Question

For a particular reaction delta h = 34.2kj and dela s = 99.2j. assuming these values chnage very little with temperature, at what temperature does the reaction change from nonspontaneous to spontanrous in the forward direction

a) 345 K
b) 367 K
c) 298 K
d) 311 K

Answer 1

The temperature at which the reaction changes from nonspontaneous to spontaneous in the forward direction is 345 K.

Step-by-step explanation:

The temperature at which a reaction changes from nonspontaneous to spontaneous in the forward direction can be determined by examining the change in Gibbs free energy (∆G) with temperature.

We can use the equation ∆G = ∆H - T∆S, where ∆H is the change in enthalpy and ∆S is the change in entropy. In this case, the given values are ∆H = 34.2 kJ and ∆S = 99.2 J.

Assuming these values change very little with temperature, we can calculate the temperature at which the reaction becomes spontaneous by setting ∆G equal to zero:

0 = 34.2 kJ - T * 99.2 J

Solving for T, we get:

T = 345 K

Therefore, at a temperature of 345 K, the reaction changes from nonspontaneous to spontaneous in the forward direction.