# When 50.0 liters of oxygen at 20.0 c is compressed to 5.00 liters, what must the new temperature be to maintain constant pressure According to the Charles' law of gases, the volume occupied by a gas and the temperature are directly proportional to each other, provided the pressure remains constant.

Thus, at constant pressure conditions,

V `alpha`  T

where, V and T represent the volume and temperature of gases. In other words,

`V/T...

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According to the Charles' law of gases, the volume occupied by a gas and the temperature are directly proportional to each other, provided the pressure remains constant.

Thus, at constant pressure conditions,

V `alpha`  T

where, V and T represent the volume and temperature of gases. In other words,

`V/T = constant`

or, `V_1/T_1 = V_2/T_2`

where the notations 1 and 2 represent older conditions (volume and temperature) and new conditions, respectively.

Here, V1 = 50.0 liters, T1 = 20.0 degrees Celsius and V2 = 5.0 liters

Thus, T2 = (V2/V1) T1 = (5/50) x 20 = 2.0 degrees Celsius.

Thus, at constant pressure, the temperature of the oxygen will have to be decreased to 2 degrees Celsius (from an initial temperature of 20 degrees Celsius) to be able to compress it from 50 liters to 5 liters.

Hope this helps.

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