Question

According to the following reaction, how many grams of a mmonium nitrite are necessary to form 0.880 moles water? ammonium nitrite (aq)nitrogen (g) + water (I) grams ammonium nitrite Retry Entire Group 9 more group attempts remaining Submit Answer According to the following reaction, how many moles of phosphoric acid will be formed upon the complete reaction of 23.6 grams of perchloric acid (HCIO4) with excess tetraphosphorus decaoxide? perchloric acid (HCIO4) (aq) + tetraphosphorus decaoxide (s) phosphoric acid (aq) + dichlorine heptaoxide () moles phosphoric acid

Answer 1

1)

Given, the chemical reaction,

ammonium nitrite (aq)  $\rightarrow$ nitrogen(g) + water(l)

NH₄NO₂(aq) $\rightarrow$ N₂(g) + 2H₂O(l)

Also given,

Moles of water = 0.880 mol

The mole ratio between ammonium nitrite and nitrogen is 1:2. Using the given moles of water and the mole ratio to calculate the number of moles of ammonium nitrite,

= 0.880 mol of H₂O x ( 1 mol of NH₄NO₂ / 2 mol of H₂O)

= 0.44 mol of NH₄NO₂

Converting the number of moles to grams,

= 0.44 mol of NH₄NO₂ x (64.06 g / 1mol)

= 28.2 g of NH₄NO₂

2) Given,

The reaction,

perchloric acid(HClO₄)(aq) + tetraphosphorus decaoxide(s) $\rightarrow$ phosphoric acid(aq) + dichlorine heptoxide(l)

12HClO₄(aq) + P₄O₁₀(s) $\rightarrow$ 4H₃PO₄(aq) + 6Cl₂O₇(l)

Also given,

Mass of HClO₄ = 23.6 grams

Calculating the number of moles of HClO₄ from the given mass,

= 23.6 g of HClO₄ x ( 1 mol /100.46 g)

= 0.2349 mol of HClO₄

Now, from the balanced reaction, the mole ratio between HClO₄ and H₃PO₄ is 12: 4,

Using the calculated moles of HClO₄ and the mole ratio, calculating the number of moles of phosphoric acid,

= 0.2349 mol of HClO₄ x ( 4 mol of H₃PO₄ / 12 mol of HClO₄)

= 0.0783 mol of H₃PO₄ will be produced