In a reaction,$n_1 A + n_2 B \rightarrow m_1 C + m_2 D$,$5 \ M$ solution of reactant $A$ is allowed to react with $3 \ M$ solution of reactant $B$. After $5 \ s$,the concentration of $A$ was found to be $4 \ M$. The rate of decomposition of $A$ and the rate of formation of $D$ are respectively $:-$

• A
  $0.2 \ M \ sec^{-1} ; \left(\frac{m_2}{m_1} \times 0.2\right) \ M \ sec^{-1}$
• B
  $0.2 \ M \ sec^{-1} ; \left(\frac{n_2}{m_2} \times 0.2\right) \ M \ sec^{-1}$
• C
  $0.1 \ M \ sec^{-1} ; \left(\frac{m_2}{n_1} \times 0.2\right) \ M \ sec^{-1}$
• D
  $0.2 \ M \ sec^{-1} ; \left(\frac{m_2}{n_1} \times 0.2\right) \ M \ sec^{-1}$