Using PV=nRT, 10.0ºC = 283.15ºK, R = 62.36 L torr/mol K
V= (nRT)/P
V = (2.35m*(62.36 L torr/mol K)*283.15ºK)/766.7 Torr
V = 54.12 L
The frequency of collisions is reduced
number of molecules
In a sample of air, an increase in temperature will result in an increase in the partial pressure of oxygen.
If a fixed sample of gas has a change of temperature pressure would increase.
liquid
contains the same number of molecules
The frequency of collisions is reduced
number of molecules
In a sample of air, an increase in temperature will result in an increase in the partial pressure of oxygen.
If a fixed sample of gas has a change of temperature pressure would increase.
cos2(s)
liquid
temperature
More pressure means less volume. Calculate the ratio of pressure, then divide the 4.2 liters by that ratio.This assumes: * That the temperature doesn't change. * That the gas behaves like an ideal gas.
The pressure is 103,5 at.
The temperature of the water is 100 degrees celsius.
For the pressure to remain the same, the temperature would double if the volume also doubled.