A sample of oxygen gas occupies 7.00 L at a pressure of 1.00 atm. What will the pressure of the gas be if the volume is 3.00 L and the temperature remains unchanged?
You could use the combined gas law formula (numbers= subscripts):
(P1)(V1)(T2)=(P2)(V2)(T1)
Just ignore the T's, and plug in the information given in the problem and let 'x' represent the missing information.
(1.00 atm)(7.00L)= (3.00L)(x)
Work it out like an algebra problem and you should get:
7/3 atm or 2.33 atm
you just mulyipy the pressure by the mass. PV=K
(7.00L)(3.00L)=21.0L2
Teacher's Note: Did you notice that the units do not work here?
Pressure is atm and not L2
You could use the combined gas law formula (numbers= subscripts):
(P1)(V1)(T2)=(P2)(V2)(T1)
Just ignore the T's, and plug in the information given in the problem and let 'x' represent the missing information.
(1.00 atm)(7.00L)= (3.00L)(x)
Work it out like an algebra problem and you should get:
7/3 atm or 2.33 atm
you just mulyipy the pressure by the mass. PV=K
(7.00L)(3.00L)=21.0L2
Teacher's Note: Did you notice that the units do not work here?
Pressure is atm and not L2
you just mulyipy the pressure by the mass. PV=K
(7.00L)(3.00L)=21.0L2
Teacher's Note: Did you notice that the units do not work here?
Pressure is atm and not L2
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