The theoretical yield will be #"7.48 g"# of carbon dioxide and the reaction's percent yield will be #"93.9%"#.
Start with the balanced chemical equation
#2CO_((g)) + O_(2(g)) -> 2CO_(2(g))#
Notice that you have a #"1:1"# (2:2) mole ratio between carbon monoxide and carbon dioxide - more precise, for every mole of the former that reacts, 1 mole of the latter will be produced.
This is what your theoretical yield will be #-># the number of moles of #CO_2# produced must be equal to the number of moles of #CO# that reacted, assuming in this case that all available moles of #CO# will react.
Determine the number of moles of #CO# by using its molar mass