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In a reversible reaction $A\underset{{{k_2}}}{\overset{{{k_1}}}{\longleftrightarrow}}B,$ the initial concentration of $A$ and  $B$ are $a$ and $b$ and the equilibrium concentration are $(a -x)$ and $(b + x)$ respectively. Express $"x"$ in terms of $k_1, k_2,$ $a$ and $b$

• ✓
  $\frac{{{k_1}a - {k_2}b}}{{{k_1}\, + \,{k_2}}}$
• B
  $\frac{{{k_1}a - {k_2}b}}{{{k_1}\, - \,{k_2}}}$
• C
  $\frac{{{k_1}a - {k_2}b}}{{{k_1}{k_2}}}$
• D
  $\frac{{{k_1}a + {k_2}b}}{{{k_1}\, + \,{k_2}}}$