\({\text{3.0 d}}{{\text{m}}^{\text{3}}}\) of ethyne, \({{\text{C}}_{\text{2}}}{{\text{H}}_{\text{2}}}\), is mixed with \({\text{3.0 d}}{{\text{m}}^{\text{3}}}\) of hydrogen and ignited. The equation for the reaction that occurs is shown below.

\[{{\text{C}}_{\text{2}}}{{\text{H}}_{\text{2}}}{\text{(g)}} + {\text{2}}{{\text{H}}_{\text{2}}}{\text{(g)}} \to {{\text{C}}_{\text{2}}}{{\text{H}}_{\text{6}}}{\text{(g)}}\]

Assuming the reaction goes to completion and all gas volumes are measured at the same temperature and pressure, what volume of ethane, \({{\text{C}}_{\text{2}}}{{\text{H}}_{\text{6}}}\), in \({\text{d}}{{\text{m}}^{\text{3}}}\), is formed?

A.     1.5

B.     2.0

C.     3.0

D.     6.0

A