9B. In the gaseous reaction between ammonia, oxygen gas, and methane, hydrogen cyanide and water are produced. Ideally, what mass of each product is yielded if you start with 600. g of each reactant?

Answer 1

In the gaseous reaction between ammonia, oxygen gas, and methane, hydrogen cyanide and water are produced. Ideally, what mass of each product is yielded if you start with 600. g of each reactant?

First, you MUST begin with a correctly balanced equation:

2NH3(g) + 3O2(g) + 2CH4(g) ==> 2HCN(g) + 6H2O(l)

Starting with 600 g NH3:

600 g x 1 mol NH3/17 g x 2 mol HCN/2 moles NH3 x 27 g HCN/mole = 953 g HCN (3 sig. figs.)

600 g x 1 mol NH3/17 g x 6 mol H2O/2 moles NH3 x 18g H2O/mole = 1910 g H2O (3 sig. figs.)

Starting with 600 g O2:

600 g x 1 mol O2/32 g x 2 mole HCN/3 moles O2 x 27 g HCN/mole = 338 g HCN (3 sig. figs.)

600 g x 1 mol O2/32 g x 6 moles H2O/3 moles O2 x 18 g H2O/mole = 675 g H2O (3 sig. figs.)

Starting with 600 g CH4:

you should be able to do this yourself by following the above examples.