Question #ef325

1 Answer
Sep 12, 2017

Answer:

#~=54*kg*"melamine"#

Explanation:

We need a stoichiometric equation that represents the formation of melamine.

#6(H_2N)_2CO(s) rarr underbrace(C_3H_6N_6(s))_"melamine" + 6 NH_3(g) + 3 CO_2(g)#

Which I think is balanced. And thus we see that each equiv melamine required SIX EQUIV urea

And thus....#"mass of melamine"# given by........

#1/6xxunderbrace((154.5xx10^3*g)/(60.06*g*mol^-1))_"moles of urea"xxunderbrace(126.12*g*mol^-1)_"molar mass of melamine"xx78.0%=#

#~=54*kg*"melamine"#