass of CO2 = 44.1*8.02 = 353.7 g

c)

PV = nRT

After 82.3 g of CO2 leak out, the mass remaining = 353.7 - 82.3 = 271.4 g

So, number of moles in 271.4 g CO2 = 271.4/44.1 = 6.15 moles

final temperature, T = 273 + 19.4 + 69.1 = 361.5 K

PV = nRT

So, P*(0.0213) = 6.15*8.314*361.5

So, P = 8.68*10^5 Pa <---------answer

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