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A sample of N2O gas has a density of 2.697 g/L at 298 K. What must be the pressure of the gas (in mmHg)?

User Huiyan Wan
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1 Answer

5 votes

Answer:


P=1139.16384mmHg

Step-by-step explanation:

Given data


R=0.08206((L.Atm)/(mol.K) )\\Density=2.697g/L\\Temperature=298K\\f.wt=44(g/mol)\\

To find

Pressure

Solution

From Ideal gas law we know that


PV=nRT\\P=(nR(T)/(V) )=(R((mass)/(f.wt) )((T)/(V) ))\\P=R((mass)/(volume)) ((T)/(f.wt) )=R(Density)((T)/(f.wt) )

Substitute the given values to find pressure

So


P=(0.08206(L.Atm)/(mol.K) )(2.697g/L)(298K)(44g/mol)^(-1)\\ P=1.4989Atm\\

Convert Atm to mmHg

Multiply the pressure values by 760

So


P=1139.16384mmHg

User Borealis
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