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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) +...

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?

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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 re 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/

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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) +...
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