Question

5 gram of a gas at 27 degree Celsius occupies the same volume is 0.25 gram of H2 at 17°C at same pressure find the volume molecular mass of gas​?
Also give the explanation

Answer 1

Answer: TO FIND Vm ( volume molecular mass of gas)​ :

2.00048

Explanation:     For gas ,                         For H2,

m1 = 5gm                                                  m2 = 0.25gm

T1 = 27 +273 = 300K                                T2 = 290K

v1 = v (say)                                                  v2 = v

p1 = p (say)                                                  p2 = p

P1V1 =n1 RT1                                                P2V2 = n2 RT2

Since pressure and volume are same so we can write,

n1 RT1 = n2RT2

n1 T1 = n2T2

(m1/ M1) * T1 = ( m2 / M2 ) * T2        [ n= m/ M]

putting all the above values

M1 = 41. 37 amu ( since any unit is not fixed)

Also , we know that;  Molecular mass = 2 * VD

                                   41.37 /2 = D

                                    D = 20.67

Hence ,  volume molecular mass of gas​ ( Vm) = molar mass / mass density

                                                                            = 41.37 / 20.67

                                                                            = 2.000048 ans.

Molar mass also termed as molecular mass for 1 mole.

Answer 2

Answer:

41.37

Explanation:

I am goanna try my best... (I have been stuck with this forever)

M1=5g

M2=0.25

T1=273+27=300K

T2= 273+17=290

n1=Mass/M.wt=5/M

n2=Mass/M.wt=0.25/2=0.125

for the gas-> P1V1=n1RT1->i

for H2-> P2v2=n2RT2->ii

PV will be same for both as mentioned

so when equation i divided by equation 2 u get

1=n1T1/n2T2

1=5/M*300/0.125*290

1=1500/M*36.25

M=1500/36.25=41.37

That's all I can do hope it helps