The equilibrium constant K for a certain reaction was measured as a function of temperature (in Kelvin). A plot of ln(K) versus 1/T for this reaction gives a straight line with a slope of 1.352 x 104 K and a y-intercept of -14.51. Determine the value of ΔH° for this reaction.

- 1.124 x 10⁵ J = -1.124 x 10² kJ

Step-by-step explanation:

The change in Gibbs free energy is related to the equilibrium constant K by

ΔGº = - RTlnK

But, we also know that by definition

ΔGº = ΔHº - TΔSº

thus

ΔHº - TΔSº =  - RTlnK

lnK = - ΔHº/RT + ΔSº/R

This equation has the form y = mx + b where m is the slope and b is the y intercept.

Therefore, a plot lnK versus 1/T will give us a straight line with slope ,        m= - ΔHº/R.

We know m = 1.352 x 10⁴ K

so we can solve for ΔHº

ΔHº = - mR = 1.352 x 10⁴ K  x 8.314 J / K = - 1.124 x 10⁵ J = -1.124 x 10² kJ

answer: all of the odd numbers were opened

the first person was the one that was opening all of the lockers. since one is odd, this causes all of the odd number lockers to be opened in the end.