Question

b) Calculate the mass of 500 ml of O2 at 27°c and 740 mm of Hg.​

Answer 1

Using n = PV÷RT

n=(740/760)0.5÷(0.0821×300)

n=0.02 approx Hence mass = moles × molecular mass Mass of O2=0.02×32

=0.64g

Answer 2

Answer:

The answer is

Explanation:

According to ideal gas law

PV=nRT

since1

n=m/M

so

PV=mRT/M. (1)

using this formula we can calculate the mass of given compound at stp

Keep this in mind when u are dealing with ideal gas eq: and its derivatives always take the temprature T in kelvins and pressure P in mmHg and volume in dm³

T in kelvin=T in C°+273

=27+273=300K

Pressure is already given in mmHg

Now applying formula

PV=mRT/M

here value of R is 62.4dm³ mmHg/mol/K

m=PVM/RT=740×0.5dm³×32/62.4×300

=

and in this way u will get ur answer