(Solved):   Shown below is the aqueous reaction of \( \mathrm{KNO}_{2}, \mathrm{HCl} \), and \( \mathr ...

 

Shown below is the aqueous reaction of \( \mathrm{KNO}_{2}, \mathrm{HCl} \), and \( \mathrm{SnCl}_{2} \). \( 2 \mathrm{KNO}_{2}(\mathrm{aq})+6 \mathrm{HCl}(\mathrm{aq})+2 \mathrm{SnCl}_{2}(\mathrm{aq}) \rightarrow 2 \mathrm{SnCl}_{4}(\mathrm{aq})+\mathrm{N}_{2} \mathrm{O}(\mathrm{g})+3 \mathrm{H}_{2} \mathrm{O}(\mathrm{I})+2 \mathrm{KCl}(\mathrm{aq}) \) 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 \( 50.0 \mathrm{~g} \) of \( \mathrm{KNO}_{2} \) is consumed in this reaction, how many liters of \( \mathrm{N}_{2} \mathrm{O} \) would be produced at STP? c. How many grams of \( \mathrm{SnCl}_{2} \) would need to react to produce \( 1.6 \mathrm{~L} \) of \( \mathrm{N}_{2} \mathrm{O} \) gas at a pressure of \( 1.25 \) atm and a temperature of \( 320 \mathrm{~K} \) ? d. Consider a \( 250 \mathrm{~mL} \) solution of \( 86 \mathrm{mM} \mathrm{KNO}_{2} \). If all of the \( \mathrm{KNO}_{2} \) in this solution is consumed by this reaction, how many moles of water will be produced?