In a laboratory, 23.5 g of cyclohexane is burned and 5.5 liters of carbon dioxide was obtained ? a) Balance the reaction b) Calculate the reaction yield. d(CO2)= 1.9 g/L
1 Answer
Dec 23, 2017
Explanation:
- Write and balance the equation
#C_6H_12+9O_2->6CO_2+6H_2O# - Find the molar masses of the involved compounds that can be used later for the usual molar conversions.
#C_6H_12=(84g)/(mol)#
#CO_2=(44g)/(mol)# - Given the mass of
#C_6H_12# , per convention, convert it to mole (#eta# ). Knowing the fact as shown above that#1molC_6H_12-=84gC_6H_12# , a conversion factor is obtainable from this relationship; i.e.,
#=23.5cancel(gC_6H_12)xx(1molC_6H_12)/(84cancel(gC_6H_12))#
#=0.2798molC_6H_12# - Then, find the mole of
#CO_2# . Given the relationship#1molC_6H_12-=6molCO_2# from the balanced equation, a factor used for the conversion is obtainable; i.e.,
#=0.2798cancel(molC_6H_12)xx(6molCO_2)/(1cancel(molC_6H_12))#
#=1.6786molCO_2# - Now, find the Theoretical Yield
#(TY)# of this reaction.
#TY=1.6786cancel(molCO_2)xx(44gCO_2)/(1cancel(molCO_2))#
#color(red)(TY=73.86gCO_2# - Given the volume produced in the lab and the density of the
#CO_2# , the Actual Yield#(AY)# can be computed as:
#rho=m/V#
#m=rhoxxV#
#m=(1.9g)/cancel((L))xx5.5cancel(L)#
#color(blue)(m=10.45gCO_2=AY#
