The heat of formation of liquid hydrazine (N 2 H 4 ) is 50.63 kJ/mol. Use tabula
ID: 787227 • Letter: T
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.
I also need help with delta E.
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.Explanation / Answer
Anyways....Ok, so delta H is -125.924 kj
q is going to be the same exact answer as delta H in this case.
w is equal to -moles of gas (produced minus consumed) * 8.314 * 298
w1 = -4.955 kj
but this for for a full scale reaction. since we only need 9.24/92.011 amount, multiply moles * w1. additionally, there is still only mol of n2o4 so just multiply by 1.
w = -.4976 kj
and delta E is simply q + w. e = -126.422 kj
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