Question

7. Shown below is the aqueous reaction of KNO2, HCl, and SnCl2. 2 KNO2 (aq) + 6 HCl (aq) + 2 SnCl2 (aq) à 2 SnCl4 (aq) + N2O (g) + 3 H2O (l) + 2 KCl (aq)

a. Is this a redox reaction? If so, which atom was reduced and which atom was oxidized. Support your answer by determining the oxidation states of the relevant atoms.

b. If 50.0 g of KNO2 is consumed in this reaction, how many liters of N2O would be produced at STP?

c. How many grams of SnCl2 would need to react to produce 1.6 L of N2O gas at a pressure of 1.25 atm and a temperature of 320 K?

d. Consider a 250 mL solution of 86 mM KNO2. If all of the KNO2 in this solution is consumed by this reaction, how many moles of water will be produced?

Answer 1

Given recurkion : - a) 13 2 KNO2 (694) + GH4 Ceas + 2 Sncia (09) → 2 Snele coon + N20299 + 3 thale) + 2 kelia! It is redox reaction. - N20 - 200 Oxidation state of Noalan changes from t3 to H. so that it is a reduction half reaction. & inel - mely tree KNOZ Il Oxidation of sn-arem changes from t2 to 44. So that, It is a Oxidation half realian, No. of mole of KNO2 consumed = 50 = 0.59 mole. 85 from equatias, & mol KNO, = 1 mol N20 :. No of mole of N20 prodwed = 0.59x₂ = 0.295 mole :. Volisme of Ngo produced (vt MRT 0.295X0.0821x273.15 P © (V) – 6.61 L No of mole of N20 produesd cm) = ? 125x1.6 0.0871X320 5% 0.076 mole Imole smile = 1 more Noo No. of mole of soills required - 0.076*2 = 0.152 mole Mass of smug required = 0.152 x 169.6 = 28.9 grams,

No. Of male of KNO2 reacted = 0.25%0.086 = 0.0215 mole z mole KNO, = 3 mole Ho. No. of mole of Wats (Hro) foomad = 0.0215 *3/2 0.0323 mole.