Question

What is the change in entropy when 7.61 mL of liquid benzene (C6H6, d = 0.879 g/mL) is combusted in the presence of 22.3 L of oxygen gas, measured at 298 K and 1 atm pressure? (R = 0.0821 L · atm/(K · mol)) 2C6H6(l) + 15O2(g) → 12CO2(g) + 6H2O(l); ΔS° = –437.7 J/K at 298 K a. 436 J/K b. 37.4 J/K c. 398 J/K d. 45.3 J/K e. 18.7 J/K

Answer 1

option e, 18.7 J/K

Step-by-step explanation:

Volume of C6H6 = 7.61 mL

Density of C6H6 = 0.879 g/mol

`Mass=Volume* density`

`Mass=7.61* 0.879 = 6.69 g\;mol`

No. of mol = Mass in g/Molecular mass

No. of mol of benzene = 6.69/78 = 0.086 mol

Volume of oxygen = 22.3 L

No. of moles of oxygen will be calculated using PV = nRT

Where,

P = 1 atm, V = 22.3 L, R = 0.0821 L · atm/(K · mol, T = 298 K

n = PV/RT

`n=(1*22.3)/(0.0821*298)=0.911 mol`

`2C_6H_6\;(l) + 15O_2 (g)\rightarrow 12CO_2 (g)\;6H_2O (l)`

From reaction stoichiometry,

2 moles of benzene react with 15 moles of O2

0.086 mole of benzene will react with

`15* 0.086/2=0.645` mol of O2

Since, 0.911 mol of O2 is present in reaction mixture, therefore O2 will not be the limiting reagent.

So the limiting reagent of the reaction will ne C6H6.

2 moles of C6H6 reacts with O2, then change in entropy is –437.7 J/K

0.086 mole of C6H6 reacts with O2 and change in entropy

`=437.7 J/K * 0.086/2 = 18.7 J/K`

so, the correct will be option e.