The following sequence of reactions occurs in the commercial productions of aqueous nitric acid: 4NH3(g) + 5O2(g) ⟶ 4NO(g) + 6H2O(l); LaTeX: ΔH = -907 kJ

2NO(g) + O2(g) ⟶ 2NO2(g); ΔH = -113 kJ

3NO2 + H2O(l) ⟶ 2HNO3(aq) + NO(g); ΔH = -139 kJ

Determine the total energy change for the production of one mole of aqueous nitric acid by this process.

Chlorine and water react to form hydrogen chloride and oxygen, like this: 2cl2 (g) + 2h2o (g) → 4hcl (g) + o2 (g) also, a chemist finds that at a certain temperature the equilibrium mixture of chlorine, water, hydrogen chloride, and oxygen has the following composition: compound concentration at equilibrium cl2 0.55m h2o 0.57m hcl 0.53m o2 0.34m calculate the value of the equilibrium constant kc for this reaction. round your answer to 2 significant digits.

Which one of the following substances would be the most soluble in ccl4? na2so4 h2o ch3ch2ch2ch2oh c4h10 hi

The diagrams to the right show the distribution and arrangement of gas particles in two different containers. according to kinetic-molecular theory, which of the following statements is true? check all that apply. if the temperatures of both containers are equal, container a has greater pressure than container b. if the volume of container a decreased, its pressure would decrease. if the pressure in both containers is equal, container a has a lower temperature than container b.