Question

50cm³ of carbon(iv)oxide was exploded with 150cm³ of air containing 20% oxygen by volume.which of the reactant was in excess​

Answer 1

Step-by-step explanation:

V(CO) = 50 cm^3 = 50 ml = 0.05 l

V(air) = 150 cm^3 = 150 ml = 0.15 l

V(O2)/V(air) = 20%

_____________________________

2 CO + O2 = 2CO2

n(CO) = V(CO)/V(M) = 0.05/22.4 = 0.0022mol

V(O2)/V(air) = x/150 x=150×0.2 =30 ml=0.03l

n(O2) = V(O2)/V(M) =0.03/22.4 = 0.0013 mol

From the reaction ratio n(CO): n(O2) = 2:1

For explosing 0.0022 mol CO need 0.0011 mol O2. We have 0.0013 mol O2, then , 0.0003 mol O2 is excess.

Answer: O2 was in excess