Nitrogen gas reacts with hydrogen gas to form ammonia what are reactants in this chemical reaction?

1 mol 2 mol  

84g of N2(g) = 84/28 = 3 mol of N2(g)  

From the above reaction 1 mol of N2(g) gives 2 mol 0f NH3(g). So 3 mol of N2(g) should give 6 mol or (6x17) 102 g of NH3(g). But we are getting only 85.0 g of NH3.  

Hence %yield of NH3 = 100x85.0/102 = 83.3%  

Answer D. is correct.  

2. 2HgO (s) 2Hg (l) + O2 (g)  

2 mol 2 mol 1 mol  

4 mol 4 mol 2 mol  

As only 1.5 mol of O2 is obtained, so % yield = 1.5x100/2 = 75.0%  

Moreover 603 g of Hg = 603/200.59 = 3.00 molof Hg. Considering this also  

% yield = 3x100/4 = 75%

Nitrogen gas and hydrogen gas

3H 2 (g)+ N 2 (g)= 2 NH 3 (g)

This is the chemical reaction for above experiment.

A mixture of nitrogen gas and hydrogen gas reacts in a closed container to form ammonia, . The reaction ceases before either reactant has been totally consumed.

Molybdenum as promoter too can enhance the effeciency of the catalyst.

is this for the e2020 class

i was thinking 4.0 v hope this