Formation of Nitric Acid
From given reactions ,
Rxn(2) + 1/2 × rxn(1)
1/2 N2 + .3/2 H2 + 2 O2 -------> HNO3 + H2O
So ∆Hrxn = -330 - (-92/2)
=> -376 kJ
Nitric acid can be formed in two steps from the atmospheric gases nitrogen and oxygen, plus...
Nitric acid can be formed in two steps from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by reforming natural gas. In the first step, nitrogen and hydrogen react to form ammonia: N (0) + 3H (9) 2 NH,(9) AH = -92. kJ In the second step, ammonia and oxygen react to form nitric acid and water: NH (g) + 20 (g) – INO,g) + H20() AH -330, RJ Calculate the net change in enthalpy for the formation of...
Nitric acid can be formed in two steps from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by reforming natural gas. In the first step, nitrogen and hydrogen react to form ammonia: N2(g) + 3H2(g) 2NH3(g) H = -92.kJ In the second step, ammonia and oxygen react to form nitric acid and water: NH3(g) + 2O2(g) HNO3(g) + H20 (g) H=-330.kJ Calculate the net change in enthalpy for the formation of one mole of nitric acid from nitrogen, hydrogen...
Nitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, plus hydrogen prepared by reforming of natural gas, in a two-step process. In the first step, nitrogen and hydrogen react to form ammonia:N2(g)+3H2(g)→2NH3(g)In the second step, ammonia and oxygen react to form nitric acid and water:NH3(g)+2O2(g)→HNO3(g)+H2O(g)Write the net chemical equation for the production of nitric acid from nitrogen, hydrogen and oxygen. Be sure your equation is balanced.
Nitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, and hydrogen prepared by reforming natural gas, in a two-step process. In the first step, nitrogen and hydrogen react to form ammonia: N2+3H2=2NH3 In the second step, ammonia and oxygen react to form nitric acid HNO3 and water: NH3+ 2O2=HNO3+H2O Suppose the yield of the first step is 96.% and the yield of the second step is 85.%. Calculate the mass of hydrogen required to make 5.0kg of...
Nitric oxide (NO) can be formed from nitrogen, hydrogen and oxygen in two steps. In the first step, nitrogen and hydrogen react to form ammonia: N2(9) + 3 H (9) 2NH (9) AH = -92. kJ In the second step, ammonia and oxygen react to form nitric oxide and water: 4 NH (9) + 50,(9) 4 NO(9) + 6H2O(9) AH = -905. kJ Calculate the net change in enthalpy for the formation of one mole of nitric oxide from nitrogen,...
Nitric acid is often manufactured from the atmospheric gases nitrogen and oxygen, and hydrogen prepared by reforming natural gas, in a two-step process. In the first step, nitrogen and hydrogen react to form ammonia: 2 NH,(8) N2(8) + 3H2(8) In the second step, ammonia and oxygen react to form nitric acid (HNO) and water: NH5()+ 20,(8) HNO,(8) + H,O(8) Suppose the yleld of the first step is 62. % and the yield of the second step is 71.%. Calculate the...
? ?STOICHIOMETRY Writing the net equation for a sequence of reactions utnc atid s teten manufactred from the atmospheic gass nitrogen and oxygen, plus hydrogen prepared by reforming of natural gas, in a two step process In the first step, nitrogen and hydrogen react to form ammonia: N(9)+3 H2(9)-2NH,(9) In the second step, ammonia and oxygen react to form nitric acid and water: NH3(9)+202(9)-HNO (9)+H20(9) Write the net chemical equation for the production of nitric acid from nitrogen, hydrogen and...
The Ostwald process for the commercial production of nitric acid from ammonia and oxygen involves the steps in the table below. (a) Use the values of AHfº in Appendix 4 to calculate the value of AHO for each of the following reactions. Reaction AH 4 NH3(g) + 5 02(9) ► 4 NO(g) + 6 H20(9) 2 NO(g) + O2(g) +2 NO2(9) 3 NO2(g) + H20(1) - 2 HNO3(aq) + NO(g) (b) Write the overall equation for the production of nitric...
An Important step in the synthesis of nitric acid is the conversion of ammonia to nitric oxide according to the following balanced chemical equation. What is AHpxn for this reaction? 4NH3(g) + 5O2(g) -4NO(g) + 6H2O(9) Substance AH?f(kJ/mol) NH3(g) -46.3 NO(9) 90.3 H2O(9) -241.8 0 -1274.8 kJ/mol -904.4 kJ/mol 0 -240.2 kJ/mol 0 -197.8kJ 197.8 kJ/mol
There are two steps in the usual industrial preparation of acrylic acid, the immediate precursor of several useful plastics. In the first step, calcium carbide and water react to form acetylene and calcium hydroxide: CaC (s) + 2 H2O(g) - CH (9) + Ca(OH),(s) AH -414. kJ In the second step, acetylene, carbon dioxide and water react to form acrylic acid: 6 C H (9) + 3 CO2(9) + 4H2O(g) - SCH,CHCO,H) AH-132. kJ Calculate the net change in enthalpy...