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 and oxygen. Round your answer to the nearest kJ.

Hence, the net change in enthalpy for the formation of one mole of nitric acid from nitrogen, hydrogen and oxygen is -376 kJ

Explanation:

According to Hess’s law of constant heat summation, the heat absorbed or evolved in a given chemical equation is the same whether the process occurs in one step or several steps.

According to this law, the chemical equation can be treated as ordinary algebraic expression and can be added or subtracted to yield the required equation. That means the enthalpy change of the overall reaction is the sum of the enthalpy changes of the intermediate reactions.

The given chemical reactions are:

   (1)

      (2)

Now we have to determine the value of for the following reaction i.e,

    (3)

According to the Hess’s law, if we multiply the reaction 1 by  and add to 2.

Hence, the net change in enthalpy for the formation of one mole of nitric acid from nitrogen, hydrogen and oxygen is -376 kJ

smooth muscle is composed of involuntary muscles found within the walls of organs and structures such as the esophagus, stomach, intestines, and blood vessels. those muscles push materials like food or blood through organs. unlike skeletal muscle, smooth muscle can never be under your control.

> b takes place in the gas phase in an isothermal tubular reactor. the feed is one mole of a per one mole of c, an inert. the entering temperature and pressure are 427°c and 10 atm, respectively. the gas constant r = 0.08206 atm · l/mol · k.