A 17.0-L tank of carbon dioxide gas (CO2) is at a pressure of 9.30 105 Pa and te

Question

A 17.0-L tank of carbon dioxide gas (CO2) is at a pressure of 9.30 105 Pa and temperature of 16.0°C.

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

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

(c) Use the periodic table to compute the molecular weight of carbon dioxide, expressing it in grams per mole.
3 g/mol

(d) Obtain the number of grams of carbon dioxide in the tank.
4 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.    

     (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

Explanation / Answer

here,

volume of the tank , V = 17 l

pressure , P = 9.3 * 10^5 Pa

P = 930 KPa

temprature , T = 16 degree C

(a)

temprature in kelvin = temprature in celcius + 273.16

T = 273.16 + 16

T = 289.16 K

(b)

let the number of moles be n

using ideal gas equation

P*V = n*R*T

930 *17 = n*8.314 * 289.16

n = 6.58 moles

(c)

the molecular weight of carbon diaoxide is 44.01 g/mol

(d)

the number of grams, m = n*44.01

m = 6.58 * 44.01

m = 289.4 g

the number of grams of carbon diaoxide in the tank is 289.4 g

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