Question

The value of the equilibrium constant for a reaction is 2.65 x 10-6 at 35° Calculate the value of LaTeX: \DeltaΔG°rxn.

Answer 1

The answer is "33.95
`\bold{ (kj)/(mol)}\\`".

Step-by-step explanation:

Formula:

`\bigtriangleup G_0= -R * T l_n * K_(eq)\\`

where

`K_(eq) = \text{equilibrium constant}\\`

Given value:

`T =35^(\circ) C\\`

convert temperature celsius (°C) to Kelvin (K):

`= (273+45) \ kelvin \\\\= 318 \ Kelvin \\\\= 318 \ K`

`R = 8.314 \ \ (J)/( mol \cdot K)`

`\bigtriangleup G_0= -(8.314 ) * 31.8 * l_n (2.65* 10^(-6))\\`

`=-(8.314 ) * 31.8T l_n * (2.65* 10^(-6))\\\\`

After solving the value it will give:

= 33.95
`\bold{ (kj)/(mol)}\\`