Formation reaction involves formation of compound from its individual elements. N2H4 contains N2and H2 as its constituents. So, formation reaction is;
N2(g) + 2H2(g) -----> N2H4(g)
What is the equation for the formation reaction for gaseous hydrazine, N2H4, at 25°C and 1...
The formation of hydrazine N2H4(g) follows the proposed mechanism: Step I) N2 + H2 → N2H2 Step II) H2 + N2H2 → N2H4 If the second step is the slow step, write the rate law for the overall reaction. Show your work.
3. (3 points) Hydrazine (N2H4) can react with oxyger in the following chemical reaction: NaH.(1 +0:0) - N2(g) + 2H20 (1) Calculate AH, for the reaction above, given the following data: 2NH3(g) + 3N20(g) - 4260) + 3H2000 AH,º=-1010. kJ/mol N20(g) + 3H2(g) → N2H (1) + H2O(1 AH-=-317 k!/inol 2NH3(g) + 40:09) - NzH4O + H20(1 AH,"=-143 kJ/mol H2(g) +4202(9) - H20(1) AH"=-286 kJ/mol
Hydrazine reacts with O2 according to the following equation: N2H4(g) + O2(g) → N2(g) + 2H2O(l) Assume the 02 needed for the reaction is in a 720 L tank at 27.0°C what must the oxygen pressure be in the tank to have enough oxygen to consume 2.47 kg of hydrazine completely? Pressure = _______ atm
Hydrazine (N2H4) is a fuel used by some spacecraft. It is normally oxidized by N2O4according to this equation: N2H4(l)+N2O4(g)→2N2O(g)+2H2O(g) Standard Enthalpies of Formation at 25 ∘C Substance ΔH∘f(kJ/mol) N2H4(l) 50.6 N2H4(g) 95.4 N2O(g) 81.6 N2O4(l) −19.5 N2O4(g) 9.16 H2O(l) −285.8 H2O(g) −241.8 Calculate ΔH∘rxn for this reaction using standard enthalpies of formation. Express your answer using one decimal place.
15. (10 pts.) Hydrazine (N,Ha) is commonly used as rocket fuel. It reacts with oxygen according to the balanced chemical equation: N2H4(g) + 302(g) + 2N02(g) + 2H20(1) 70.5 g of Hydrazine (N,Ha) is reacted with 195.3 g of Oz to test the thermodynamics of the reaction. MAKE SURE TO SHOW ALL OF YOUR WORK Compound Molecular Weight (g/mol) N2H4 32.06 0 32.00 NOZ 46.01 a. Identify the limiting reactant: b. How many grams of NO, should be produced in...
Please explain step by step
12. Calculate the standard reaction enthalpy for the reaction: N2H4(4) + H2(g) → 2NH3(g) Given: N2H4(4) + O2(g) → N2(g) + 2H2O(g) AH° = 0543 kJ 2H2(g) + O2(g) → 2H2O(g) AH° = 1484 kJ N2(g) + 3H2(g) + 2NH3(g) AH° = 092.2 kJ A. - 1119 kJ B. - 33 kJ C. -151 kJ D. + 151 kJ E. + 1119 kJ
Determine the limiting reactant for the reaction of 50.0 g N204 and 50.0 g N2H4. Some possibly useful molar masses are as follows: N204 = 92.02 g/mol, N2H4 = 32.05 g/mol. N2016) + 2N2H4() — 3 N2(g) + 4H2O(g) ON2 O N₂ Ha N20 ОНО
hydrazine N2H4 reacts with oxygen to form nitrogen gas and
water
Hydrazine, N, H, reacts with oxygen to form nitrogen gas and water. N,H, (aq) +0,6) N,(g) + 2 H2O(1) If 2.45 g of N, H, reacts with excess oxygen and produces 0.950 L of N,, at 295 K and 1.00 atm, what is the percent yield of the reaction? percent yield:
question 17.77
AMMONA Ammonia, NH3, is used to make hydrazine, N2H4, which can be used as a fuel. Calculate AG° at 300 and 390 K for the following 17.76 reactions. (a) BaCOs(s)BaO(s) +CO2(g) (b) CH2COOH(l) - CH(g) +CO2g) 17.77 Suppose you are looking for a chemical reaction that is spontaneous at low temperatures but proceeds in the reverse direction at high temperatures. What are the signs of AH" and AS for such a reaction? 17.78 Suppose you are looking for...
For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N2(g) + 3H2(g) + 2NH3(g) the standard change in Gibbs free energy is AG° –72.6 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are Pin, 0.150 atm, PH, = 0.200 atm, and PNH, 0.850 atm? = = =