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
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
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 ideal gas law. This allows you to use liters for volume and atmospheres for pressure
Definition Definition Law that is the combined form of Boyle's Law, Charles's Law, and Avogadro's Law. This law is obeyed by all ideal gas. Boyle's Law states that pressure is inversely proportional to volume. Charles's Law states that volume is in direct relation to temperature. Avogadro's Law shows that volume is in direct relation to the number of moles in the gas. The mathematical equation for the ideal gas law equation has been formulated by taking all the equations into account: PV=nRT Where P = pressure of the ideal gas V = volume of the ideal gas n = amount of ideal gas measured in moles R = universal gas constant and its value is 8.314 J.K-1mol-1 T = temperature
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