Question

A chemist fills a reaction vessel with 9.47 atm nitrogen monoxide (NO) gas, 2.61 atm chlorine (C12) gas, and 8.64 atm nitrosyl chloride (NOCI) gas at a temperature of 25.0°C. Under these conditions, calculate the reaction free energy AG for the following chemical reaction:

2NO(g) + Cl2(g) = 2NOCI (g)
Use the thermodynamic information in the ALEKS Data tab. Round your answer to the nearest kilojoule.

Answer 1

Answer: The Gibbs free energy change of the reaction is 2.832 kJ.

Step-by-step explanation:

The relationship between Gibbs free energy change and reaction quotient of the reaction is:

`\Delta G^o=-RT\ln Q_p`

where,

`\Delta G^o` = Gibbs free energy change

R = Gas constant = 8.314 J/mol.K

T = temperature =
`25^oC=298K`

`Q_p` = reaction quotient =
`(p_(NOCl)^2)/((p_(NO)^2)* (p_(Cl_2)))`

We are given:

`p_(NOCl)=8.64atm\\p_(NO)=9.47atm\\p_(Cl_2)=2.61atm`

Putting values in above equation, we get:

`\Delta G^o=-(8.314)* 298K* \ln (((8.64)^2)/((9.47)^2* (2.61)))\\\\\Delta G^o=-8.314* 298* (-1.143)`

`\Delta G^o=2831.86J=2.832kJ` (Conversion factor: 1 kJ = 1000 J)

Hence, the Gibbs free energy change of the reaction is 2.832 kJ.