${\text{3.0 d}}{{\text{m}}^{\text{3}}}$ 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