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 Any of various laws that describe the ways in which volume, temperature, pressure, and other conditions correlate when matter is in a gaseous state. At a constant temperature, the pressure of a particular amount of gas is inversely proportional with its volume (Boyle's Law) In a closed system with constant pressure, the volume of an ideal gas is in direct relation with its temperature (Charles's Law) At a constant volume, the pressure of a gas is in direct relation to its temperature (Gay-Lussac's Law) If the volume of all gases are equal and under the a similar temperature and pressure, then they contain an equal number of molecules (Avogadro's Law) The state of a particular amount of gas can be determined by its pressure, volume and temperature (Ideal Gas law)
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