102 - For the reaction at equilibrium: $2\mathrm{NO(g)} + \mathrm{Br_2(g)} \rightleftharpoons 2\mathrm{NOBr(g)}$, at a certain temperature, 66 g of $\mathrm{NOBr}$, 18 g of $\mathrm{NO}$, and 24 g of $\mathrm{Br_2}$ exist in a 3-liter container. The equilibrium constant at these conditions is fixed, and to reach this equilibrium, 60 percent of the initial amount of $\mathrm{Br_2}$ has been consumed. With how many moles of $\mathrm{Br_2}$ was the reaction started? $$(\mathrm{N{=}14,\ O{=}16,\ Br{=}80\ :\ g{\cdot}mol^{-1}})$$ (1) $0/25\ ,\ 2\cdot0$ (2) $0/375\ ,\ 2\cdot0$ (3) $0/375\ ,\ 0/05$ (4) $0/25\ ,\ 0/05$ \begin{flushright} \framebox{Calculation Space} \end{flushright} %% Page 17
\textbf{102 -} For the reaction at equilibrium: $2\mathrm{NO(g)} + \mathrm{Br_2(g)} \rightleftharpoons 2\mathrm{NOBr(g)}$, at a certain temperature, 66 g of $\mathrm{NOBr}$, 18 g of $\mathrm{NO}$, and 24 g of $\mathrm{Br_2}$ exist in a 3-liter container. The equilibrium constant at these conditions is fixed, and to reach this equilibrium, 60 percent of the initial amount of $\mathrm{Br_2}$ has been consumed. With how many moles of $\mathrm{Br_2}$ was the reaction started?
$$(\mathrm{N{=}14,\ O{=}16,\ Br{=}80\ :\ g{\cdot}mol^{-1}})$$
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(1) $0/25\ ,\ 2\cdot0$ \hspace{1cm} (2) $0/375\ ,\ 2\cdot0$ \hspace{1cm} (3) $0/375\ ,\ 0/05$ \hspace{1cm} (4) $0/25\ ,\ 0/05$
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