Given the moleculer mass of two molecules ( __M1__ and __M2__ ), their masses present ( __m1__ and __m2__ ) in a vessel of volume ( __V__ ) at a specific temperature ( __T__ ). Find the total pressure exerted by the molecules ( __Ptotal__ ) .
input
====
Six values : 
- __m1__
- __m2__
- __M1__
- __M2__
- __V__
- __T__
output
==== 
One value : 
- __Ptotal__ 
notes
====
Units for each of the following are given as under : 
- _m1_ = gram 
- _m2_ = gram
- _M1_ = _gram.mole^(-1)_
- _M2_ = _gram.mole^(-1)_
- _V_             = _dm^(3)_
- _T_             = Celsius
- __Ptotal__ = atmpspheric pressure (_atm_)
Remember : Temperature is given in Celsius while SI unit is Kelvin (_K_)
0 Celsius = 273.15Kelvin
The gas constant (_R_) has value of _0.082dm^(3).atm.K^(-1).mol^(-1)_
def solution(molar_mass1, molar_mass2, given_mass1, given_mass2, volume, temp) :
    molar_mass1 = given_mass1*0.001/molar_mass1
    molar_mass2 = given_mass2*0.001/molar_mass2
    tempKelvin = temp + 273.15
    R = 0.082
    Ptotal = (((molar_mass1 + molar_mass2)*R*tempKelvin)/volume)*1000
    return Ptotal
def solution(molar_mass1, molar_mass2, given_mass1, given_mass2, volume, temp) :
    molar_mass1 = given_mass1*0.001/molar_mass1
    molar_mass2 = given_mass2*0.001/molar_mass2
    tempKelvin = temp + 273.15
    R = 0.082
    Ptotal = (((molar_mass1 + molar_mass2)*R*tempKelvin)/volume)*1000
    return Ptotal