The ideal gas law relates temperature T, pressure P, and volume V of an ideal gas: PV=8.314T. Note that in the equation, we assume there is 1 mole of gas so that the units of the constant 8.314 are Joules per degree Kelvin. 1) Write an equation relating the rates of change of temperature, pressure, and volume with respect to time. 2) If an ideal gas is held at a constant volume 3.8 cubic meters and is being heated at a rate of 10 degrees K per minute, how quickly is the pressure increasing? Include units in your answer. Note that the constant has units as described above and that 1 Joule per cubic meter is equvalent to 1 Pascal (units of pressure).
The ideal gas law relates temperature T, pressure P, and volume V of an ideal gas: PV=8.314T. Note that in the equation, we assume there is 1 mole of gas so that the units of the constant 8.314 are Joules per degree Kelvin. 1) Write an equation relating the rates of change of temperature, pressure, and volume with respect to time. 2) If an ideal gas is held at a constant volume 3.8 cubic meters and is being heated at a rate of 10 degrees K per minute, how quickly is the pressure increasing? Include units in your answer. Note that the constant has units as described above and that 1 Joule per cubic meter is equvalent to 1 Pascal (units of pressure).
Chapter3: Polynomial Functions
Section3.5: Mathematical Modeling And Variation
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The ideal gas law relates temperature T, pressure P, and volume V of an ideal gas: PV=8.314T. Note that in the equation, we assume there is 1 mole of gas so that the units of the constant 8.314 are Joules per degree Kelvin.
1) Write an equation relating the rates of change of temperature, pressure, and volume with respect to time.
2) If an ideal gas is held at a constant volume 3.8 cubic meters and is being heated at a rate of 10 degrees K per minute, how quickly is the pressure increasing? Include units in your answer. Note that the constant has units as described above and that 1 Joule per cubic meter is equvalent to 1 Pascal (units of pressure).
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