At 46°C a sample of ammonia gas exerts a pressure of 5.3 atm. What is the pressure when the volume of the gas?
At 46°C a sample of ammonia gas exerts a pressure of 5.3 atm. What is the pressure when the volume of the gas is reduced to one-eighth (0.125) of the original value at the same temperature?
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The pressure will be 8 times what it was. At a constant temperature, P1 x V1 = P2 x V2
pv=nRT or for a given temp. seeing as n and R are constants for the pattern. pv=consistent, 0.5 v double p, so the tension would be 10.6atm. n=moles, R is molar gas consistent( R = 8.31 J · ok-a million · mol-a million ), T is temp, p is press v is quantity,