The equilibrium constant for the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$ is $4 \times 10^{-4}$ at $2000 \ K$. In the presence of a catalyst,equilibrium is attained ten times faster. Therefore,the equilibrium constant in the presence of the catalyst at $2000 \ K$ is:

• A
  $40 \times 10^{-4}$
• B
  $4 \times 10^{-4}$
• C
  $4 \times 10^{-3}$
• D
  Difficult to compute without more data