If 29.4 grams of hydrogen and 3701.3 grams of iodine combine to form hydrogen iodide, how many grams of hydrogen iodide must form?

1 Answer
Apr 5, 2016

Answer:

#3.730kg#

Explanation:

First write down a balanced chemical equation for the reaction :

#H_2+I_2->2HI#

This represents the mole ratio in which chemicals combine.

Now calculate the number of moles of each reactant present :

#n_(H_2)=m/M_r=29.4/2=14.7mol#

#n_(I_2)=m/M_r=3701.3/253.8=14.583mol#

Since the balanced chemical equation illustrates that the reactants combine in a #1:1# ratio, it implies that iodine is the limiting reagent and decides how much product is formed. Hydrogen is in excess.

So hence, since #1mol I_2# produces #2molHI#, it follows that #14.583molI_2# will produce #29.166molHI#

This corresponds to a mass of product of

#m=nxxM_r#

#=29.166xx127.9#

#=3730.33g#