Which equation is true to calculate the energy of activation,if the rate of reaction is doubled by increasing temperature from $T_1 \ K$ to $T_2 \ K$?

• A
  $\log_{10} \frac{k_2}{k_1} = \frac{E_a}{2.303R} \left[ \frac{T_2 - T_1}{T_1 T_2} \right]$
• B
  $\log_{10} 2 = \frac{E_a}{2.303R} \left[ \frac{T_2 - T_1}{T_1 T_2} \right]$
• C
  $\log_{10} \frac{k_1}{k_2} = \frac{E_a}{2.303R} \left[ \frac{1}{T_1} - \frac{1}{T_2} \right]$
• D
  $\log_{10} \frac{1}{2} = \frac{E_a}{2.303} \left[ \frac{1}{T_2} - \frac{1}{T_1} \right]$