Consider the production of liquid water, H2O(l), from hydrogen combustion: H2(g)

Question

Consider the production of liquid water, H2O(l), from hydrogen combustion:
H2(g) + 1/2 O2(g) H2O(l) H = -285.9 kJ

(a) What is the enthalpy change for the reverse reaction?

Hreverse = kJ/mol.




(b) Balance the forward reaction with whole-number coefficients. What is H for the reaction represented by this equation?

H = kJ/mol.




(c) Which is more likely to be thermodynamically-favored, the forward reaction or the reverse reaction?






(d) If the (forward) reaction were written to produce water gas, H2O(g), instead of liquid water, would you expect the magnitude of H to increase (become more positive), decrease (become more negative), or stay the same?

H should .

Explanation / Answer

a) H = 285.9 KJ b) 2H2 + O2 ---> 2H2O , H = -571.8 c) forward reaction is favoured thermodynamically d) H value increases i.e H becomes more positive

Related Questions

Navigate

• Browse (All)
• Browse C
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.