The heat of formation of liquid hydrazine (N 2 H 4 ) is 50.63 kJ/mol. Use tabula

Question

The heat of formation of liquid hydrazine (N2H4) is 50.63 kJ/mol. Use tabulated data for other heats of formation.

The tolerance on each question is only 0.03 kJ, so express all answers to 0.01 kJ.

H = kJ q = kJ w = kJ E = kJ Determine delta H, q, w, and delta E at 298 K and 1 atm for the complete reaction of 8.560 g of N2O4. N2O4(g) + 2N2H4(l) 3N2(g) + 4H2O(l). The heat of formation of liquid hydrazine (N2H4) is 50.63 kJ/mol. Use tabulated data for other heats of formation. The tolerance on each question is only 0.03 kJ, so express all answers to 0.01 kJ.

Explanation / Answer

First you need to find all your values for H from the book. Once you have them do products minus the reactants. So for example 3(value for N2)+2(value for H20) - (50.63) + 2(value for N2H4) Make sure you look up the right values in the correct states. If it says liquid look up the value of H for water as liquid. Remeber though that you have 8.560g so divide that by the wieght of N2O4 to get your ratio. Then multiply all the numbers you got by this ratio.

Q=delta H when preasure is constant. So take your delta H and multiply it by the molar ratio you got.

W=-q

Change in E equals= q-w

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

---

---

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