Given the reactions at $500 \ K$:
$(i) \ H_{2(g)} + 1/2 O_{2(g)} \rightleftharpoons H_2O_{(g)}$,$K_c = 2.4 \times 10^{47}$
$(ii) \ H_2O_{(g)} \rightleftharpoons H_{2(g)} + 1/2 O_{2(g)}$,$K_c = 4.1 \times 10^{-48}$
What does the magnitude of $K_c$ indicate about the formation of the product in reaction $(i)$?

• A
  The product is highly stable and formed in large amounts.
• B
  The product is unstable and decomposes rapidly.
• C
  The reaction does not proceed to form the product.
• D
  The reaction is at equilibrium with equal amounts of reactants and products.