When production first began some eighty years ago, ammonia production relied upon the direct reaction between gaseous hydrogen and nitrogen called the haber process: 3 h2(g) + n2(g) ⇀↽ 2 nh3(g) ∆h = −92.2 kj decreasing the temperature of an equilibrated reaction between hydrogen and nitrogen will 1. increase the velocity of the gas molecules. 2. produce more ammonia. 3. increase the kinetic energy of the gas molecules. 4. produce less ammonia. 5. have no effect.

Explanation:

The influence of temperature in equilibrium reactions can be predicted from the heat (enthalpy) information.

This is the chemical reaction:

The information about the enthalpy of the reaction, ∆H = − 92.2 kJ,  indicates that energy (heat) has been released to the surroundings (the products of the forward reaction have less energy than the reactants), which is defined as an exothermic reaction.

Then, you can rewrite the equaition in the form:

This is, the heat can be seen as a product of the direct reaction (or a reactant of the reverse reaction).

Now, it is quite straight to apply  Le Chatelier's principle:

a) Decreasing temperature is equivalent to extract heat or having less heat on the left side.

b) Then, the equilibrium must shift in a way that this lack of heat is compensated. Then, the reaction will shift to the right to produce more heat.

As conclusion, you can tell that in exothermic reactions, a decrase in temperature will cause the equilibrium to shift to the right.

This shift, of course, means the production of more ammonia.

The other choices are discarded following this brief reasoning:

1. increase the velocity of the gas molecules: the average velocity of the particles increases when the average kinetic energy increases, and the average kinetic energy will decrease if the temperature decreases. So, this statement is false.

3. increase the kinetic energy of the gas molecules: no, the average kinetic energy is proportional to the temperature, then reducing the temperature decreasese the average kinetic energy.

4. produce less ammonia: it was shown that reducing the temperature will produce more ammonia.

5. have no effect: no, it does have effect, as shown.

  the   balanced   equation   for   reaction of   ca metal   with   o2 to   produce   cao   is as below

2 ca+ o2→ 2 cao2

  explanation

the reaction is   balanced     since the   number of atoms   in reactant side is   equal to   number of atoms   in   product side.   for   example   they   are 2   atom of   ca in   reactant   side   and   2   atoms of ca   in   the product side.

  the   process   is a   meet the   requirement   of   redox   reaction because :     calcium   is   oxidized   from   oxidation state 0   to 2+   while   oxygen   is reduced from   oxidation   state   0   to 2-