"High pressur and low temperature favours the formation of ammonia in Haber's processs". Analyse the statement and illustrate the conditions using Le-Chatliers principle?

What is the use of appliying high pressure during the formation of ammonia from nitrogen and hydrogen?

Statement 1 : When hydrogen gas at high pressure and room temperature expands adiabatically into a region of low pressure, there is a decrease in temperature. Statement 2 : Hydrogen gas at room temperature is above its inversion temperature.

Real gases behave ideally at low temperature and high pressure. a) Is the above statement correct or not?

The principle goal of chemical synthesis is to maximize the conversion of reactants into products. Le-Chatlier's principle can be applied to achieve this goal. Preidct the conditions to be applied to maximize the production of ammonia in the following reaction: N_(2(g))+3H_(2(g))iff2NH_(3(g)) DeltaH=-92.38kj mol^-1

"The van der waal's equation reduces itself to the ideal gas equation at low pressure and high temperature". Check whether the statement is true or false?

The following raphs are obtained for He at different conditions. The graph A is drawn at high temperature and low pressure and graph B is drawn at low temperature and high pressure. Which graph represents ideal behaviour?