Asample of o2 gas is observed to effuse through a porous barrier in 5.69 minutes. under
the same conditions, the same number of moles of an unknown gas requires 11.7 minutes
to effuse through the same barrier. what is the molar mass of the unknown gas?
a) 11.6 g/mol
b) 135 g/mol
c) 7.56 g/mol
d) 66.5 g/mol
e) more information is needed

MX = 135 g/mol

Explanation:

The rate of effusion (r) is the distance travelled (d) over the time elapsed (t). Let's call the uknown gas X. The ratio of rates rO₂/rX is:

We can find the molar mass of X using Graham's law.

answer: the value of enthalpy change will be -152.80 kj.

solution:

pressure = 1atm , temperature = = 298 k

given that pressure and temperature are same in both gases , the number of moles of both gases can be determined by the ideal gas equation.

according to reaction 3 moles no are reacting with 1 mol of ,then 0.49 mol of no will react with moles of ozone that is 0.16 moles of ozone. since, no is limiting reagent and is an excessive reagent.

enthalpy change for the reaction between the given volumes of the gases is :