Calculate ΔGo for the reaction of ammonia with oxygen:
4NH3 (g) + 3 O2 (g) → 2N2 (g) + 6 H2O (g)
using the following data:
Substance NH3 (g) O2 (g) N2 (g) H2O (g)
ΔGo (kJ/mol) - 16 0 0 -228.6
a) 212.6 kJ
b) 1307.6 kJ
c) - 212.6 kJ
d) -1435.6 kJ
e) -1307.6kJ
Calculate ΔGo for the reaction of ammonia with oxygen: 4NH3 (g) + 3 O2 (g)...
Ammonia can be oxidized in oxygen as shown: 4 NH3(g) + 3 O2(g) <=> 2 N2(g) + 6 H2O(g). When 0.541 mol of NH3 and 0.595 mol of O2 are placed in a 1.00 L container at a certain temperature, the equilibrium {N2} is 0.1347. Calculate the value of Kc for the reaction. Give your answer to 4 decimal places.
1) Ammonia, NH3, reacts with molecular oxygen, O2, to form nitric oxide, NO, and water:4NH3(g) + 5O2(g) = 4NO (g) +6H2O(l)A. What is the limiting reactant and what is the theoretical yield of NO?B. What is the theoretical yield of H2O?C. How many grams of excess reagent will be left over?D. If the actual yield of NO had been 91 g, what would be the percent yield of the reaction
Ammonia reacts with oxygen to form nitric oxide and water vapor: 4NH3 + 5O2 ---> 4NO + 6H2O When 20.0 g NH3 and 50.0 g O2 are allowed to react, which is the limiting reagent? A) NO B) O2 C) H2O D) no reagent is limiting E) NH3 What is the coefficient for O2 when the following combustion reaction of a hydrocarbon is balanced? ___C7H14 + ___ O2 ---> ___ CO2 + __ H2O A) none of these B) 10...
35. Calculate ΔrH° for the combustion of ammonia, 4 NH3(g) + 7 O2(g) → 4 NO2(g) + 6 H2O( ) using standard molar enthalpies of formation. molecule ΔfH° (kJ/mol-rxn) NH3(g) –45.9 NO2(g) +33.1 H2O( ) –285.8 a. +30.24 kJ/mol-rxn b. –206.9 kJ/mol-rxn c. –298.6 kJ/mol-rxn d. –1398.8 kJ/mol-rxn e. –1663.6 kJ/mol-rxn
Ammonia reacts with oxygen according to the equation: 4NH3(g) +502(g) → 4NO(g) + 6H2O(g) AH.,.. = 4906 kJ Calculate the heat (in kJ) associated with the complete reaction of 355 g of NH3. Express your answer with the appropriate units. Value Units
Ammonia reacts with oxygen to form nitrogen dioxide and steam, as follows: 4NH3(g) + 7O2(g) ---> 4NO2(g) + 6H2O(g) Using the following bond energies, estimate the enthalpy change for the reaction. BE(O–H) = 464 kJ/mol BE(N–H) = 389 kJ/mol BE(O=O) = 498 kJ/mol BE(N–O) = 222 kJ/mol BE(N=O) = 590 kJ/mol
. Given the following reaction at 25o C. 4NH3(g) + 5 O2(g) 4NO(g) + 6H2O(l) ΔHo = -1168 kJ ΔHo f(NH3) = -46.2 kJ/mol; ΔHo f(H2O) = -285.8 kJ/mol. What is the standard enthalpy of formation of NO gas at 25o C?
Anhydrous ammonia is an ultra-clean and energy-dense alternative fuel that produces no greenhouse gases on combustion. In an experiment, gaseous ammonia is burned with oxygen in a container of fixed volume per the following equation: 4NH3(g) + 302(g) -> 2N2(g) 6H20(0) The initial and final states are at 298 K. After combustion with 12.80 g of O2, some NH3 remains unreacted. Calculate the enthalpy change during the process, given the following data. | ?,Ho (KJ mol-1) compound NH3 (g) H20...
Determine ΔrH° for the following reaction, 2 NH3(g) + 5/2 O2(g) → 2 NO(g) + 3 H2O(g) given the thermochemical equations below. N2(g) + O2(g) → 2 NO(g) ΔrH° = +180.8 kJ/mol-rxn N2(g) + 3 H2(g) → 2 NH3(g) ΔrH° = –91.8 kJ/mol-rxn2 2H2(g) + O2(g) → 2 H2O(g) ΔrH° = –483.6 kJ/mol-rxn a. –1178.2 kJ/mol-rxn b. –452.8 kJ/mol-rxn c. –394.6 kJ/mol-rxn d. –211.0 kJ/mol-rxn e. +1178.2 kJ/mol-rxn
1. Ammonia reacts with oxygen according to the equation 4NH3(g)+5O2(g)→4NO(g)+6H2O(g),ΔHrxn=−906 kJ Calculate the heat (in kJ) associated with the complete reaction of 155 g of NH3. 2. What mass of butane in grams is necessary to produce 1.5×103 kJ of heat? What mass of CO2 is produced? Assume the reaction to be as follows: C4H10(g)+132O2(g)→4CO2(g)+5H2O(g),ΔHrxn=−2658 kJ