The reactions rate $${N_2}\left( g \right) + 3{H_2}\left( g \right) \to 2N{H_3}\left( g \right)$$      was measured $$\frac{{d\left[ {N{H_3}} \right]}}{{dt}} = 2 \times {10^{ - 4}}\,mol\,{\sec ^{ - 1}}.$$       The rates of reactions expressed in terms of $${N_2}$$  and $${H_2}$$  are:

	Rate in terms of $${N_2}.$$ $$\left( {mol\,{L^{ - 1}}\,{{\sec }^{ - 1}}} \right)$$	Rate in terms of $${H_2}$$ $$\left( {mol\,{L^{ - 1}}\,{{\sec }^{ - 1}}} \right)$$
(a)	$$2 \times {10^{ - 4}}$$	$$2 \times {10^{ - 4}}$$
(b)	$$3 \times {10^{ - 4}}$$	$$1 \times {10^{ - 4}}$$
(c)	$$1 \times {10^{ - 4}}$$	$$3 \times {10^{ - 4}}$$
(d)	$$2 \times {10^{ - 1}}$$	$$2 \times {10^{ - 3}}$$