Question

Calculate the number of moles of hydrogen contained in 18 litres of the gas at 27°C and 70 cm pressure. Given

that R = 0.0821 litre atm 1 K

 1 mol 

. Further, if the mass of hydrogen taken as above is found to be 1.350g,

calculate the molecular mass of hydrogen​

Answer 1

Explanation:

Here, we are given : V=18 litres,

=27+273 K=300K <br>

<br> Using the ideal gas equation, PV=nRT <br> we have

<br> Further, we know that

(Molar mass=mass

Answer 2

Answer:

here it is

Explanation:

Here, we are given : V=18 litres, T=27∘C=27+273 K=300K

P=70cm=70/76 atm,R=0.0821 litre atm K−1mol−1

Using the ideal gas equation, PV=nRT

we have  n=PVRT=(70/76 atm)(18L)(0.0821 L atm mol−1)(300 K)=0.67 mole

Further, we know that n=(Mass)/(Mo≤ca−−rmass)=(m)/(M):. M=(m)/(n)=(1.350)/(0.67)=2.015u(Molar mass=mass mol−1)