Answer:
The maximum amount of work that can be done by this system is -2.71 kJ/mol
Explanation:
Maximum amount of work denoted change in gibbs free energy 
during the reaction.
Equilibrium concentration of B = 0.357 M
So equilibrium concentration of A = (1-0.357) M = 0.643 M
So equilibrium constant at 253 K, ![K_{eq}= \frac{[B]}{[A]}](https://tex.z-dn.net/?f=K_%7Beq%7D%3D%20%5Cfrac%7B%5BB%5D%7D%7B%5BA%5D%7D)
[A] and [B] represent equilibrium concentrations
When concentration of A = 0.867 M then B = (1-0.867) M = 0.133 M
So reaction quotient at this situation, 
We know, 
where R is gas constant and T is temperature in kelvin
Here R is 8.314 J/(mol.K), T is 253 K, Q is 0.153 and 
is 0.555
So, 
= -2710 J/mol
= -2.71 kJ/mol
The balanced chemical equation would be as follows:
<span>NH3+HCL->NH4CL
For this, we assume these gases are ideal gases so we can use the equation PV=nRT. We first calculate the number of moles of each reactants. We do as follows:
</span>PV=nRT
1.02 (4.21) = n (0.08206)(27+273.15)
n = 0.17 mol NH3 -------><span>consumed completely and therefore the limiting reactant</span>
PV=nRT
0.998 (5.35 L) = n (0.08206)(26+273.15)
n = 0.22 mol HCl
<span>what mass of NH4Cl(s) will be produced?
0.17 mol NH3 (1 mol NH4Cl / 1 mol NH3 ) = 0.17 mol NH3
which gas is the limiting reactant?
NH3 gas
which gas is present in excess?
HCl gas</span>
Air molecules are spaced far apart is the answer. Since air is a gas, it’s safe to say its particles are separated in random ranges and fits the statement well.
