For an elementary chemical reaction, , the expression for is:

Engineering

Chemistry

Order of Reaction and Law of Mass Action

Question

For an elementary chemical reaction, $A_{2} ⇌_{k_{2}}^{k_{1}} 2 A$ , the expression for $\frac{d [A]}{dt}$ is:

k₁[A₂] – k_–1[A]²

k₁[A₂] + k_–1[A]²

2k₁[A₂] –2k_–1[A]²

2k₁[A₂] –k_–1[A]²

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Rate of forward reaction, RF = k₁.[A₂]¹ = $\frac{1}{2} (\frac{d [A]}{dt})$

Rate of backward reaction, Rb = k_–1[A]² = $\frac{1}{2} (- \frac{d [A]}{dt})$

so ${(\frac{d [A]}{dt})}_{net}$ = 2k₁[A₂]¹ – 2k_–1[A]²