Calculate ∆H°rxn using
∆Hf° for the reaction
4NH3(g) +
7O2(g) → 4NO2(g)
+ 6H2O(l )
Compound ∆H°f (kJ/mol)
NH3(g) -46.0
NO2 (g) +34.0
H2O(l) -285.9
Calculate ∆H°rxn using ∆Hf° for the reaction 4NH3(g) + 7O2(g) → 4NO2(g) + 6H2O(l ) Compound ∆H°f (kJ/mol)...
What is ΔG°rxn for 2C2H6(g) + 7O2(g) → 4CO2(g) + 6H2O(l) ΔG°f(C2H6) = -33 kJ/mol; ΔG°f(CO2) = -394 kJ/mol; ΔG°f(H2O) = -237 kJ/mol ?
Nitrogen dioxide reacts with water to produce oxygen and ammonia: 4NO2(g)+6H2O(g)→7O2(g)+4NH3(g) How many grams of NH3 can be produced when 4.10 L of NO2 reacts at 385 ∘C and 735 mmHg ?
Refer to the following equation: 4NH3(g) + 7O2(g) ® 4NO2(g) + 6H2O(g) How many molecules of water are produced for each mole of NO2 given off?
Consider the exothermic reaction 2C2H6(g)+7O2(g)→4CO2(g)+6H2O(g) Calculate the standard heat of reaction, or ΔH∘rxn, for this reaction using the given data. Also consider that the standard enthalpy of the formation of elements in their pure form is considered to be zero. Reactant or product ΔH∘f (kJ/mol) C2H6(g) -84.7 CO2(g) -393.5 H2O(g) -241.8 Express your answer to four significant figures and include the appropriate 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
Calculate the ^Ho in (kj) for the following reaction : 4NH3 (s) + 5O2 (g) ---> 4NO (g) + 6H2O (l) ^Ho: NH3 - 46.0 NO 90.0 H2O - 286 A. - 1,172 B. - 1,716 C. - 150 D. - 1,356
Consider the following reaction: 4NH3(g) + 7O2(g) à 4 NO2(g) + 6H2O (l) Is it a balanced or unbalance equation? How many liters of nitrogen dioxide gas is produced from 527 g of gaseous ammonia? Hint: At standard temperature & pressure, 1 mole gas occupies 22.4 Liters
. 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?
Determine delta sub r H in Kj/mol for this reaction. 4No+6H2O --> 4NH3 +5O2 using the equations and the enthalpy change of the reactions given. N2 + O2 --> 2NO delta sub r H= 180.1 NH3 --> 1/2 N2 +1.5H2. delta sub r H= 54.3 2H2O --> 2H2 + O2 delta sub r H= 486.7
LUCJLIUILI Calculate the AH°rxn (in kJ) for combustion of acetone (C3HO): 2C3H6O(g) + 9O2(g) — 6CO2(g) + 6H2O(1) The standard enthalpies of formation are: CO2(g) AH°F = -393.5 kJ/mol H2O(1) AHºr=-285.9 kJ/mol C3H6O(g) AH° = -216.6 kJ/mol