What is the value of integrated Rate reaction in zero order reaction ?

Explanation

Consider the general first order reaction
R `to` product
Let [R] is concentration of reactant [R] and K is rate constant for first order reaction. Rate of reaction is directly proportional to concentration of reactant.
k is rate constant.
Rate or reaction proportional to zero power of concentration of R.
Rate = ` (-d[R])/(dt)`
`(d[R])/(dt) = k[R]`
Differential rate equation
`(d[R])/([R]) = -k dt`
`ln [R] = -kt + I " " ...(1)`
when `[R]_0` is Initial concentration of reaction at when `t=0 `
`ln [R]_0 = I " "....(2)`
Putting value of I in equation (2)
`ln [R] =- kt + In [R]_0`
Solving
`ln[R]_0 - ln [R] = kt`
`(ln[R]_0)/([R]) = kt " " {log A - log A = "log" A/B}`
`k = (ln [R]_0)/(t[R]) " " `{ natural `lnx = 2.303 logx`}
`k = (2.303)/(t) " log " ([R]_0)/([R])`