Avessel of volume 22.4 dm3 contains 20 mol h2 and 1 mol n2 ad 273.15 k initially. all of the nitrogen reacted with sufficient hydrogen to form nh3. calculate the total pressure and the partial pressure of each component in the final mixture at 273.15 k.

Nitrogen combine with hydrogen to produce ammonia at a ratio:

Assuming that the reaction has indeed proceeded to completion- with all nitrogen used up as the question has indicated. of hydrogen gas would have been consumed while of ammonia would have been produced. The final mixture would therefore contain

Apply the ideal gas law to find the total pressure inside the container and the respective partial pressure of hydrogen and ammonia:

not clear

answer: the value of enthalpy change will be -152.80 kj.

solution:

pressure = 1atm , temperature = = 298 k

given that pressure and temperature are same in both gases , the number of moles of both gases can be determined by the ideal gas equation.

according to reaction 3 moles no are reacting with 1 mol of ,then 0.49 mol of no will react with moles of ozone that is 0.16 moles of ozone. since, no is limiting reagent and is an excessive reagent.

enthalpy change for the reaction between the given volumes of the gases is :