Question

From the following balanced equation, 4NH,(9) +50,(9) — 4NO(g) + 6H2O(1) how many grams of HO can be formed from 3.78 g NH? Select the correct answer below: 2.38 2.676 4.56 O 6.00% Content attribution QUESTION 141 POINT Use the periodic table below to answer the question that follows Presen Hom

Answer 1

Molar mass of NH 3 = 14.0067 + 3( 1.0079 ) = 17.0304 g / mol

Mass of NH 3 = 3.78 g

No. of moles of NH 3 gas = 3.78 g / ( 17.0304 g / mol ) = 0.222 mol

Consider given reaction, 4 NH 3 (g) + 5 O 2 (g) $\rightarrow$ 4 NO (g) + 6 H2O (l)  

According to reaction, 6 mol H2O are produced from 4 mol NH 3 . Hence, moles of H2O produced from 0.222 mol NH 3 would be

0.222 mol NH 3 $\times$ ( 6 mol H2O / 4 mol NH 3 ) = 0.333 mol H2O

Mass of H2O produced in the reaction = 0.333 mol H2O $\times$ ( 18.015 g / mol ) = 5.998995 g

ANSWER : 6.00 g