How many grams of potassium chloride are produced if $4\mathrm{.}00g$ of nickel $($III$)$ chloride

are reacted, according to the following unbalanced equation?

$NiC{l}_3+K_{2}C{O}_3-N{i}_2(C{O}_3{)}_3+KCl$

$5\mathrm{.}42g$

$1\mathrm{.}49g$

$10\mathrm{.}8g$

$0\mathrm{.}60g$

$2\mathrm{.}70$gTitanium dioxide is used as a white pigment in paints, rubbers, plastics, and paper.

Titanium dioxide is formed in the following reaction:

$TiC{l}_{4(g)}+O_{2(g)}-*>Ti{O}_{2(s)}+2C{l}_{2(g)}$

If the masses of the products and reactants were accurately measured $($with an equal

number of moles of reactants present$),$ what could we expect?

The masses of the products would outweigh the masses of the reactants.

The masses of the reactants would outweigh the masses of the prodcuts.

The mass of chlorine would be exactly twice the mass of titanium dioxide.

The combined masses of the products would equal the combined masses of the

reactants.