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If a 20 Liter helium gas cylinder is pressurized to 70.8 ATM at a temperature of 34.1 Celsius what is the temp in degrees Celsius if the pressure is 67.5 ATM?
Wiki User
∙ 14y ago
Assuming helium behaves sufficiently as an ideal gas at these pressures then the following equation can be applied :- pV = RT ( where p is pressure,V is volume,T is absolute temperature and R the universal gas constant ) The required temperature Tx is found as follows :- 67.5 * V = R * (273 + Tx) 70.8 * V = R * (273 + 34.1) Note that we don't need to know the volume except that it be the same at both pressures, nor the value of the gas constant for however many moles as both cancel when dividing the one equation by the other. Division also means we don't have to worry about the units of pressure so long as we are consistent. Thus dividing and cancelling 67.5/70.8 = (273 + Tx)/(273 + 34.1) or Tx = (273 + 34.1)*67.5/70.8 - 273 ie Tx = 19.8 Celsius
Wiki User
∙ 14y ago
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Which term is defined as the atmospheric pressure at sea level at zero degrees celsius?
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