Give two examples for each of zero order and first order reactions. Write the equations for the rate of reaction in terms of concentration changes of reactants and products for the following ractions.
1) `A(g) +B(g) to C(g) +D(g)`
2) `A(g) to B(g)+C(g)`
3) `A(g) +B(g)to C(g)`

Explanation

Examples of zero order reaction :
1) `2NH_(3(g))(Pt)/(1130K)N_(2(g))+3H_(2(g))`
2) ` 2HI_((g))("gold")/(Delta) H_(2(g))+I_(2(g))`
Examples of first order reaction :
`N_(2)O_(5(g))to N_(2)O_(4(g))+1/2 O_(2(g))`
`SO_(2)Cl_(2(g))to SO_(2(g))+Cl_(2(g))`
1) `A(g) +B(g) to C(g) +D(g)`
Rate ` =-(Delta[A])/(Deltat)=-(Delta[B])/(Deltat) =+(Delta[C])/(Deltat)`
2) `A(g)toB(g) +C(g)`
`(Delta[A])/(Deltat) =+ (Delta[B])/(Deltat) =+(Delta[C])/(Deltat)`
3) `A(g) + B(g) to C(g)`
rate `=-(Delta[A])/(Deltat)=-(Delta[B])/(Deltat) =+(Delta[C])/(Deltat)`