In the reaction , `4A+bBrarrcC+dD`, the rate of disappearance of A andB are 0.064 and `0.08"mol L"^(-1).s^(-1)` , respectively . The rate of formation of C and D are 0.064 and `0.096"mol.L"^(-1).s^(-1)` , respectively . Find the values of b , c and d.

Explanation

The rate of the given reaction is
`(r)=-(1)/(4)(Delta[A])/(Deltat)=-(1)/(b)(Delta[B])/(Deltat)=(1)/(c)(Delta[C])/(Deltat)=(1)/(d)(Delta[D])/(Deltat)`
Given : `-(Delta[A])/(Deltat)=0.064"mol.L"^(-1).s^(-1),(Delta[B])/(Deltat)=0.08"mol.L"^(-1).s^(-1), `
`-(Delta[C])/(Deltat)=0.064"mol.L"^(-1).s^(-1),(Delta[D])/(Deltat)=0.096"mol.L"^(-1).s^(-1),`
`therefore(1)/(4)(-(Delta[A])/(Deltat))=(1)/(b)(-(Delta[B])/(Deltat))" or, "(1)/(4)xx0.064=(1)/(b)xx0.08 " or, "b=5`
`(1)/(4)(-(Delta[A])/(Deltat))=(1)/(c)((Delta[C])/(Deltat))" or, "(1)/(4)xx0.064=(1)/(c)xx0.064 " or, "c=4`
`and(1)/(4)(-(Delta[A])/(Deltat))=(1)/(d)((Delta[D])/(Deltat))" or, "(1)/(4)xx0.064=(1)/(d)xx0.096 " or, "d=6`