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Using the differential rate equation and rate law, the rate of the reaction in terms of the rate of disappearance of reactant A is

Rate = - d[A]/dt = k[A]^{n}

**Zero order reactions:**

Reactions in which the rate of reaction doesn't depend on the concentration of the reactants are called zero order reactions.

The integrated rate equation for a zero order reaction is,

- d[A]/dt = k

âˆ« d[A] = - k âˆ« dt

[A] = -kt + C

C = Constant of Integration

Initial Concentration [A] = [A]_{o} at t = 0

[A] = -kt + C

[A]_{o} = -k x 0 + C

C = [A]_{o}

[A] = -kt + C

C = [A]_{o}

[A] = -kt + C

[A] = -kt + [A]_{o}

Ex: Photochemical reactions are zero order reactions. Certain enzymatic reactions are also zero order reactions.

_{hv}

H_{2} + Cl_{2 } â†’ 2HCl

_{hv}

6CO_{2} + 6H_{2}O â†’ C_{6}H_{12}O_{6} + 6O_{2}

_{Pt,1130 k}

2NH_{3} â†’ N_{2} + 3H_{2}

^{High Pressure}

_{Î”}

2HI â†’ H_{2} + I_{2}

^{Au}

**First order reactions:**

A reaction in which the rate of reaction is proportional to the first power of the concentration of the reactant is called a first order reaction.

The integrated rate equation for a first order reaction is

- d[A]/dt = k[A]^{n}

- d[A]/dt = k[A]

âˆ« d[A]/[A] = -k âˆ« dt

log_{e}[A] = -kt + C

[A] = [A]_{0}, at t = 0

log_{e}[A]_{0} = -k x 0 + C

C = log_{e}[A]_{0}

log_{e}[A] = -kt + log_{e}[A]_{0}

k = 1/t . log_{e}([A]_{0}/[A])

log_{e} = 2.303 log_{10}

k = 2.303/t log_{10} ([A]_{0}/[A])

Using the differential rate equation and rate law, the rate of the reaction in terms of the rate of disappearance of reactant A is

Rate = - d[A]/dt = k[A]^{n}

**Zero order reactions:**

Reactions in which the rate of reaction doesn't depend on the concentration of the reactants are called zero order reactions.

The integrated rate equation for a zero order reaction is,

- d[A]/dt = k

âˆ« d[A] = - k âˆ« dt

[A] = -kt + C

C = Constant of Integration

Initial Concentration [A] = [A]_{o} at t = 0

[A] = -kt + C

[A]_{o} = -k x 0 + C

C = [A]_{o}

[A] = -kt + C

C = [A]_{o}

[A] = -kt + C

[A] = -kt + [A]_{o}

Ex: Photochemical reactions are zero order reactions. Certain enzymatic reactions are also zero order reactions.

_{hv}

H_{2} + Cl_{2 } â†’ 2HCl

_{hv}

6CO_{2} + 6H_{2}O â†’ C_{6}H_{12}O_{6} + 6O_{2}

_{Pt,1130 k}

2NH_{3} â†’ N_{2} + 3H_{2}

^{High Pressure}

_{Î”}

2HI â†’ H_{2} + I_{2}

^{Au}

**First order reactions:**

A reaction in which the rate of reaction is proportional to the first power of the concentration of the reactant is called a first order reaction.

The integrated rate equation for a first order reaction is

- d[A]/dt = k[A]^{n}

- d[A]/dt = k[A]

âˆ« d[A]/[A] = -k âˆ« dt

log_{e}[A] = -kt + C

[A] = [A]_{0}, at t = 0

log_{e}[A]_{0} = -k x 0 + C

C = log_{e}[A]_{0}

log_{e}[A] = -kt + log_{e}[A]_{0}

k = 1/t . log_{e}([A]_{0}/[A])

log_{e} = 2.303 log_{10}

k = 2.303/t log_{10} ([A]_{0}/[A])