Question

question 10 (1 point)
4 ph₃ + 2 h₂ + 9 o₂ ⇔ 2 p₂o₅ + 8 h₂o(liq) + 25 kj
the reaction has δg = - 25 kj or δg = + 25 kj ? 1
the reaction is exergonic or endergonic ? 2
the reaction is spontaneous or non - spontaneous ? 3
a. exothermic b. endothermic c. absorbs heat d. gives off heat
e. none of these choices f. exergonic g. endergonic h. δg = - 25 kj
i. δg = + 25 kj j. spontaneous k. non - spontaneous

Explanation:

Step1: Analyze ΔG sign

In the reaction, energy (25 kJ) is a product (on the right side), meaning the reaction releases free energy. For a reaction that releases free energy, $\Delta G$ is negative. So $\Delta G = -25$ kJ (option H).

Step2: Determine exergonic/endergonic

A reaction with $\Delta G < 0$ (negative) is exergonic (releases free energy). So the reaction is exergonic (option F).

Step3: Determine spontaneous/non - spontaneous

Exergonic reactions (ΔG < 0) are spontaneous because they can occur without external energy input. So the reaction is spontaneous (option J).

Answer:

1. H. $\Delta G = - 25$ kJ
2. F. exergonic
3. J. spontaneous