14. A 21.0-L tank of carbon dioxide gas (CO2) is at a pressure of 9.20 105 Pa an

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. PLEASE SHOW ALL FORMULAS AND COMPUTATIONS ON HOW YOU GET YOUR FIGURES. THANKS

Explanation / Answer

v=21 L =21*10^-3 m^3

P=9.2*10^5 Pa

T=20 oC

a)

temperature, T=20+273=293 K

b)

P*V=n*R*T

9.2*10^5*21*10^-3=n*8.314*293

===> no of mole, n=7.93 or 8

c)

molecular weight of CO2 is, M =12g+2*16g=44 g/mol

d)

mass of CO2 is, m=M*n

=44*7.93

=348.92 g

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