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

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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 H, q, w, and 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. W is -0.4976. I really need help with the rest. Thanks. So I am having trouble determining delta H and q and then I know once I solveb hese I will be able to determine work and E of the reaction. I looked up heat formation for the other chemicals involved and it as so: HF N2SO4= -19.5 N2= 0 H2O= -285.83 I also need help with delta E.

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