The rate of effusion of Xe gas through a porous barrier is observed to be 9.14 x 10-4 mol/h. Under the same conditions, the rate of effusion of Ar gas would be:
mol/h.​

Rate of Ar= 1.65 x mol/h

Explanation:

Here we'll use Graham's Law where

R= rate of effusion and M= molar mass

Let's plug in what we know.

You could switch them where Xe is M1 (on the bottom)  instead of M2, but I find it easier when the unknown is R1, where it acts like a whole number. It makes the algebra part of the equation easier.

Let's solve for R1.

R1= 1.089 x

R1= 1.65 x mol/h

the correct answer is a

answer: the enthalpy of the overall chemical reaction is +87.88 kj or +88 kj.

according to hess's law, the overall enthalpy of a reaction is the difference between the sum of enthalpy values of all the products and the sum of enthalpy values of all the reactants.

δh(reaction) = ∑nδh(products) - ∑nδh(reactants)

δh(reaction) = [δh +δh] - [δh]

δh(reaction) = [1(-287.02) + 1(0) ] - [1(-374.9)] kj = +87.88 kj

here, δh (pcl3) = -287.02 kj, δh(cl2) = 0, δh(pcl5) = -374.9 kj

therefore, enthalpy of the overall reaction is +87.88 kj or +88 kj.