Consider the following reaction at constant P. Use the information here to determine the value of ΔSsurr at 398 K. Predict whether or not this reaction will be spontaneous at this temperature. 4 NH3(g) + 3 O2(g) → 2 N2(g) + 6 H2O(g) ΔH = -1267 kJ

The reaction                         2 NO(g)   ⇆  N2O4(g) occurs at 25oC under standard state conditions with ΔGo = 13.1 kJ/mol. What is the free energy change (in J/mol) when the NO partial pressure is 0.649 Atm and the N2O4 partial pressure is 0.0015 Atm?

Consider the two different systems, A and B, shown below.  If there are 3 particles with a total energy of 12 J, which system would have more entropy and why? Question 21 options:   System A has more entropy because it has greater separation between energy levels and hence more microstates than system B.   System B has more entropy because it has more than two microstates, whereas System A only has two microstates possible.   System A has more entropy because it has three microstates, whereas System B has less than three microstates possible.   System B has more entropy because it has more than three microstates, whereas System A only has three microstates possible.   System A has more entropy because it has more than one microstate, whereas System B only has one microstate possible.

Read the descriptions of physical or chemical changes in the table below. Then decide whether the change will be spontaneous, if you can. Change A gas condenses to a liquid, neither absorbing nor releasing heat. An exothermic chemical reaction between a solid and a liquid results in gaseous products. Two liquids mix, neither absorbing nor releasing heat. Is this change spontaneous? Yes. No. Can't decide with information given. ○ Yes. ○ No. Can't decide with information given. Yes. No. ○ Can't decide with information given.