A 21-L tank of carbon dioxide (CO2) is at a pressure of 8 atm and temperature of 19◦C. Calculate the number of moles of gas in the tank. 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. A fire breaks out, raising the ambient temperature to 69.1◦C while 82.3 g of gas leak out of the tank. Calculate the final pressure in the tank as a result of the fire and leakage. Hint: Use R =0.0821 liter-atm/mole-K for the gas constant in the ideal gas law. This allows you to use liters for volume and atmospheres for pressure
20-1 A 21-L tank of carbon dioxide (CO2) is at a pressure of 8 atm and temperature of 19◦C.
Calculate the number of moles of gas in the tank.
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.
A fire breaks out, raising the ambient temperature to 69.1◦C while 82.3 g of gas leak out of the
tank. Calculate the final pressure in the tank as a result of the fire and leakage.
Hint: Use R =0.0821 liter-atm/mole-K for the gas constant in the
use liters for volume and atmospheres for pressure
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