What will be the minimum pressure required to compress 500 dm3 o
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What will be the minimum pressure required to compress 500 dm3 of air at 1 bar to 200 dm3 at 30C?


From the given data,



According to Boyle's law,

                   


Substituting the values, we have,

   

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What would be the SI unit for the quantity fraction numerator PV squared straight T squared over denominator straight n end fraction ?


The unit of pressure is given as= Nm-2
The unit of volume is given as= m3
The unit of Temperature is given as= K2
Unit of mol is givne as = mol-1.
Thus SI unit of given quantity is given as,

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In terms of Charles’s law explain why –273°C is the lowest possible temperature.


The law states that at constant pressure, the volume of a fixed mass of gas is directly proportional to its absolute temperature. It was found that for all gases (at any given pressure), the plots of volume vs. temperature is a straight line. If this line is extended to zero volume, then it intersects the temperature axis at -2730C.



In other words, the volume of any gas at 273 0C is zero. This is because all gases get liquefied before reaching a temperature of 2730C.

Hence, it can be concluded that -273 0C is the lowest possible temperature

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Explain the physical significance of van der Waals parameters.


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Critical temperature for carbon dioxide (CO2) and methane (CH4) are 31·1°C and –81 ·9°C respectively. Which of these has stronger intermolecular forces and why?

We know that higher the critical temperature, more easily the gas can be liquefied i.e. greater are intermolecular forces of attraction. This means that the intermolecular forces of attraction between the molecules of a gas are directly proportional to its critical temperature. Since CO2 has greater critical temperature than CH4, therefore CO2 has stronger intermolecular forces than CH4.

 

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