3) No of mol of KClO3 reacted = 1.115/122.55 = 0.0091
mol
from equation, 2 mol KClO3 = 3 mol O2
No of mol of O2 formed = 0.0091*3/2 = 0.01365 mol
volume of O2 formed(V) = nRT/P
n = 0.01365 mol
R = 0.0821 l.atm.k-1.mol-1
T = 273.15 k (at STP)
P = 1 atm
V = 0.01365*0.0821*273.15/1
= 0.306 L
= 306 ml
4) from equation, 2 mol K = 1 mol H2
No of mol of H2 liberated(n) = PV/RT
P = 1 atm
V = 75.5 ml = 0.0755 L
R = 0.0821 l.atm.k-1.mol-1
T = 273.15 k (at STP)
= 1*0.0755/(0.0821*273.15)
= 0.00337 mol
No of mol of K reacted = 0.00337*2 = 0.00674 mol
mass of K reacted = 0.00674*39.1 = 0.263 g
5)
No of mol of CO2 reacted(n) = PV/RT = 1*15/(0.0821*273.15) = 0.67 mol
No of mol of NH3 taken = 1*10/(0.0821*273.15) = 0.446 mol
from equation, 1 mol CO2 = 1 mol NH3
so that, limiting reactant = NH3
no of mol of NaHCO3 formed = 0.446mol
mass of NaHCO3 formed = 0.446*84 = 37.5 g
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