Ideal gas equation
A tank in a room at 19 ˚C is initially open to the atmosphere on a day when the barometric pressure is 102 kPa. A block of dry ice (solid CO2) with a mass of 15.7 kg is dropped into the tank, which is then sealed. The reading on the tank pressure gauge initially rises very quickly, then much more slowly, eventually reaching a value of 3.27 MPa. Assume =19 ˚C.
a) How many moles of air were in the tank initially? Neglect the volume occupied by CO2 in the solid state, and assume that a negligible amount of CO2 escapes prior to the sealing of the tank.
b) What is the final density (g/liter) of the gas in the tank?
c) Explain the observed variation of pressure with time. More specifically, what is happening in the tank during the initial rapid pressure increase and during the later slow pressure increase?
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A tank in a room at 19 degree C is initially open to the atmosphere on...
A tank in a room at 19 degree C is initially open to the atmosphere on a day when the barometric pressure is 102 kPa. A block of dry ice (solid CO_2) with a mass of 15.7 kg is dropped into the tank, which is then sealed. The reading on the tank pressure gauge initially rises very quickly, then much more slowly, eventually reaching a value of 3.27 MPa. Assume T_final = 19 degree C. How many moles of air...
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A tank in a room at 19 degree C is initially open to the atmosphere on a day when the barometric pressure is 102 kPa. A block of dry ice (solid CO_2) with a mass of 15.7 kg is dropped into the tank, which is then sealed. The reading on the tank pressure gauge initially rises very quickly, then much more slowly, eventually reaching a value of 3.27 MPa. Assume T_final = 19 degree C. How many moles of air...
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and we continue to increase the amount of CO2 at the rate of about
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